If a clot were made up of a mass of proteins, what change in the proteins led to the formation of a clot?

Answer:

The correct answer is a. Chloride

Explanation:

GABAA receptors, is an ionotropic receptor that controls most of the central nervous system inhibitory transmission. GABAA receptors exist as ionotropic ligand-gated ion channel and selectively conduct chloride ions Cl⁻ when activated by GABA through its pore where by the flow of Cl⁻ depends on the internal voltage of the cell and the resting potential. Cl⁻ will flow in a cell if the internal voltage is more than resting potential which is -75 mV. When the internal voltage is less than resting potential, Cl⁻ will transit out of the cell

Final answer:

The ion responsible for the changes when GABA is released onto Cell Y with a resting membrane potential at -55mV and only GABAA receptors present is chloride, which causes an inhibitory postsynaptic potential.

Explanation:

When Cell X fires an action potential and releases GABA onto Cell Y, and only GABAA receptors are present on the postsynaptic membrane which is at rest at -55mV, the ion responsible for the observed changes is chloride. The binding of GABA to GABAA receptors increases the influx of chloride ions into the postsynaptic cell, making the inside of the cell more negative. This increase in negative charge pulls the membrane potential towards the equilibrium potential of chloride which is -65 mV and creates an inhibitory postsynaptic potential (IPSP), thus inhibiting the neuron from firing an action potential.

Answer:

The correct answer is "False".

Explanation:

The Elizabethan Era was a period of England's history that corresponds to  the reign of Queen Elizabeth I (1558–1603). The Elizabethan Era is considered a golden age of England's history, and part of the Renaissance Era (1300-1600). The Elizabethan view of life changed drastically from  the characteristic Medieval view of life. During Medieval times life was seen with a religiously perspective only, while during The Elizabethan Era more people start to view life with a scientific perspective.

THE ANSWER IS FALSE!

Answer:

To regulate the gas pressure in the lighter tank and avoid build-up of pressure.  

Explanation:

We soak the lighter in the water bath to achieve uniform heating and reduce the fire hazard inherent in direct heating methods, ensuring a safer laboratory environment.

We soak the lighter in the water bath to ensure uniform heating of the reaction mixture with less fire hazard. Direct heating on a Bunsen burner or hot plate can cause uneven temperatures and increased risks of fire or overheating. A water bath is especially beneficial when a chemical reaction must be heated for a certain time to occur. It provides a stable and consistent heat source, which is safer and can prevent accidents in the lab. By using a water bath, we also prevent the lighter from getting excessively hot, which could cause it to malfunction or pose a safety risk.

Answer:

The final temperature of the mixture is 21.4°C

Explanation:

Specific heat capacity of water = 1 cal/g°c

Heat loss by water  = 77.1 g X 1 cal/g°c X 50.9°c = 3924.39 Cal

Latent heat of fusion of ice = 79.7 g⁻¹

Heat required to melt ice at 0°c= 22.5 g X 79.7 g⁻¹ = 1793.25 Cal

Heat gained by ice from water at a higher temperature, T°c = 22.5 X 1 X T  

= 22.5T

Also heat lost by water = 77.1  X 1  X (50.9-T)cal

By calorimetric principle

Heat lost by a hot body = heat gained by a cold body

77.1  X 1  X (50.9-T) = 22.5T + 1793.25

3924.39 -77.1T = 22.5T + 1793.25

99.6T = 3924.39 - 1793.25

T = 2131.14/99.6

T = 21.4°C

Therefore, the final temperature of the mixture is 21.4°C

Answer:

The first question is water vapor.

Explanation:

Water vapor is not a green house gas. Clouds are made of water vapor.

Answer:

Explanation:

The same charges repel each other while opposite charges attract each other. During electron-electron interaction repulsion take palace because the electron has negative charges. Nucleus has positive charges so the interaction between two nucleus results in the form of repulsion. When interaction takes place between nucleus and electron then attraction takes place between nucleus and electrons due to opposite charges.

          The formation of a bond that takes place due to the sharing of the electrons is known as a covalent bond and thus the covalent molecule is formed.

The forces between two atoms is the result of electron-electron repulsion, nucleus-nucleus repulsion, and nucleus-electron attraction. At the point of equilibrium, the attractive forces balance the repulsive forces. The most stable configuration of atoms exists at the point of minimum potential energy, when the atoms bond covalently and a covalent bond forms.

The force of attraction between atoms leads to the formation of covalent bonds. The force of attraction is defined by the magnitude of oppositely charged ions bonded with one another. There are various forces of attraction in between molecules which are studied in chemistry. These are:

Answer:

The answer to this question is 3.  Kinetic energy decreases as temperature decreases.

Explanation:

The average Kinetic energy is given by

[tex]K = \frac{3}{2}[/tex] × [tex]K_{B}[/tex] × T where

K = The average molecular kinetic energy of the gas (J)

[tex]K_{B}[/tex] = Boltzmann's constant (1.38×[tex]10^{-23}[/tex] J/K)

T = Temperature of the gas in Kelvin (k)

When the temperature of a given mass of gas drops average kinetic energy of the molecules goes down and the average molecular speed decreases.  The lower kinetic energy  which is the energy of motion of the molecules indicates lower speed of the molecules.

Note that, the kinetic energy and average speed are related by the following formula

KE = [tex]\frac{1}{2}[/tex]×m×v²

Where KE = Kinetic energy in Joules (J)

v = the velocity in m/s and

m = the mass of the molecule in Kg

Answer:

Answer is C

Explanation:

Edge 2020

Answer:

The answer to your question is   C₃H₆O

Explanation:

Data

mass of sample = 23.2 g

mass of carbon dioxide = 52.8 g

mass of water = 21.6 g

empirical formula = ?

Process

1.- Calculate the mass and moles of carbon

                       44 g of CO₂ ---------------  12 g of C

                        52.8 g          ---------------  x

                        x = (52.8 x 12)/44

                        x = 633.6/44

                        x = 14.4 g of C

                        12 g of C ------------------  1 mol

                        14.4 g of C ---------------   x

                         x = (14.4 x 1)/(12)

                         x = 1.2 moles of C

2.- Calculate the grams and moles of Hydrogen

                         18 g of H₂O ---------------  2 g of H

                         21.6 g of H₂O -------------  x

                          x = (21.6 x 2) / 18

                         x = 2.4 g of H

                         1 g of H -------------------- 1 mol of H

                         2.4 g of H -----------------  x

                          x = (2.4 x 1)/1

                          x = 2.4 moles of H

3.- Calculate the grams and moles of Oxygen

Mass of Oxygen = 23.2 - 14.4 - 2.4

                           = 6.4 g

                         16 g of O ----------------  1 mol

                          6.4 g of O --------------  x

                          x = (6.4 x 1)/16

                          x = 0.4 moles of Oxygen

4.- Divide by the lowest number of moles

Carbon = 1.2 / 0.4 = 3

Hydrogen = 2.4/ 0.4 = 6

Oxygen = 0.4 / 0.4 = 1

5.- Write the empirical formula

                                C₃H₆O

Final answer:

To find the empirical formula of a compound from its combustion products, convert the masses of carbon dioxide and water to moles to determine the moles of carbon, hydrogen, and oxygen in the compound. Calculating these mole ratios leads to determining that the empirical formula of the compound is C3H6O.

Explanation:

To determine the empirical formula of the compound given its combustion products, begin by converting the mass of carbon dioxide (CO2) and water (H2O) to moles. This reveals the moles of carbon and hydrogen in the original compound. Since oxygen is also part of the compound, calculate its moles by subtraction from the total mass of the original compound.

Convert 52.8 g of CO2 to moles: (52.8 g) / (44.01 g/mol) = 1.2 mol of C.Convert 21.6 g of H2O to moles: (21.6 g) / (18.015 g/mol) = 1.2 mol of H2, or 2.4 mol of H.Calculate moles of oxygen in the compound: Subtract the mass of C and H in the original compound from its total mass. Mass of C from CO2 = 1.2 mol × 12 g/mol = 14.4 g; Mass of H from H2O = 2.4 mol × 1 g/mol = 2.4 g. Total mass of C and H = 14.4 g + 2.4 g = 16.8 g; Mass of O = 23.2 g (total mass) - 16.8 g = 6.4 g, which is (6.4 g) / (16 g/mol) = 0.4 mol of O.To find the empirical formula, divide each mole value by the smallest number of moles: C=1.2/0.4, H=2.4/0.4, O=0.4/0.4, giving a ratio of C: 3 H: 6 O: 1. Therefore, the empirical formula is C3H6O.

Answer:

Molecular formula of the compound is C₃H₆O

Explanation:

Firstly let's determine the moles of the vapor (gas) with the Ideal Gases Law, so it can give us the molar mass with the mass and afterwards we can work with the percent composition.

Pressure . Volume = moles . Ideal Constant Gases . Temperature in K

Temperature in K = T°C + 273 → 150°C + 273 = 423K

P . V = n . R . T

n = (P .V) / (R. T)

n = 1 atm . 0.5L / (0.082 . 423K)

n =  0.0144 moles

These are the moles for 0.8365 g, so let's determine the molar mass

Molar mass (g/mol) = 0.8365 g / 0.0144 mol → 58.02 g/mol

Percent composition means:

100 g of compound have 62.04 g of C

100 g of compound have 10.41 g of H

100 g of compound have 27.54 g of O

Let's make the rule of three:

100 g of compound have __ 62.04 g of C __ 10.41 g of H __ 27.54 g of O

The 58.02 g of compound must have:

(58.02 g . 62.04 g) / 100 g  = 36 g of C

(58.02 g . 10.41 g) / 100 g  = 6 g of H

(58.02 g . 27.54 g) / 100 g  = 16 g of O

Let's find out the moles of each

Mass / Molar mass

36 g / 12 g/mol = 3 C

6 g / 1 g/mol = 6 H

16g / 16 g/mol = 1 O

The molecular formula of the given compound is C₃H₆O. The molecular formula can be determined by finding the ratio of each element in the compound.

It can be determined by finding the ratio of each element in the compound.

First, calculate the moles of the compound from the ideal gas formula,

[tex]n = \dfrac {1 {\rm\ atm \times 0.5L} }{(0.082 \times 423{\rm \ K})}\\\\n = 0.0144 \rm \ moles[/tex]

Then calculate the molar mass of the compound,

[tex]m = {\rm \dfrac {0.8365 \ g }{0.0144 \ mol}} \\\\m = 58.02 \rm \ g/mol[/tex]

Then calculate the mass of individual elements in the 58.02 g of compound:

[tex]\text{ Mass of Carbon} = \dfrac {58.02 {\rm \ g} \times 62.04 {\rm \ g}}{100 {\rm \ g}}\\ \text{ Mass of Carbon} = 36 \rm \ g[/tex]

[tex]\text{ Mass of Hydrogen } = \dfrac {58.02 {\rm \ g} \times 10.14 {\rm \ g}}{100 {\rm \ g}}\\ \text{ Mass of Hydrogen } = 6 \rm \ g[/tex]

[tex]\text{ Mass of Oxygen } = \dfrac {58.02 {\rm \ g} \times 27.54 {\rm \ g}}{100 {\rm \ g}}\\ \text{ Mass of Oxygen } = 16 \rm \ g[/tex]

Now find the moles of each element, we get

3 moles of Carbon

6 moles of Hydrogen

1 mole of Oxygen

Therefore, the molecular formula of the given compound is C₃H₆O.

Learn more about the molecular formula,

https://brainly.com/question/14666499

Answer : The molar enthalpy of reaction is, 33.3 KJ/mole

Explanation :

First we have to calculate the mass of water.

As we know that the density of water is 1 g/ml. So, the mass of water will be:

The volume of water = [tex]60ml+60ml=120ml[/tex]

Now we have to calculate the heat absorbed during the reaction.

[tex]q=m\times c\times (\Delta T)[/tex]

where,

q = heat absorbed = ?

[tex]c[/tex] = specific heat of water = [tex]4.18J/g^oC[/tex]

m = mass of water = 120 g

[tex]\Delta T[/tex] = change in temperature = [tex]5.18^oC[/tex]

Now put all the given values in the above formula, we get:

[tex]q=120g\times 4.18J/g^oC\times (5.18)^oC[/tex]

[tex]q=2598.288J=2.60KJ[/tex]

Now we have to calculate the molar enthalpy of reaction.

[tex]\Delta H=\frac{q}{n}[/tex]

where,

[tex]\Delta H[/tex] = enthalpy of neutralization = ?

q = heat released = 2.60 KJ

n = number of moles =

[tex]\Delta H=\frac{2.60KJ}{0.078mole}=33.3KJ/mole[/tex]

Therefore, the molar enthalpy of reaction is, 33.3 KJ/mole

The molar enthalpy of reaction of HCl(aq) is calculated to be approximately -33.28 kJ/mol, using calorimetry principles and the given data.

To calculate the molar enthalpy of reaction of HCl(aq), we use the concept of calorimetry and the given temperature change. The provided reaction is a neutralization reaction where HCl reacts with AgNO₃ to form AgCl(s) and HNO₃(aq)

Firstly, we need to calculate the total heat (q) released during the reaction. This can be done by using the formula:

q = mcΔT

where m is the mass of the solution, c is the specific heat capacity of water (assumed to be 4.18 J/g°C as the specific heat capacity is not provided), and ΔT is the change in temperature. The mass (m) of the solution is the sum of the volumes of AgNO₃(aq) and HCl(aq) solutions, assuming a density of 1 g/mL for both solutions:

m = volume of AgNO₃ + volume of HCl = 60 mL + 60 mL

= 120 mL

= 120 g

Substitute the values into the formula to calculate q:

q = (120 g)(4.18 J/g°C)(5.18°C)q

= 2596.416 J

= 2.596 kJ

Next, calculate the number of moles of HCl which is equal to the moles of AgNO₃ since they react in a 1:1 ratio:

Moles of HCl = Volume of HCl × Concentration of HCl

= 0.060 L × 1.30 mol/L

= 0.078 mol

Finally, divide the total heat energy by the number of moles to find the molar enthalpy (ΔH) of the reaction per mole of HCl:

ΔH = q / moles of HClΔH

= 2.596 kJ / 0.078 mol

= -33.28 kJ/mol

Therefore, the molar enthalpy of reaction of HCl(aq) is approximately -33.28 kJ/mol.

Answer:

23 kPa = Partial pressure O₂

Explanation:

In a mixture of gases, the sum of partial pressure of each gas that contains the mixture = Total pressure

Total pressure = Partial pressure N₂ + Partial pressure CO₂ + Partial pressure O₂

95 kPa = 48 kPa + 24 kPa + Partial pressure O₂

95 kPa - 48 kPa - 24 kPa = Partial pressure O₂

23 kPa = Partial pressure O₂

Final answer:

The final temperature of the mixture will be 15.44°C.

Explanation:

In this problem, we can use the principle of conservation of energy to find the final temperature of the mixture. The heat gained by the ice cubes is equal to the heat lost by the water.

To find the heat gained by the ice cubes, we can use the formula:

Q = m × c × ΔT

where Q is the heat gained, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.

Since the ice cubes are at 0°C, the heat gained is:

Q = 4 × (53.5 g) × (4.184 J/(g°C)) × (0°C - T-f)

where T-f is the final temperature.

To find the heat lost by the water, we can use the formula:

Q = m × c × ΔT

where Q is the heat lost, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.

Since the water is at 75°C, the heat lost is:

Q = (115 g) × (4.184 J/(g°C)) × (T-f - 75°C)

Since no heat is lost to the surroundings, the heat gained by the ice cubes is equal to the heat lost by the water. Setting the two equations equal to each other, we can solve for T-f:

4 × (53.5 g) × (4.184 J/(g°C)) × (0°C - T-f) = (115 g) × (4.184 J/(g°C)) × (T-f - 75°C)

Simplifying the equation gives:

14.0816 × T-f = 496.82 - 18.0714 × T-f

32.1526 × T-f = 496.82

T-f = 15.44°C

Answer:

The answer to your question is below

Explanation:

The specific heat is a physical property equal to the amount of heat necessary to increase the temperature of 1 gram of a substance by one degree celsius.

The lower the specific heat, the lower the amount of heat to increase the temperature 1°C, the higher the specific heat, the higher the amount of heat necessary to increase the temperature by 1°C.

The specific heat of copper is 0.093 cal/g°C

The specific heat of water is 1 cal/g°C.

That is why is necessary more heat to warm water.

More energy to increase the temperature of 100 grams of liquid water by one degree Celsius than it does 100 grams of copper metal due to higher specific heat.

Specific heat refers to the amount of heat needed to raise the temperature of 1 gram of a substance by 1 degree Celsius. Water has a high specific heat which means it takes more energy to increase the temperature of water compared to other substances like metals.

So we can conclude that more energy is needed to increase the temperature of 100 grams of liquid water by one degree Celsius than copper metal because of higher specific heat of water.

Learn more about metal here: https://brainly.com/question/4701542

Answer:

the velocity of the tomato will be  v  = u + gt

kinetic energy = 9.64 h

Explanation:

At that time, let the initial speed be u.

The acceleration due to gravity be g

The final velocity will be given as v = u + at

but a = g = 9.81 m/s² [acceleration due to gravity]

so the final velocity will be given as v = u + at

Let the potential energy be Ep

Before landing the ground, 93.8 % of the potential energy will be converted to kinetic energy. Therefore, the calculation will be as follows:

Ep = mgh

Kinetic energy Ek = 1/2mv²

But, Ek = 0.938 Ep

            = 0.983 × gh

            = 9.64 h

where h is the height of the object from the ground.

Answer:

9 atm is the total pressure of the combined gases.

Explanation:

According to the Dalton's law of partial pressure , the total pressure of the gas is equal to the sum of the partial pressure of the mixture of gasses.

[tex]P_T=p_{1}+p_{2}....p_{n}[/tex]

where,

[tex]P_T[/tex] = total pressure =

[tex]p_{1}[/tex] = partial pressure of gas-1

[tex]p_{2}[/tex] = partial pressure of gas -2

[tex]p_{n}[/tex] = partial pressure of nth gas

We have :

Pressure of the oxygen gas in flask before mixing = 8 atm

Pressure of the hydrogen gas in flask before mixing = 1 atm

Partial pressure of oxygen gas after mixing = [tex]p_1=8 atm[/tex]

Partial pressure of hydrogen gas after mixing = [tex]p_2=1 atm[/tex]

Total pressure of the mixture : P

[tex]P=P_1+P_2[/tex] (Dalton's law of partial pressure)

[tex]P=8 atm+1 atm=9 atm[/tex]

9 atm is the total pressure of the combined gases.

Answer:

D

Explanation:

Sound waves are D) Mechanical and Longitudinal

Explanation:

In physics, waves are classified into two types:

Moreover, waves are further classified into:

Sound waves are oscillations of a medium that occurs back-and forth along the direction of propagation of the wave. Therefore, they are mechanical (they need a medium to propagate) and longitudinal. So the correct answer is

D) Mechanical and Longitudinal

Learn more about sound waves:

brainly.com/question/4899681

#LearnwithBrainly

Final answer:

Sound waves are best described as Mechanical and Longitudinal waves, as they need a medium to travel and have disturbances parallel to the direction of propagation in fluids.

Explanation:

The set of terms that best describes sound waves is Mechanical and Longitudinal. Sound waves require a medium to travel through, which makes them mechanical waves. Furthermore, in fluids such as air and water, sound waves are longitudinal because their disturbances (variations in pressure) are parallel to the direction of propagation. In solids, sound waves can be both longitudinal and transverse; however, in the context of your question which seems to imply a generic scenario, the focus is often on sound in fluids.

Answer: (a) NH3 + H20 ⇔ NH4⁺ + OH⁻ Kb =  [tex]\frac{ [NH4][OH]}{[NH3]}[/tex]

(b) CN⁻ + H20 ⇔ HCN⁺ + OH⁻ Kb =  [tex]\frac{ [HCN][OH]}{[CN]}[/tex]

(c) C5H5N + H20 ⇔ C5H5NH⁺ + OH⁻ Kb = [tex]\frac{[C5H5NH][OH]}{ [C5H5N]}[/tex]

(d) C6H5NH2 + H20 ⇔ C6H5NH3⁺ + OH⁻ Kb = [tex]\frac{[C6H5NH3][OH]}{[C6H5NH2] }[/tex]

Explanation: There are ways to calculate the strength of acids and bases. The pH is more commom but there is pKa, pKb, Ka and Kb. Ka and Kb are the dissociation constant for acids and bases, respectively.

Using the balanced equation of dissociation, Kb is calculated by dividing the concentration of the products with the concentration of the reagent.

The reactions and Kb equilibrium expressions for NH₃, CN⁻, pyridine (C₅H₅N), and aniline (C₆H₅NH₂) as bases in water are summarized including all necessary chemical equations and equilibrium expressions.

The following reactions and corresponding Kb equilibrium expressions for NH₃, CN⁻, pyridine (C₅H₅N), and aniline (C₆H₅NH₂) acting as bases in water are as follows:

Answer:

the initial amount of calcium oxide will decrease as the system moves toward equilibrium

Explanation:

The question should have this variable:

a) 655g CaCO3, 95.0g CaO, P(CO2) = 2.55atm

The reaction formula of dry ice, calcium oxide and calcium carbonate should be:

CaCO3 (s) --> CaO(s) + CO2(g)

With Kp = 1.04 at 900 degrees C

in this tank, only CO2(g) is in gaseous form. The amount of gas will determine the pressure of the tank. When the tank heated, its temperature rise and will also rise the pressure. When pressure higher than Kp, the equilibrium will shift toward side with less gas.

There is only one gas in the reaction, so Kp=  P(CO2)

Since P(CO2) is 2.55 atm and its higher than Kp(1.04), the equilibrium will shift to the left. Since the reaction direction to the left, the amount of calcium carbonate will increase while carbon dioxide and calcium oxide will decrease.

The initial amount of calcium oxide will decrease because  the system moves toward equilibrium

In this tank, only CO2(g) should be in gaseous form. The amount of gas will measure the pressure of the tank. At the time When the tank is heated, its temperature should be increased due to this the pressure is also increased.  

Since P(CO2) is 2.55 atm and it's more than Kp(1.04), the equilibrium should shift to the left. The reaction shifted to the left, the amount of calcium carbonate will increase while on the other hand, carbon dioxide and calcium oxide will decrease.

learn more about volume here: https://brainly.com/question/22083481

Answer:

The molarity is 1.33×10^-7M

Explanation:

15ppb = 15g of chlorobenzene/10^9g of solution × 1 mole of chlorobenzene/112.6g × 1g of solution/mL = 1.33×10^-10mol/mL × 1000mL/1L = 1.33×10^-7mol/L

The molarity of a chlorobenzene solution with a concentration of 15 ppb is calculated by first converting the ppb measurement to mass per volume and then using the molar mass to find the number of moles per liter, resulting in a molarity of 1.33 × 10⁻⁷ M.

To calculate the molarity of chlorobenzene in a solution with a concentration of 15 ppb, we first need to convert this concentration into a mass-volume relationship. Since 1 ppb is equivalent to 1 µg/L, 15 ppb is equal to 15 µg/L, which is the same as 0.015 mg/L.

Using the molar mass of chlorobenzene, which is 112.6 g/mol, we can convert this mass into moles using the following equation:

The solution has a concentration of 15 µg/L, which is equal to 0.015 mg/L or 0.000015 g/L. So the amount of moles of chlorobenzene is:

Number of moles = 0.000015 g / 112.6 g/mol = 1.33 × 10-7 moles/L

Therefore, the molarity of the chlorobenzene solution is 1.33 × 10-7 M.

Final answer:

To calculate the percent composition of aluminum and magnesium in the sample, we use stoichiometry. Moles of hydrogen gas produced help to establish moles of the metals reacting, but without complete reaction equations for the alloy, or more data, a definitive calculation cannot be provided.

Explanation:

To calculate the percentage by mass of aluminum and magnesium in the sample, we need to perform a few stoichiometric calculations based on the reaction of the alloy with hydrochloric acid and the production of hydrogen gas. The typical reactions for aluminum and magnesium with hydrochloric acid are:

Using the molar mass of hydrogen (1.008 g/mol), we can calculate the moles of hydrogen gas produced using the equation:

moles H₂ = 0.998 g / (2 * 1.008 g/mol) = 0.495 moles

The mole ratio of Al to H₂ in the reaction is 2:3, and for Mg to H₂ is 1:1. We can calculate the mass of aluminum or magnesium that would produce 0.495 moles of hydrogen.

For aluminum:

moles Al = (2/3) * moles H₂ = (2/3) * 0.495 = 0.330 moles

For magnesium:

moles Mg = moles H₂ = 0.495 moles

Now, we calculate the mass:

mass Al = moles Al * atomic mass Al = 0.330 moles * 26.98 g/mol = 8.904 g

mass Mg = moles Mg * atomic mass Mg = 0.495 moles * 24.31 g/mol = 12.033 g

These numbers are hypothetical maximums if the sample was 100% Al or Mg, and do not add up to 9.87 g. Therefore, we need to set up a system of equations considering the total mass of the alloy and the mass of hydrogen produced to find the exact mass of Al and Mg in the sample. This requires more information or a different approach that accounts for the actual reaction stoichiometry with the alloy sample, which isn't provided here.

The alloy consists of: 62.2% aluminium, 37.8% magnesium

To calculate the percentage by mass of each metal (aluminium and magnesium) in the alloy, we need to use the stoichiometry of their reactions with hydrochloric acid and the information given about the mass of the hydrogen gas produced.

Step 1: Write the balanced chemical equations for the reactions

For aluminium:

[tex]\[ 2\text{Al} + 6\text{HCl} \rightarrow 2\text{AlCl}_3 + 3\text{H}_2 \][/tex]

For magnesium:

[tex]\[ \text{Mg} + 2\text{HCl} \rightarrow \text{MgCl}_2 + \text{H}_2 \][/tex]

Step 2: Determine the moles of hydrogen gas produced

The molar mass of hydrogen gas [tex](\(\text{H}_2\))[/tex] is:

[tex]\[ \text{Molar mass of H}_2 = 2 \times 1.008 = 2.016 \, \text{g/mol} \][/tex]

The number of moles of hydrogen gas produced is:

[tex]\[ \text{Moles of H}_2 = \frac{0.998 \, \text{g}}{2.016 \, \text{g/mol}} \]\[ \text{Moles of H}_2 = 0.495 \, \text{mol} \][/tex]

Step 3: Relate moles of hydrogen gas to moles of metals

Let  x be the mass of aluminium and  y be the mass of magnesium in the alloy.

From the reactions:

- Aluminium produces 3 moles of [tex]\(\text{H}_2\)[/tex] per 2 moles of [tex]\(\text{Al}\)[/tex]:

[tex]\[ 2\text{Al} \rightarrow 3\text{H}_2 \]\[ \frac{3}{2} \text{moles of H}_2 \text{ per mole of Al} \]\[ 1 \text{ mole of Al} \rightarrow \frac{3}{2} \text{ moles of H}_2 \][/tex]

- Magnesium produces 1 mole of [tex]\(\text{H}_2\) per mole of \(\text{Mg}\):[/tex]

[tex]\[ \text{Mg} \rightarrow \text{H}_2 \]\[ 1 \text{ mole of Mg} \rightarrow 1 \text{ mole of H}_2 \][/tex]

Thus, the moles of hydrogen gas produced by aluminium and magnesium are:

[tex]\[ \text{Moles of H}_2 \text{ from Al} = \frac{3}{2} \times \frac{x}{26.98} \]\[ \text{Moles of H}_2 \text{ from Mg} = \frac{y}{24.305} \][/tex]

The total moles of hydrogen gas produced:

[tex]\[ \frac{3}{2} \times \frac{x}{26.98} + \frac{y}{24.305} = 0.495 \][/tex]

Step 4: Set up the mass equation for the alloy

The total mass of the alloy is:

[tex]\[ x + y = 9.87 \, \text{g} \][/tex]

Step 5: Solve the system of equations

We have two equations:

[tex]1. \[ \frac{3}{2} \times \frac{x}{26.98} + \frac{y}{24.305} = 0.495 \]\\[/tex]

2.  x + y = 9.87

Let's solve these equations step by step.

First, express  y  in terms of x  from the second equation:

[tex]\[ y = 9.87 - x \][/tex]

Substitute this into the first equation:

[tex]\[ \frac{3}{2} \times \frac{x}{26.98} + \frac{9.87 - x}{24.305} = 0.495 \][/tex]

Simplify and solve for x :

[tex]\[ \frac{3x}{2 \times 26.98} + \frac{9.87 - x}{24.305} = 0.495 \]\[ \frac{3x}{53.96} + \frac{9.87 - x}{24.305} = 0.495 \]\[ \frac{3x}{53.96} + \frac{9.87}{24.305} - \frac{x}{24.305} = 0.495 \]\[ \frac{3x}{53.96} - \frac{x}{24.305} = 0.495 - \frac{9.87}{24.305} \][/tex]

Calculate the constant term:

[tex]\[ 0.495 - \frac{9.87}{24.305} = 0.495 - 0.406 = 0.089 \][/tex]

Combine the \( x \)-terms:

[tex]\[ \frac{3x}{53.96} - \frac{x}{24.305} = 0.089 \]\[ x \left( \frac{3}{53.96} - \frac{1}{24.305} \right) = 0.089 \][/tex]

Calculate the coefficient of \( x \):

[tex]\[ \frac{3}{53.96} = 0.0556 \]\[ \frac{1}{24.305} = 0.0411 \]\[ 0.0556 - 0.0411 = 0.0145 \][/tex]

Now, solve for x :

[tex]\[ x \times 0.0145 = 0.089 \]\[ x = \frac{0.089}{0.0145} \]\[ x = 6.14 \, \text{g} \][/tex]

Now, find y :

[tex]\[ y = 9.87 - x \]\[ y = 9.87 - 6.14 \]\[ y = 3.73 \, \text{g} \][/tex]

Step 6: Calculate the percentage by mass of each metal

[tex]\[ \% \, \text{Al} = \frac{6.14 \, \text{g}}{9.87 \, \text{g}} \times 100 = 62.2\% \]\[ \% \, \text{Mg} = \frac{3.73 \, \text{g}}{9.87 \, \text{g}} \times 100 = 37.8\% \][/tex]

Answer:

The right answer to this question is no, all of the liquid will not evaporate, there will be 8.61 ×10⁻⁴ moles or 6.22×10⁻² grams left in the container

At equilibrium the pressure in the container will be the vapor pressure of liquid pentane which is = 100. mm Hg

Explanation:

To solve this we list the known values as follows

vapor pressure of liquid pentane = 100 mmHg = 13.33 KPa

Temperature T = 260 K

Volume of container = 350 mL = 0.00035 m³

The number of moles of liquid pentane = n

The universal gas constant = R = 8.314 J/(mol·K)

Thus From the ideal gas equation PV = nRT →

Thus plugging in the values in the above equateion we have

n = [tex]\frac{PV}{RT} = \frac{(13330)(0.00035)}{(8.314)(260)}[/tex] = 2.16×10⁻³ moles

Hence the number of moles in 0.218 g sample of liquid   pentane C₅H₁₂ with molar mass = 72.15 g/mol = 0.218/72.15 = 3.02×10⁻³ moles

Hence the number of moles present in the sample placed in the closed evacuated container = 3.02×10⁻³ moles

However number of moles to completely evaporate at 100 mmHg and 260 K is 2.16×10⁻³ moles hence, 3.02×10⁻³ moles - 2.16×10⁻³ moles,  or 8.61 ×10⁻⁴ moles will be left in the container

converting the value in moles to mass we have number of moles, n = mass/(molar mass)

Therefore the mass = number of moles × molar mass = 8.61 ×10⁻⁴ × 72.15 = 6.22 × 10⁻² grams left in the container

The pressure in the container at equilibrium will be vapor pressure of liquid pentane C₅H₁₂, or 100. mm Hg

In the described closed system, all of the liquid pentane will evaporate due to the vapor pressure. The final pressure when equilibrium is reached will be the vapor pressure, which is 100.0 mm Hg.

The subject of the question is the vapor pressure of pentane, C5H12, which is a concept from Chemistry.

The given vapor pressure is 100.0 mm Hg at 260 K. In this closed system the liquid and vapor will come to equilibrium at the given temperature, at which point the vapor pressure will be equal to the given 100.0 mm Hg.

The sample mass of 0.218 g doesn't exceed the amount needed for evaporation at the equilibrium pressure. Therefore, all of the liquid pentane will evaporate.

The final pressure in the container when equilibrium is reached will be the vapor pressure, which is 100.0 mm Hg.

https://brainly.com/question/34135527

#SPJ11

Answer: 0.147

Explanation:

[tex]K_p[/tex] is the constant of a certain reaction at equilibrium.

For the given chemical reaction:

     [tex]NH_4HS(s)\rightleftharpoons NH_3(g)+H_2S(g)[/tex]

at t= 0       0                                           0               0

at eqm                                                   p                p

Total pressure = p+p = 0.766 atm

2p= 0.766 atm

p= 0.383 atm

The expression of [tex]K_p[/tex] for above equation follows:

[tex]K_p={p_{NH_3}\times p_{H_2S}}[/tex]

We are given:

[tex]K_p={0.383\times 0.383[/tex]

[tex]K_p=0.147[/tex]

Thus [tex]K_{eq}[/tex] at this temperature is 0.147

Answer:

calculate the molecular formula of a compound with the empirical formula CH2O and a molar mass of 150g/mol

the molecular formula is [tex]C_{5} H_{10}O_{5}[/tex]

The molecular formula of a compound is the formula comprising of the constituent elements chemical symbols each of which carries the number of atoms of that element present in a molecule of the compound appearing in the smallest whole number ratio to other eatoms present in the compound

Explanation:

The masses of the constitent element is determined forst from which the number of moles is then calculated by dividing the mass by the molar mass then then each calculated molar mass value is divided by the smallest  number of moles calculated from the previous step so the value calculated is then rounded up to the nearest whole number giving the ratios of the moles of the elements in the compound which represents the subscripts in the empirical formula of the compound.

If the subscrips are in fractions, then multiply each of them by the same number to derive the smallest whole number factor, that is if the calculated formula contains a facor of 0.5, multiply by 2

Mass pf Carbon  = 12g

mass of Hydrogen = 1g

molar mass of oxygen - 16g

Total mass of CH2O = 30g

Therefore dividing molar mass by empirical formula mass = 150g/30g = 5

Hence our factor is 5

multiplying each subscript of the empirical formula by 5 gives

C5H10O5 hence the molecular formula is [tex]C_{5} H_{10}O_{5}[/tex]

Answer: The [tex]\Delta H^o_{rxn}[/tex] for the reaction is -162.5 kJ/mol

Explanation:

Hess’s law of constant heat summation states that the amount of heat absorbed or evolved in a given chemical equation remains the same whether the process occurs in one step or several steps.

According to this law, the chemical equation is treated as ordinary algebraic expressions and can be added or subtracted to yield the required equation. This means that the enthalpy change of the overall reaction is equal to the sum of the enthalpy changes of the intermediate reactions.

The given chemical reaction follows:

[tex]O_3(g)+Cl(g)\rightarrow ClO(g)+O_2[/tex]      [tex]\Delta H^o_{rxn}=?[/tex]

The intermediate balanced chemical reaction are:

(1) [tex]ClO(g)+O_3(g)\rightarrow Cl(g)+2O_2(g)[/tex]    [tex]\Delta H_1=-122.8kJ/mol[/tex]

(2) [tex]2O_3(g)\rightarrow 3O_2(g)[/tex]     [tex]\Delta H_2=-285.3kJ/mol[/tex]

The expression for enthalpy of the reaction follows:

[tex]\Delta H^o_{rxn}=[1\times (-\Delta H_1)]+[1\times \Delta H_2][/tex]

Putting values in above equation, we get:

[tex]\Delta H^o_{rxn}=[(1\times (-(-122.8))+(1\times (-285.3))=-162.5kJ/mol[/tex]

Hence, the [tex]\Delta H^o_{rxn}[/tex] for the reaction is -162.5 kJ/mol

Answer : The rate law for the overall reaction is, [tex]Rate=k[NO]^2[H_2][/tex]

Explanation :

Rate law : It is defined as the expression which expresses the rate of the reaction in terms of molar concentration of the reactants with each term raised to the power their stoichiometric coefficient of that reactant in the balanced chemical equation.

As we are given the mechanism for the reaction :

Step 1 : [tex]2NO+H_2\rightarrow N_2+H_2O_2[/tex]    (slow)

Step 2 : [tex]H_2O_2+H_2\rightarrow 2H_2O[/tex]     (fast)

Overall reaction : [tex]2NO+2H_2\rightarrow N_2+2H_2O[/tex]

The rate law expression for overall reaction should be in terms of [tex]NO\text{ and }H_2[/tex].

As we know that the slow step is the rate determining step. So,

The slow step reaction is,

[tex]2NO+H_2\rightarrow N_2+H_2O_2[/tex]

The expression of rate law for this reaction will be,

[tex]Rate=k[NO]^2[H_2][/tex]

Hence, the rate law for the overall reaction is, [tex]Rate=k[NO]^2[H_2][/tex]

Answer:

formula for NO2 is nitrogen dioxide

Answer:

Critical Point

Explanation:

You can no longer distinguish a liquid from a gas when a object hits it's critical point.

Answer:

5.6 × 10⁻¹⁷ J

Explanation:

We know that the work done by an electric field, E on an electric charge, q moving a distance, d is W = qEdcosθ. From above, q = 3.2 × 10⁻¹⁹ C, d = 20 cm = 2 × 10⁻² m, E = V/d = 175V /2 × 10⁻² m = 8750 V/m and θ = 0 since the α particle moves in the same direction as the electric field. So W = qEdcosθ = 3.2 × 10⁻¹⁹ C × 8750 V/m × 2 × 10⁻² m × cos0  = 5.6 × 10⁻¹⁷ J. We know that the work done by the electric field on the charge W = ΔK the change in kinetic energy of the charge. So, W = 1/2m(v₂² - v₁²) where v₁ = initial velocity and v₂ = final velocity. Since the charge is at rest at the positive plate, v₁ = 0. So, W = 1/2mv₂² = K which is the kinetic energy of the particle after moving the distance of 20 cm between the plates. So K = W = 5.6 × 10⁻¹⁷ J

Answer:

2

Explanation:

A careful look at CO2, reveals that CO2 contains:

1 atom of C

2 atoms of O.

Answer:

2

Explanation:

i just took the test

No I don't think it works that way. What you could do is drink one energy drink, wait 5 hours and then drink another.

Answer:

10 hrs of energy

Explanation:

these bottles hold energy for 5hrs so if it is double you have double the time of energy