Calculating the Partial Pressure of Hydrogen

Oct 13, 2025 by recoveryshake.com 58 views

Introduction

In a mixture of gases, each gas exerts a partial pressure that is proportional to its mole fraction in the mixture. The partial pressure of a gas can be calculated using the formula: $\frac{P_2}{P_T}=\frac{n_2}{n_T}$ , where $P_2$ is the partial pressure of the gas, $P_T$ is the total pressure of the mixture, $n_2$ is the number of moles of the gas, and $n_T$ is the total number of moles in the mixture.

Calculating the Partial Pressure of Hydrogen

Given that the container holds 6.4 moles of gas and hydrogen gas makes up $$25%$$ of the total moles, we can calculate the number of moles of hydrogen gas as follows:

$n_2 = 0.25 \times n_T = 0.25 \times 6.4 = 1.6$ moles

Now, we can use the formula $\frac{P_2}{P_T}=\frac{n_2}{n_T}$ to calculate the partial pressure of hydrogen:

$\frac{P_2}{1.24} = \frac{1.6}{6.4}$

Solving for Partial Pressure

To solve for $P_2$ , we can multiply both sides of the equation by 1.24:

$P_2 = \frac{1.6}{6.4} \times 1.24$

$P_2 = 0.3125 \times 1.24$

$P_2 = 0.388$

Rounding the Answer

Rounding the answer to two decimal places, we get:

$P_2 = 0.39$ atm

However, this is not among the given options. Let's re-evaluate the calculation:

$P_2 = \frac{1.6}{6.4} \times 1.24$

$P_2 = 0.25 \times 1.24$

$P_2 = 0.31$ atm

Conclusion

The partial pressure of hydrogen in the container is 0.31 atm.

Discussion

The partial pressure of a gas in a mixture is an important concept in chemistry, particularly in the study of gas mixtures and their behavior. The formula $\frac{P_2}{P_T}=\frac{n_2}{n_T}$ provides a simple and effective way to calculate the partial pressure of a gas in a mixture. In this problem, we used this formula to calculate the partial pressure of hydrogen in a container holding 6.4 moles of gas, with hydrogen making up $$25%$$ of the total moles. The result shows that the partial pressure of hydrogen is 0.31 atm.

Key Takeaways

The partial pressure of a gas in a mixture is proportional to its mole fraction in the mixture.
The formula $\frac{P_2}{P_T}=\frac{n_2}{n_T}$ can be used to calculate the partial pressure of a gas in a mixture.
The partial pressure of a gas can be used to determine its behavior in a mixture.

References

Chemistry textbook, chapter 5: Gas Mixtures
Online resources: Khan Academy, Chemistry LibreTexts

Introduction

Calculating the Partial Pressure of Hydrogen

Given that the container holds 6.4 moles of gas and hydrogen gas makes up $$25%$$ of the total moles, we can calculate the number of moles of hydrogen gas as follows:

$n_2 = 0.25 \times n_T = 0.25 \times 6.4 = 1.6$ moles

Now, we can use the formula $\frac{P_2}{P_T}=\frac{n_2}{n_T}$ to calculate the partial pressure of hydrogen:

$\frac{P_2}{1.24} = \frac{1.6}{6.4}$

Solving for Partial Pressure

To solve for $P_2$ , we can multiply both sides of the equation by 1.24:

$P_2 = \frac{1.6}{6.4} \times 1.24$

$P_2 = 0.3125 \times 1.24$

$P_2 = 0.388$

Rounding the Answer

Rounding the answer to two decimal places, we get:

$P_2 = 0.39$ atm

However, this is not among the given options. Let's re-evaluate the calculation:

$P_2 = \frac{1.6}{6.4} \times 1.24$

$P_2 = 0.25 \times 1.24$

$P_2 = 0.31$ atm

Conclusion

The partial pressure of hydrogen in the container is 0.31 atm.

Discussion

Key Takeaways

The partial pressure of a gas in a mixture is proportional to its mole fraction in the mixture.
The formula $\frac{P_2}{P_T}=\frac{n_2}{n_T}$ can be used to calculate the partial pressure of a gas in a mixture.
The partial pressure of a gas can be used to determine its behavior in a mixture.

References

Chemistry textbook, chapter 5: Gas Mixtures
Online resources: Khan Academy, Chemistry LibreTexts

Q&A

Q: What is the partial pressure of a gas in a mixture?

A: The partial pressure of a gas in a mixture is the pressure that the gas would exert if it were the only gas present in the mixture.

Q: How is the partial pressure of a gas calculated?

A: The partial pressure of a gas can be calculated using the formula: $\frac{P_2}{P_T}=\frac{n_2}{n_T}$ , where $P_2$ is the partial pressure of the gas, $P_T$ is the total pressure of the mixture, $n_2$ is the number of moles of the gas, and $n_T$ is the total number of moles in the mixture.

Q: What is the mole fraction of a gas in a mixture?

A: The mole fraction of a gas in a mixture is the ratio of the number of moles of the gas to the total number of moles in the mixture.

Q: How does the partial pressure of a gas change with temperature?

A: The partial pressure of a gas increases with temperature, according to Charles' Law.

Q: What is the difference between partial pressure and total pressure?

A: The partial pressure of a gas is the pressure that the gas would exert if it were the only gas present in the mixture, while the total pressure is the sum of the partial pressures of all the gases in the mixture.

Q: Can the partial pressure of a gas be greater than the total pressure?

A: No, the partial pressure of a gas cannot be greater than the total pressure.

Q: How is the partial pressure of a gas affected by the addition of another gas to the mixture?

A: The partial pressure of a gas decreases with the addition of another gas to the mixture, according to Dalton's Law of Partial Pressures.

Q: What is the significance of partial pressure in chemical reactions?

A: Partial pressure is an important factor in chemical reactions, particularly in the study of gas-phase reactions.

Q: Can the partial pressure of a gas be measured directly?

A: No, the partial pressure of a gas cannot be measured directly. It must be calculated using the formula: $\frac{P_2}{P_T}=\frac{n_2}{n_T}$ .

Q: What is the unit of measurement for partial pressure?

A: The unit of measurement for partial pressure is typically atmospheres (atm) or pascals (Pa).

Q: How does the partial pressure of a gas change with volume?

A: The partial pressure of a gas decreases with an increase in volume, according to Boyle's Law.

Q: Can the partial pressure of a gas be affected by the presence of a catalyst?

A: Yes, the partial pressure of a gas can be affected by the presence of a catalyst.

Q: What is the relationship between partial pressure and chemical equilibrium?

A: The partial pressure of a gas is related to chemical equilibrium, particularly in the study of gas-phase reactions.

Q: Can the partial pressure of a gas be used to determine the rate of a chemical reaction?

A: Yes, the partial pressure of a gas can be used to determine the rate of a chemical reaction.

Q: What is the significance of partial pressure in the study of gas mixtures?

A: Partial pressure is an important concept in the study of gas mixtures, particularly in the calculation of the partial pressures of individual gases in a mixture.

Q: Can the partial pressure of a gas be affected by the presence of a solvent?

A: Yes, the partial pressure of a gas can be affected by the presence of a solvent.

Q: What is the relationship between partial pressure and the mole fraction of a gas?

A: The partial pressure of a gas is directly proportional to its mole fraction in the mixture.

Q: Can the partial pressure of a gas be used to determine the concentration of a gas in a mixture?

A: Yes, the partial pressure of a gas can be used to determine the concentration of a gas in a mixture.

Q: What is the significance of partial pressure in the study of chemical kinetics?

A: Partial pressure is an important concept in the study of chemical kinetics, particularly in the calculation of reaction rates and the determination of the order of a reaction.

Q: Can the partial pressure of a gas be affected by the presence of a surface?

A: Yes, the partial pressure of a gas can be affected by the presence of a surface.

Q: What is the relationship between partial pressure and the temperature of a gas?

A: The partial pressure of a gas increases with temperature, according to Charles' Law.

Q: Can the partial pressure of a gas be used to determine the pressure of a gas in a mixture?

A: Yes, the partial pressure of a gas can be used to determine the pressure of a gas in a mixture.

Q: What is the significance of partial pressure in the study of gas-phase reactions?

A: Partial pressure is an important concept in the study of gas-phase reactions, particularly in the calculation of reaction rates and the determination of the order of a reaction.

Q: Can the partial pressure of a gas be affected by the presence of a magnetic field?

A: No, the partial pressure of a gas is not affected by the presence of a magnetic field.

Q: What is the relationship between partial pressure and the volume of a gas?

A: The partial pressure of a gas decreases with an increase in volume, according to Boyle's Law.

Q: Can the partial pressure of a gas be used to determine the concentration of a gas in a mixture?

A: Yes, the partial pressure of a gas can be used to determine the concentration of a gas in a mixture.

Q: What is the significance of partial pressure in the study of chemical thermodynamics?

A: Partial pressure is an important concept in the study of chemical thermodynamics, particularly in the calculation of reaction free energies and the determination of the spontaneity of a reaction.