A Container Holds 6.4 Moles Of Gas. Hydrogen Gas Makes Up $25\%$ Of The Total Moles In The Container. If The Total Pressure Is 1.24 Atm, What Is The Partial Pressure Of Hydrogen?Use $\frac{P_a}{P_T}=\frac{n_a}{n_T}$.A. 0.31 Atm B.

Understanding Partial Pressure

In a mixture of gases, each gas contributes to the overall pressure of the mixture. The partial pressure of a gas is the pressure that the gas would exert if it were the only gas present in the container. The partial pressure of a gas can be calculated using the formula:

$$\frac{P_a}{P_T}=\frac{n_a}{n_T}$$

where $P_a$ is the partial pressure of the gas, $P_T$ is the total pressure of the mixture, $n_a$ is the number of moles of the gas, and $n_T$ is the total number of moles in the mixture.

Calculating Partial Pressure of Hydrogen Gas

In this problem, we are given that a container holds 6.4 moles of gas, and hydrogen gas makes up 25% of the total moles in the container. We are also given that the total pressure is 1.24 atm. We need to calculate the partial pressure of hydrogen gas.

First, let's calculate the number of moles of hydrogen gas in the container. Since hydrogen gas makes up 25% of the total moles, we can calculate the number of moles of hydrogen gas as follows:

$$n_{H_2} = 0.25 \times n_T$$

$$n_{H_2} = 0.25 \times 6.4$$

$$n_{H_2} = 1.6$$

Now that we have the number of moles of hydrogen gas, we can use the formula to calculate the partial pressure of hydrogen gas:

$$\frac{P_{H_2}}{P_T}=\frac{n_{H_2}}{n_T}$$

$$\frac{P_{H_2}}{1.24}=\frac{1.6}{6.4}$$

$$P_{H_2} = \frac{1.6}{6.4} \times 1.24$$

$$P_{H_2} = 0.3125 \times 1.24$$

$$P_{H_2} = 0.388$$

However, the answer is not in the options. Let's recheck the calculation.

$$P_{H_2} = \frac{1.6}{6.4} \times 1.24$$

$$P_{H_2} = 0.25 \times 1.24$$

$$P_{H_2} = 0.31$$

Therefore, the partial pressure of hydrogen gas in the mixture is 0.31 atm.

Conclusion

In this problem, we calculated the partial pressure of hydrogen gas in a mixture using the formula:

$$\frac{P_a}{P_T}=\frac{n_a}{n_T}$$

We were given that a container holds 6.4 moles of gas, and hydrogen gas makes up 25% of the total moles in the container. We also knew that the total pressure is 1.24 atm. We calculated the number of moles of hydrogen gas and used the formula to calculate the partial pressure of hydrogen gas. The partial pressure of hydrogen gas in the mixture is 0.31 atm.

References

• Chemistry textbook
• Online resources

Related Topics

• Partial pressure of a gas
• Mixture of gases
• Ideal gas law

Frequently Asked Questions

• What is partial pressure?
• How do you calculate partial pressure?
• What is the formula for partial pressure?

Answers

• Partial pressure is the pressure that a gas would exert if it were the only gas present in the container.
• The formula for partial pressure is: $\frac{P_a}{P_T}=\frac{n_a}{n_T}$
• The formula for partial pressure is: $\frac{P_a}{P_T}=\frac{n_a}{n_T}$
  Partial Pressure of a Gas: Frequently Asked Questions =====================================================

Q: What is partial pressure?

A: Partial pressure is the pressure that a gas would exert if it were the only gas present in the container. It is a measure of the contribution of a particular gas to the overall pressure of a mixture of gases.

Q: How do you calculate partial pressure?

A: The partial pressure of a gas can be calculated using the formula:

$$\frac{P_a}{P_T}=\frac{n_a}{n_T}$$

where $P_a$ is the partial pressure of the gas, $P_T$ is the total pressure of the mixture, $n_a$ is the number of moles of the gas, and $n_T$ is the total number of moles in the mixture.

Q: What is the formula for partial pressure?

A: The formula for partial pressure is:

$$\frac{P_a}{P_T}=\frac{n_a}{n_T}$$

Q: How do you calculate the number of moles of a gas in a mixture?

A: To calculate the number of moles of a gas in a mixture, you need to know the total number of moles in the mixture and the percentage of the gas in the mixture. You can calculate the number of moles of the gas as follows:

$$n_a = \frac{\text{percentage of gas}}{100} \times n_T$$

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

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

Q: Can you give an example of how to calculate partial pressure?

A: Yes, let's say we have a container that holds 6.4 moles of gas, and hydrogen gas makes up 25% of the total moles in the container. We are also given that the total pressure is 1.24 atm. We can calculate the partial pressure of hydrogen gas as follows:

$$n_{H_2} = 0.25 \times n_T$$

$$n_{H_2} = 0.25 \times 6.4$$

$$n_{H_2} = 1.6$$

$$\frac{P_{H_2}}{P_T}=\frac{n_{H_2}}{n_T}$$

$$\frac{P_{H_2}}{1.24}=\frac{1.6}{6.4}$$

$$P_{H_2} = \frac{1.6}{6.4} \times 1.24$$

$$P_{H_2} = 0.25 \times 1.24$$

$$P_{H_2} = 0.31$$

Therefore, the partial pressure of hydrogen gas in the mixture is 0.31 atm.

Q: What are some common applications of partial pressure?

A: Partial pressure is an important concept in chemistry and physics, and it has many practical applications. Some common applications of partial pressure include:

• Calculating the pressure of a gas in a mixture
• Determining the composition of a mixture of gases
• Understanding the behavior of gases in a mixture
• Calculating the pressure of a gas in a container

Q: What are some common mistakes to avoid when calculating partial pressure?

A: When calculating partial pressure, it's easy to make mistakes. Here are some common mistakes to avoid:

• Not using the correct formula for partial pressure
• Not knowing the total number of moles in the mixture
• Not knowing the percentage of the gas in the mixture
• Not converting units correctly
• Not checking units before calculating partial pressure

Conclusion

In this article, we have discussed the concept of partial pressure and how to calculate it. We have also answered some frequently asked questions about partial pressure and provided examples of how to calculate it. We hope that this article has been helpful in understanding the concept of partial pressure and how to apply it in real-world situations.