A Scientist Is Examining A Mixture Of Nitrogen, Hydrogen, And Ammonia. The Individual Pressures Exerted By Nitrogen And Hydrogen Are 0.26 Atm And 0.28 Atm, Respectively. If The Total Pressure Is 0.90 Atm, What Is The Partial Pressure Of Ammonia?Use The
Understanding Partial Pressure
In chemistry, partial pressure refers to the pressure exerted by a specific gas in a mixture of gases. The concept of partial pressure is crucial in understanding the behavior of gases in various systems, including industrial processes and environmental phenomena. In this article, we will explore the calculation of partial pressure using the ideal gas law and apply it to a mixture of nitrogen, hydrogen, and ammonia.
The Ideal Gas Law
The ideal gas law is a fundamental principle in chemistry that describes the behavior of gases under various conditions. The law is expressed as:
PV = nRT
Where:
- P is the pressure of the gas
- V is the volume of the gas
- n is the number of moles of the gas
- R is the gas constant
- T is the temperature of the gas
Partial Pressure of Nitrogen and Hydrogen
Given that the individual pressures exerted by nitrogen and hydrogen are 0.26 atm and 0.28 atm, respectively, we can calculate the partial pressure of each gas using the ideal gas law. However, since the partial pressure of a gas is directly proportional to its mole fraction in the mixture, we can use the following equation:
P_partial = P_total * (n_gas / n_total)
Where:
- P_partial is the partial pressure of the gas
- P_total is the total pressure of the mixture
- n_gas is the number of moles of the gas
- n_total is the total number of moles in the mixture
Calculating Partial Pressure of Nitrogen
Using the given values, we can calculate the partial pressure of nitrogen as follows:
P_N2 = 0.90 atm * (0.26 / 0.54)
P_N2 = 0.40 atm
Calculating Partial Pressure of Hydrogen
Similarly, we can calculate the partial pressure of hydrogen as follows:
P_H2 = 0.90 atm * (0.28 / 0.54)
P_H2 = 0.45 atm
Calculating Partial Pressure of Ammonia
Now that we have calculated the partial pressures of nitrogen and hydrogen, we can calculate the partial pressure of ammonia using the following equation:
P_NH3 = P_total - P_N2 - P_H2
P_NH3 = 0.90 atm - 0.40 atm - 0.45 atm
P_NH3 = 0.05 atm
Conclusion
In conclusion, the partial pressure of ammonia in a mixture of nitrogen, hydrogen, and ammonia can be calculated using the ideal gas law and the concept of partial pressure. By understanding the behavior of gases in mixtures, we can better design and optimize various industrial processes and environmental systems.
References
- Ideal Gas Law: PV = nRT
- Partial Pressure: P_partial = P_total * (n_gas / n_total)
Further Reading
- Gas Mixtures: Understanding the behavior of gases in mixtures is crucial in various industrial processes and environmental phenomena.
- Partial Pressure: The concept of partial pressure is essential in understanding the behavior of gases in mixtures.
- Ideal Gas Law: The ideal gas law is a fundamental principle in chemistry that describes the behavior of gases under various conditions.
Frequently Asked Questions (FAQs) about Partial Pressure ===========================================================
Q: What is partial pressure?
A: Partial pressure is the pressure exerted by a specific gas in a mixture of gases. It is a measure of the contribution of a particular gas to the total pressure of the mixture.
Q: How is partial pressure calculated?
A: Partial pressure can be calculated using the ideal gas law and the concept of partial pressure. The equation for calculating partial pressure is:
P_partial = P_total * (n_gas / n_total)
Where:
- P_partial is the partial pressure of the gas
- P_total is the total pressure of the mixture
- n_gas is the number of moles of the gas
- n_total is the total number of moles in the mixture
Q: What is the difference between partial pressure and total pressure?
A: The total pressure of a mixture is the sum of the partial pressures of all the gases present in the mixture. Partial pressure, on the other hand, is the pressure exerted by a specific gas in the mixture.
Q: How is partial pressure related to mole fraction?
A: Partial pressure is directly proportional to the mole fraction of a gas in a mixture. The mole fraction of a gas is the ratio of the number of moles of the gas to the total number of moles in the mixture.
Q: Can partial pressure be greater than total pressure?
A: No, partial pressure cannot be greater than total pressure. The partial pressure of a gas is always less than or equal to the total pressure of the mixture.
Q: What is the significance of partial pressure in real-world applications?
A: Partial pressure plays a crucial role in various real-world applications, including:
- Industrial processes: Partial pressure is used to design and optimize industrial processes such as chemical reactions, distillation, and absorption.
- Environmental science: Partial pressure is used to understand and predict the behavior of gases in the atmosphere, oceans, and soil.
- Medical applications: Partial pressure is used to understand the behavior of gases in the human body, including the lungs, blood, and tissues.
Q: How can I calculate partial pressure using the ideal gas law?
A: To calculate partial pressure using the ideal gas law, you need to know the following:
- P_total: The total pressure of the mixture
- n_gas: The number of moles of the gas
- n_total: The total number of moles in the mixture
- R: The gas constant
- T: The temperature of the gas
You can then use the equation:
PV = nRT
to calculate the partial pressure of the gas.
Q: What are some common mistakes to avoid when calculating partial pressure?
A: Some common mistakes to avoid when calculating partial pressure include:
- Incorrectly calculating mole fraction: Make sure to calculate the mole fraction correctly using the number of moles of the gas and the total number of moles in the mixture.
- Using incorrect values for P_total: Make sure to use the correct value for the total pressure of the mixture.
- Using incorrect values for n_gas and n_total: Make sure to use the correct values for the number of moles of the gas and the total number of moles in the mixture.
By avoiding these common mistakes, you can ensure accurate calculations of partial pressure.