Calculating the Partial Pressure of SO2Cl2

Oct 13, 2025 by miodeya.com 135 views

Introduction

In a gas-phase reaction, equilibrium partial pressures play a crucial role in understanding the behavior of the system. The reaction SO2Cl2(g)⇌SO2(g)+Cl2(g) is a classic example of a reversible reaction, where the equilibrium constant (Kp) is given as 2.91×103 at 298 K. In this article, we will explore the partial pressures of the reactants and products in a mixture at equilibrium, with the partial pressure of SO2 being 133 torr and that of Cl2 being 275 torr.

Understanding the Equilibrium Constant (Kp)

The equilibrium constant (Kp) is a measure of the ratio of the partial pressures of the products to the partial pressures of the reactants at equilibrium. Mathematically, it can be expressed as:

Kp = (P_SO2 × P_Cl2) / P_SO2Cl2

where P_SO2, P_Cl2, and P_SO2Cl2 are the partial pressures of SO2, Cl2, and SO2Cl2, respectively.

Given Partial Pressures

The partial pressure of SO2 is given as 133 torr, and that of Cl2 is given as 275 torr. We need to find the partial pressure of SO2Cl2 in this mixture.

Calculating the Partial Pressure of SO2Cl2

To find the partial pressure of SO2Cl2, we can rearrange the equation for Kp as follows:

P_SO2Cl2 = (P_SO2 × P_Cl2) / Kp

Substituting the given values, we get:

P_SO2Cl2 = (133 torr × 275 torr) / (2.91×103)

Performing the Calculation

Now, let's perform the calculation to find the partial pressure of SO2Cl2:

P_SO2Cl2 = (133 torr × 275 torr) / (2.91×103) = 36,525 torr^2 / 2.91×103 = 12.58 torr

Conclusion

In conclusion, the partial pressure of SO2Cl2 in this mixture is 12.58 torr. This value can be used to understand the behavior of the system at equilibrium and to make predictions about the partial pressures of the reactants and products.

References

[1] Atkins, P. W., & de Paula, J. (2010). Physical chemistry (9th ed.). Oxford University Press.
[2] Levine, I. N. (2012). Physical chemistry (6th ed.). McGraw-Hill.

Additional Information

The equilibrium constant (Kp) is a measure of the ratio of the partial pressures of the products to the partial pressures of the reactants at equilibrium.
The partial pressure of a gas is a measure of the pressure exerted by that gas in a mixture.
The reaction SO2Cl2(g)⇌SO2(g)+Cl2(g) is a reversible reaction, where the equilibrium constant (Kp) is given as 2.91×103 at 298 K.
Frequently Asked Questions (FAQs) about Equilibrium Partial Pressures ====================================================================

Q: What is the equilibrium constant (Kp) and how is it related to the partial pressures of the reactants and products?

A: The equilibrium constant (Kp) is a measure of the ratio of the partial pressures of the products to the partial pressures of the reactants at equilibrium. Mathematically, it can be expressed as:

Kp = (P_SO2 × P_Cl2) / P_SO2Cl2

where P_SO2, P_Cl2, and P_SO2Cl2 are the partial pressures of SO2, Cl2, and SO2Cl2, respectively.

Q: How do I calculate the partial pressure of a gas in a mixture at equilibrium?

A: To calculate the partial pressure of a gas in a mixture at equilibrium, you need to know the partial pressures of the other gases in the mixture and the equilibrium constant (Kp). You can use the following equation:

P_gas = (P_other_gases × Kp) / (P_other_gases - 1)

where P_gas is the partial pressure of the gas you want to calculate, P_other_gases is the partial pressure of the other gases in the mixture, and Kp is the equilibrium constant.

Q: What is the difference between the equilibrium constant (Kp) and the equilibrium constant (Kc)?

A: The equilibrium constant (Kp) is a measure of the ratio of the partial pressures of the products to the partial pressures of the reactants at equilibrium, while the equilibrium constant (Kc) is a measure of the ratio of the concentrations of the products to the concentrations of the reactants at equilibrium.

Q: How do I determine the equilibrium constant (Kp) for a reaction?

A: The equilibrium constant (Kp) can be determined experimentally by measuring the partial pressures of the reactants and products at equilibrium. Alternatively, it can be calculated using thermodynamic data, such as the enthalpy and entropy changes for the reaction.

Q: What is the significance of the equilibrium constant (Kp) in a reaction?

A: The equilibrium constant (Kp) is a measure of the favorability of a reaction. A large value of Kp indicates that the reaction favors the products, while a small value of Kp indicates that the reaction favors the reactants.

Q: Can the equilibrium constant (Kp) be used to predict the direction of a reaction?

A: Yes, the equilibrium constant (Kp) can be used to predict the direction of a reaction. If the value of Kp is greater than 1, the reaction favors the products, and if the value of Kp is less than 1, the reaction favors the reactants.

Q: How do I calculate the partial pressure of a gas in a mixture at equilibrium using the equilibrium constant (Kp)?

A: To calculate the partial pressure of a gas in a mixture at equilibrium using the equilibrium constant (Kp), you can use the following equation:

P_gas = (P_other_gases × Kp) / (P_other_gases + Kp)

where P_gas is the partial pressure of the gas you want to calculate, P_other_gases is the partial pressure of the other gases in the mixture, and Kp is the equilibrium constant.

Q: What is the relationship between the equilibrium constant (Kp) and the partial pressures of the reactants and products?

A: The equilibrium constant (Kp) is a measure of the ratio of the partial pressures of the products to the partial pressures of the reactants at equilibrium. Mathematically, it can be expressed as:

Kp = (P_SO2 × P_Cl2) / P_SO2Cl2

where P_SO2, P_Cl2, and P_SO2Cl2 are the partial pressures of SO2, Cl2, and SO2Cl2, respectively.

Q: Can the equilibrium constant (Kp) be used to predict the equilibrium partial pressures of a reaction?

A: Yes, the equilibrium constant (Kp) can be used to predict the equilibrium partial pressures of a reaction. By knowing the equilibrium constant (Kp) and the partial pressures of the reactants and products, you can calculate the equilibrium partial pressures of the reaction.

Q: How do I use the equilibrium constant (Kp) to calculate the equilibrium partial pressures of a reaction?

A: To use the equilibrium constant (Kp) to calculate the equilibrium partial pressures of a reaction, you need to know the partial pressures of the reactants and products at equilibrium and the equilibrium constant (Kp). You can use the following equation:

P_equilibrium = (P_reactants × Kp) / (P_reactants + Kp)

where P_equilibrium is the equilibrium partial pressure of the reaction, P_reactants is the partial pressure of the reactants, and Kp is the equilibrium constant.

Q: What is the significance of the equilibrium partial pressures in a reaction?

A: The equilibrium partial pressures are a measure of the concentrations of the reactants and products at equilibrium. They can be used to predict the direction of a reaction and to calculate the equilibrium constant (Kp).

Q: Can the equilibrium partial pressures be used to predict the direction of a reaction?

A: Yes, the equilibrium partial pressures can be used to predict the direction of a reaction. If the partial pressure of the products is greater than the partial pressure of the reactants, the reaction favors the products, and if the partial pressure of the reactants is greater than the partial pressure of the products, the reaction favors the reactants.