Consider the reaction: SO 2 Cl 2 (g) ⇌ SO 2 (g) + Cl 2 (g) K p = 2.91⨉10 3 at 298 K In a reaction at equilibrium, the partial pressure of SO 2 is 137 torr and that of Cl 2 is 285 torr. What is the partial pressure of SO 2 Cl 2 in this mixture?

Hello everyone today. We are being given the following problem and asked to solve for it. So it says the equilibrium constant K. P. For the oxidation of nitric oxide is 1152 at 1 50 degrees Celsius. Were then given the following chemical reaction In that reaction mixture at equilibrium oxygen has a partial pressure of .345 atmospheres. While the partial pressure of nitrogen dioxide is .225 atmospheres were then asked to calculate the partial pressure of nitric oxide at equilibrium. So the first thing we want to do does he want to calculate, we want to write out our K. P. For the expression below. So R. K. P. It's going to be equal to the pressures of our products over reactivates. And so putting this together, We have our pressure of our only product which is nitrogen dioxide in 02. And since there is a two coefficient we're going to make this exponent into a. two and our denominator we have to react. It's present. We have nitric oxide and so we have the pressure of N. O. Nitric oxide and that has a two coefficient as well. So we're going to give that an exponent of two. And lastly we're going to multiply the second reactant from by the first one which is just molecular oxygen. And so we have our K. P. Expression below. We also were given a partial pressure of oxygen and the partial pressure of pressure of nitrogen dioxide. And so ultimately we want to find the partial pressure of nitric oxide. So we're gonna label that X. And so Plugging our values in to this reaction that we just found we have our K. P. or equilibrium constant being 1,152. And that's going to equal Our partial pressure of our nitrogen dioxide. Which in the question Stem said that it was 0.225 atmospheres. And we're going to square that and then we're going to divide that by our partial pressure of nitric oxide, which we don't know. So we're just gonna say X. And we're gonna square that as well. And then our partial pressure for molecular oxygen or 02 is 0.345 atmospheres, solving for X. We get an X. is equal to 0.0113 atmospheres. In other words, this is our partial pressure of nitric oxide. I hope this helped. And until next time.

Ch.16 - Chemical Equilibrium

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Tro 5th Edition

Ch.16 - Chemical Equilibrium

Problem 40

Chapter 16, Problem 40

Consider the reaction: SO₂Cl₂(g) ⇌ SO₂(g) + Cl₂(g) K_p = 2.91⨉10³ at 298 K In a reaction at equilibrium, the partial pressure of SO₂ is 137 torr and that of Cl₂ is 285 torr. What is the partial pressure of SO₂Cl₂in this mixture?

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Identify the equilibrium expression for the reaction. For the given reaction, SO2Cl2(g) ⇌ SO2(g) + Cl2(g), the equilibrium constant expression (Kp) is given by Kp = \( \frac{P_{SO2} \times P_{Cl2}}{P_{SO2Cl2}} \).

Substitute the known values of the partial pressures of SO2 and Cl2 into the equilibrium expression. Given that P_{SO2} = 137 torr and P_{Cl2} = 285 torr, the expression becomes Kp = \( \frac{137 \times 285}{P_{SO2Cl2}} \).

Rearrange the equation to solve for the unknown partial pressure of SO2Cl2. This can be done by isolating P_{SO2Cl2} on one side of the equation: P_{SO2Cl2} = \( \frac{137 \times 285}{Kp} \).

Substitute the value of Kp into the equation. Given that Kp = 2.91 \times 10^3, the equation to find P_{SO2Cl2} becomes P_{SO2Cl2} = \( \frac{137 \times 285}{2.91 \times 10^3} \).

Calculate the value of P_{SO2Cl2} using the values provided and the rearranged equation to find the partial pressure of SO2Cl2 in the mixture at equilibrium.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Equilibrium Constant (Kp)

The equilibrium constant (Kp) is a numerical value that expresses the ratio of the partial pressures of the products to the reactants at equilibrium for a given reaction at a specific temperature. For the reaction SO2Cl2(g) ⇌ SO2(g) + Cl2(g), Kp is calculated using the formula Kp = (P_SO2 * P_Cl2) / P_SO2Cl2, where P represents the partial pressures of the gases involved.

Partial Pressure

Partial pressure is the pressure exerted by a single component of a gas mixture. It can be determined using Dalton's Law, which states that the total pressure of a gas mixture is equal to the sum of the partial pressures of its individual components. In this case, the partial pressures of SO2 and Cl2 are given, and the partial pressure of SO2Cl2 can be derived from the equilibrium constant.

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust to counteract the change and restore a new equilibrium. In the context of this reaction, if the concentrations or pressures of the reactants or products are altered, the system will shift in a direction that minimizes the effect of that change, which is essential for understanding how equilibrium is established and maintained.