Consider the following equilibrium, for which 𝐾 𝑝 = 0.0752 at 480°C: 2 Cl 2 (𝑔) + 2 H 2 O(𝑔) ⇌ 4 HCl(𝑔) + O 2 (𝑔) (a) What is the value of 𝐾 𝑝 for the reaction 4 HCl(𝑔) + O 2 (𝑔) ⇌ 2 Cl 2 (𝑔) + 2 H 2 O(𝑔)?

Hi everyone. So here we're giving the K. P. For the following reaction below. And this is 1.10 times 10 to the 10 at 78.5°C. We were asked what would be the K. P. value if the following equation became the one below. You see that in the first reaction, hydrazine and hatching gas, other reactant while ammonia is a product. But in the second reaction, ammonia is the reactant, while hydrazine and hydrogen gas are the products. This means the second reaction is the reverse of the first reaction. If we reverse the first reaction that K. P becomes K. P equals one Over the K. P Value for the First Reaction, which is 1.10 times 10 to the 10. And this gives us 9.09. I'm sent to the mega 11 as the K. P. For the second reaction. Thanks for watching my video and I hope it was helpful.

Ch.15 - Chemical Equilibrium

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Brown 14th Edition

Ch.15 - Chemical Equilibrium

Problem 26a

Chapter 15, Problem 26a

Consider the following equilibrium, for which 𝐾_𝑝= 0.0752 at 480°C: 2 Cl₂(𝑔) + 2 H₂O(𝑔) ⇌ 4 HCl(𝑔) + O₂(𝑔) (a) What is the value of 𝐾_𝑝 for the reaction 4 HCl(𝑔) + O₂(𝑔) ⇌ 2 Cl₂(𝑔) + 2 H₂O(𝑔)?

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Identify that the given reaction is the reverse of the original reaction.

Recall that the equilibrium constant for the reverse reaction is the reciprocal of the equilibrium constant for the forward reaction.

Write the expression for the equilibrium constant of the reverse reaction: \( K'_{p} = \frac{1}{K_{p}} \).

Substitute the given value of \( K_{p} = 0.0752 \) into the expression for the reverse reaction.

Calculate the reciprocal to find \( K'_{p} \), which is the equilibrium constant for the reverse reaction.

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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 concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. It is calculated using the partial pressures of gases involved in the reaction. A Kp value less than 1 indicates that at equilibrium, reactants are favored, while a value greater than 1 indicates that products are favored.

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust itself to counteract the change and restore a new equilibrium. This principle helps predict how changes in concentration, pressure, or temperature will affect the position of equilibrium in a chemical reaction.

Reaction Quotient (Q)

The reaction quotient, Q, is a measure of the relative amounts of products and reactants present in a reaction at any point in time, not just at equilibrium. It is calculated in the same way as Kp but uses the current concentrations or partial pressures. Comparing Q to Kp allows us to determine the direction in which the reaction will proceed to reach equilibrium.

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Reaction Quotient Q

Related Practice

Textbook Question

At 1000 K, 𝐾_𝑝= 1.85 for the reaction SO₂(𝑔) + 12 O₂(𝑔) ⇌ SO₃(𝑔) (c) What is the value of 𝐾𝑐 for the reaction in part (b)?

Textbook Question

Consider the following equilibrium, for which K_p= 0.0752 at 480°C: 2 Cl₂(g) + 2 H₂O(g) ⇌ 4 HCl(g) + O₂(g) (b) What is the value of K_p for the reaction Cl₂(g) + H₂O(g) ⇌ 2 HCl(g) + 1/2 O2(g)?

Textbook Question

The following equilibria were attained at 823 K:

CoO(s) + H₂(g) → Co(s) + H₂O(g) K_c = 67

CoO(s) + CO(g) → Co(s) + CO₂(g) K_c = 490

Based on these equilibria, calculate the equilibrium constant for H₂(g) + CO₂(g) → CO(g) + H₂O(g) at 823 K.

Textbook Question

Consider the equilibrium N₂(𝑔) + O₂(𝑔) + Br₂(𝑔) ⇌ 2 NOBr(𝑔) Calculate the equilibrium constant 𝐾𝑝 for this reaction, given the following information at 298 K:

2 NO(𝑔) + Br₂(𝑔) ⇌ 2 NOBr(𝑔) 𝐾_𝑐= 2.02

NO(𝑔) ⇌ N₂(𝑔) + O₂(𝑔) 𝐾_𝑐= 2.1×10³⁰

Consider the following equilibrium, for which 𝐾𝑝 = 0.0752 at 480°C: 2 Cl2(𝑔) + 2 H2O(𝑔) ⇌ 4 HCl(𝑔) + O2(𝑔) (a) What is the value of 𝐾𝑝 for the reaction 4 HCl(𝑔) + O2(𝑔) ⇌ 2 Cl2(𝑔) + 2 H2O(𝑔)?

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Key Concepts

Equilibrium Constant (Kp)

Le Chatelier's Principle

Reaction Quotient (Q)

Consider the following equilibrium, for which 𝐾_𝑝= 0.0752 at 480°C: 2 Cl₂(𝑔) + 2 H₂O(𝑔) ⇌ 4 HCl(𝑔) + O₂(𝑔) (a) What is the value of 𝐾_𝑝 for the reaction 4 HCl(𝑔) + O₂(𝑔) ⇌ 2 Cl₂(𝑔) + 2 H₂O(𝑔)?