Consider the following equilibrium, for which at 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 15th Edition

Ch.15 - Chemical Equilibrium

Problem 26a

Chapter 15, Problem 26a

Consider the following equilibrium, for which at 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 a reverse reaction is the reciprocal of the equilibrium constant for the forward reaction.

Write the expression for the equilibrium constant of the reverse reaction as 1/K_p.

Substitute the given K_p value of 0.0752 into the expression for the reverse reaction.

Calculate the reciprocal to find the K_p 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.

Reversibility of Reactions

Chemical reactions can proceed in both forward and reverse directions, and the equilibrium constant for the reverse reaction is the reciprocal of the forward reaction's equilibrium constant. This means that if you know Kp for a reaction, you can easily find Kp for the reverse reaction by taking the inverse of that value. This principle is crucial for solving equilibrium problems.

Stoichiometry in Equilibrium

Stoichiometry refers to the quantitative relationship between reactants and products in a chemical reaction, as represented by the balanced equation. In equilibrium expressions, the coefficients of the balanced equation become the exponents in the Kp expression. Understanding stoichiometry is essential for accurately calculating equilibrium constants and predicting the direction of the reaction.

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Textbook Question

Consider the following equilibrium: 2 H₂(g) + S₂(g) ⇌ 2 H₂S(g) K_c = 1.08 × 10⁷ at 700°C (c) Calculate the value of 𝐾𝑐 if you rewrote the equation H₂(g) + 1/2 S₂(g) ⇌ H₂S(g)

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

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 value of 𝐾_𝑐 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 at 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)?

Verified video answer for a similar problem:

Key Concepts

Equilibrium Constant (Kp)

Reversibility of Reactions

Stoichiometry in Equilibrium

Consider the following equilibrium, for which at 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)?