Consider the following equilibrium: 2 H 2 (g) + S 2 (g) ⇌ 2 H 2 S(g) K c = 1.08 × 10 7 at 700°C (c) Calculate the value of 𝐾𝑐 if you rewrote the equation H 2 (g) + 1/2 S 2 (g) ⇌ H 2 S(g)

Hi everyone. So here we have the K. C. Value for the following reaction below. And this is 8.68 times 10 to the third at 27.9 degrees Celsius. Were asked what would be the K. C. Value if the following equation became the one below. We see that we have the same reactors in products, in both reactions of nitric oxide in auction, gas at the reactant and that nitrogen tetroxide as a product. But the coefficients in both reactions are different. In the first we actually have two moles of nitric oxide but only one In the second reaction, I have one more option gas in the first. Let me have one half moles of oxygen gas in the second And then we have one mole of dimension tetroxide in the 1st. 1/2 moles in the second. So this means that if we divide the first reaction by two, we get the second reaction. Sophie divide by two. This is the same as most climbed by one half. We raised the K. C. Value to the power of one half. Let me get Casey. It was 8.68 Times 10 to the 3rd. The power of one hat for K. C. We get money 3.2. 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 24c

Chapter 15, Problem 24c

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)

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Identify the original balanced chemical equation and the new equation. Original: 2 H₂(g) + S₂(g) ⇌ 2 H₂S(g). New: H₂(g) + 1/2 S₂(g) ⇌ H₂S(g).

Note that the new equation is obtained by dividing all coefficients in the original equation by 2.

Understand that the equilibrium constant expression, K_c, for a reaction depends on the stoichiometry of the reaction. When the coefficients of a balanced equation are multiplied or divided by a number, the equilibrium constant is raised to the power of that number.

Since the coefficients in the original equation are divided by 2 to get the new equation, raise the original K_c to the power of 1/2.

Calculate the new K_c by taking the square root of the original K_c value, which is 1.08×10⁷.

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Key Concepts

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

Equilibrium Constant (Kc)

The equilibrium constant (Kc) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given chemical reaction. It is temperature-dependent and provides insight into the extent of a reaction; a larger Kc indicates a greater concentration of products at equilibrium. Understanding Kc is essential for predicting how changes in conditions affect the position of equilibrium.

Stoichiometry in Chemical Reactions

Stoichiometry involves the quantitative relationships between the reactants and products in a chemical reaction, based on their coefficients in the balanced equation. When rewriting a reaction, the stoichiometric coefficients must be adjusted accordingly, which affects the calculation of the equilibrium constant. This concept is crucial for determining how the equilibrium constant changes when the reaction is expressed in different forms.

Reaction Quotient (Q)

The reaction quotient (Q) is a measure of the relative concentrations of products and reactants at any point in time, not just at equilibrium. It is calculated using the same formula as Kc but with the current concentrations. Understanding Q helps in predicting the direction in which a reaction will proceed to reach equilibrium, and it is essential when considering how changes in the reaction's stoichiometry affect Kc.