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Consider the equilibrium system described by the chemical reaction below. At equilibrium, a 5.0 L reaction vessel contained a mixture of 1.22 mol CH4, 2.79 mol H₂S, 0.630 mol CS₂, and 1.27 x 10-³ mol H₂ at 420.0 °C. What are the values of Kc and Kp for the reaction at this temperature? Complete Parts 1-2 before submitting your answer. CH₂(g) + 2 H₂S(g) = CS₂(l) + 4 H₂(g) 1 2 Based on the given data, set up the expression for

Consider the equilibrium system described by the chemical reaction below. At equilibrium, a 5.0 L reaction vessel contained a mixture of 1.22 mol CH4, 2.79 mol H₂S, 0.630 mol CS₂, and 1.27 x 10-³ mol H₂ at 420.0 °C. What are the values of Kc and Kp for the reaction at this temperature? Complete Parts 1-2 before submitting your answer. CH₂(g) + 2 H₂S(g) = CS₂(l) + 4 H₂(g) 1 2 Based on the given data, set up the expression for

Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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◄ Search 5GE 5:20 PM Question 4 of 6 Kc 1000 11% Consider the equilibrium system described by the chemical reaction below. At equilibrium, a 5.0 L reaction vessel contained a mixture of 1.22 mol CH4, 2.79 mol H₂S, 0.630 mol CS₂, and 1.27 × 10-³ mol H₂ at 420.0 °C. What are the values of Kc and Kp for the reaction at this temperature? Complete Parts 1-2 before submitting your answer. CH₂(g) + 2 H₂S(g) = CS₂(l) + 4 H₂(g) 1 2 Based on the given data, set up the expression for Kc. Each reaction participant must be represented by one tile. Do not combine terms. Once the expression is constructed, solve for Kc. = Submit [1.22] [2.79] [0.630] [0.244] [0.558] [0.126] 2[2.79] [2.79]² 2[0.558] 4[2.54 x 10-41 [2.54 x 10-4]4 4[1.27 x 10-³]| Tap here or pull up for additional resources RESET [1.27 x 10-³] [2.54 x 10-4] [0.558]² [1.27 x 10-³]4
Transcribed Image Text:◄ Search 5GE 5:20 PM Question 4 of 6 Kc 1000 11% Consider the equilibrium system described by the chemical reaction below. At equilibrium, a 5.0 L reaction vessel contained a mixture of 1.22 mol CH4, 2.79 mol H₂S, 0.630 mol CS₂, and 1.27 × 10-³ mol H₂ at 420.0 °C. What are the values of Kc and Kp for the reaction at this temperature? Complete Parts 1-2 before submitting your answer. CH₂(g) + 2 H₂S(g) = CS₂(l) + 4 H₂(g) 1 2 Based on the given data, set up the expression for Kc. Each reaction participant must be represented by one tile. Do not combine terms. Once the expression is constructed, solve for Kc. = Submit [1.22] [2.79] [0.630] [0.244] [0.558] [0.126] 2[2.79] [2.79]² 2[0.558] 4[2.54 x 10-41 [2.54 x 10-4]4 4[1.27 x 10-³]| Tap here or pull up for additional resources RESET [1.27 x 10-³] [2.54 x 10-4] [0.558]² [1.27 x 10-³]4
Expert Solution
Step 1: Rules of writing equilibrium constant expression

Equilibrium constant Kc for a reaction is defined as the product of the equilibrium molar concentrations of the products, each raised to the power equal to a stoichiometric coefficient divided by the product of the equilibrium molar concentrations of the reactant each raised to the power equal to its stoichiometric coefficient .
& the most important convention to be kept in mind is that the active mass of a pure solid or pure liquid is considered to be constant.

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