This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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You're on a roll — Question 1 Equilibrium constant expression: For the reaction C(s) + CO_2(g) + 2Cl_2(g) 2COCl_2(g), the equilibrium constant expression K_c is: K_c = ([COCl_2(g)]^2)/([CO_2(g)][Cl_2(g)]^2) (Note: Solids like C(s) are not included in the equilibrium constant expression.) Calculation of the equilibrium constant: Given reactions: 1. C(s) + CO_2(g) 2CO(g) with K_c1 = 1.4 × 10^12 2. CO(g) + Cl_2(g) COCl_2(g) with K_c2 = 5.5 × 10^1 Target reaction: C(s) + CO_2(g) + 2Cl_2(g) 2COCl_2(g) Step 1: Manipulate the given reactions to obtain the target reaction. Multiply reaction (2) by 2: 2CO(g) + 2Cl_2(g) 2COCl_2(g) The new equilibrium constant for this reaction is (K_c2)^2. Step 2: Add reaction (1) and the modified reaction (2). C(s) + CO_2(g) 2CO(g) 2CO(g) + 2Cl_2(g) 2COCl_2(g) Summing these equations and canceling 2CO(g) from both sides gives: C(s) + CO_2(g) + 2Cl_2(g) 2COCl_2(g) Step 3: Calculate the overall equilibrium constant. When reactions are added, their equilibrium constants are multiplied. K_c = K_c1 × (K_c2)^2 K_c = (1.4 × 10^12) × (5.5 × 10^1)^2 K_c = (1.4 × 10^12) × (30.25 × 10^2) K_c = (1.4 × 10^12) × (3.025 × 10^3) K_c = (1.4 × 3.025) × 10^12+3 K_c = 4.235 × 10^15 The equilibrium constant for the reaction is 4.235 × 10^15. Send me the next one 📸