You are studying the reaction:
A(aq) ↔ 3 B(aq)
The value of Kc for this reaction is 0.685. When the reaction reaches equilibrium, you find [A]eq=0.133M. What is [B]eq?
Report your answer to 3 decimal places.
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You are studying the reaction: A(aq) ↔ 3 B(aq) The value of Kc for this reaction...
You are studying the reaction: 2 A(aq) ↔ 3 B(aq) When the reaction reaches equilibrium, you find [A]eq=0.297M and [B]eq=0.617M. What is the value of Kc for this reaction? Report your answer to 2 decimal places. Your Answer:
You are studying the reaction: A(aq) + 2 B(aq) ↔ C(aq) + D(aq) When the reaction reaches equilibrium, you find [A]eq=0.209M, [B]eq=0.285M, [C]eq=0.781M, and [D]eq=0.779M . What is the value of Kc for this reaction? Report your answer to 2 decimal places. Your Answer:
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1) The Keq for the reaction: A + B ↔ A B is 36 What is the Keq for A B ↔ A + B ? 2) The Keq for the reaction: A+B ↔ ABA+B ↔ AB is 8 What is the Keq for 3 AB↔ 3 A +3 B3 AB↔ 3 A +3 B ? 3)Consider the reaction below. 1.3 mol of A and 7.5 mol of B are added to a 2 L container. At equilibrium, the concentration of...
Consider the equilibrium constant Kc for the reaction: N2O4(g) ↔ 2NO2(g) is 0.211 at 100°C. What is the value for the equilibrium constant is the reaction is balanced as ½ N2O4(g) ↔ NO2(g) ? A. 0.106 B. 0.459 C. 0.211 D. 0.422
Consider the balanced chemical equation for this equilibrium reaction: A (aq) + B (aq) = AB (aq) To determine the equilibrium constant for this reaction at 298 K, a student mixes two solutions together and allows them to react: • 10.0 mL of 0.60 M A (aq), and, • 40.0 mL of 0.25 MB (aq). When this solution reaches equilibrium, the student measures the equilibrium concentration of AB in the 50.0 mL solution: [AB]E = 0.10 M. Which values should...
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