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3) For the following reaction at 25°C: H₂ (g) + 12 (g) = 2H1 (g), Kc = 10.7 Complete the chart below: H₂(g) 0.550 M a. I C E 1₂ (g) 0.885 M 2HI (g) 0 C. Use Kp Kc (RT)An and compare it to the Kp form part b. 0.828 M b. Calculate the equilibrium partial pressures of each gas (line E above). Use them to find Kp.

3) For the following reaction at 25°C: H₂ (g) + 12 (g) = 2H1 (g), Kc = 10.7 Complete the chart below: H₂(g) 0.550 M a. I C E 1₂ (g) 0.885 M 2HI (g) 0 C. Use Kp Kc (RT)An and compare it to the Kp form part b. 0.828 M b. Calculate the equilibrium partial pressures of each gas (line E above). Use them to find Kp.

Chemistry
Chemistry
10th Edition
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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3) For the following reaction at 25°C: H₂ (g) + 12 (g) = 2HI (g), Kc = 10.7 a. Complete the chart below: H₂ (g) 0.550 M I C E 1₂ (g) 0.885 M 2HI (g) 0 C. Use Kp = Kc (RT)An and compare it to the Kp form part b. 0.828 M b. Calculate the equilibrium partial pressures of each gas (line E above). Use them to find Kp.
Transcribed Image Text:3) For the following reaction at 25°C: H₂ (g) + 12 (g) = 2HI (g), Kc = 10.7 a. Complete the chart below: H₂ (g) 0.550 M I C E 1₂ (g) 0.885 M 2HI (g) 0 C. Use Kp = Kc (RT)An and compare it to the Kp form part b. 0.828 M b. Calculate the equilibrium partial pressures of each gas (line E above). Use them to find Kp.
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