The equilibrium constant for the following reaction is 1.89×10-2 at 444 °C. 2 HI (g) ------> <----------- H2 (g) + I2 (g) K =1.89×10-2 at 444 °C Calculate the equilibrium constant for the following reactions at 444 °C. (a) H2(g) + I2(g) 2 HI(g) K = _____________ (b) HI(g) 1/2 H2(g) + 1/2 I2(g) K = ____________ B2: The following gas phase system is at equilibrium, CCl4(g) + CH4(g) ⇄ 2 CH2Cl2(g) The pressures of each gas measured are: PCCl4 = 198 mmHg PCH4 = 0.337 mmHg PCH2Cl2 = 135 mmHg What is the value of the equilibrium constant in terms of pressures, Kp?
The equilibrium constant for the following reaction is 1.89×10-2 at 444 °C. 2 HI (g) ------> <----------- H2 (g) + I2 (g) K =1.89×10-2 at 444 °C Calculate the equilibrium constant for the following reactions at 444 °C. (a) H2(g) + I2(g) 2 HI(g) K = _____________ (b) HI(g) 1/2 H2(g) + 1/2 I2(g) K = ____________ B2: The following gas phase system is at equilibrium, CCl4(g) + CH4(g) ⇄ 2 CH2Cl2(g) The pressures of each gas measured are: PCCl4 = 198 mmHg PCH4 = 0.337 mmHg PCH2Cl2 = 135 mmHg What is the value of the equilibrium constant in terms of pressures, Kp?
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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A)
The equilibrium constant for the following reaction is 1.89×10-2 at 444 °C.
2 HI (g) ------> <----------- H2 (g) + I2 (g)
K =1.89×10-2 at 444 °C
Calculate the equilibrium constant for the following reactions at 444 °C.
(a) H2(g) + I2(g) 2 HI(g) K = _____________
(b) HI(g) 1/2 H2(g) + 1/2 I2(g) K = ____________
B2:
The following gas phase system is at equilibrium,
CCl4(g) + CH4(g) ⇄ 2 CH2Cl2(g)
The pressures of each gas measured are:
PCCl4 = 198 mmHg
PCH4 = 0.337 mmHg
PCH2Cl2 = 135 mmHg
What is the value of the equilibrium constant in terms of pressures, Kp?
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