Given 2H2O (g) <--> 2H2 (g) + O2 (g) Kc = 5.9 x 103 at 200°C a) Determine the numerical value for Kp. b) Determine the numerical value of Kc for: 2H2 (g) + O2 (g) <--> 2H2O (g) c) If you start the original reaction above with 0.4 mol of H2O, 0.35 mol of H2, and 0.5 mol O2 in a 2.5 L container, how would you calculate the equilibrium concentrations for all species?
Given 2H2O (g) <--> 2H2 (g) + O2 (g) Kc = 5.9 x 103 at 200°C a) Determine the numerical value for Kp. b) Determine the numerical value of Kc for: 2H2 (g) + O2 (g) <--> 2H2O (g) c) If you start the original reaction above with 0.4 mol of H2O, 0.35 mol of H2, and 0.5 mol O2 in a 2.5 L container, how would you calculate the equilibrium concentrations for all species?
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions
Section: Chapter Questions
Problem 116SCQ: Calculate rH for the reaction 2 C(s) + 3 H2(g) + O2(g) C2H5OH() given the information below. C(s)...
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Given 2H2O (g) <--> 2H2 (g) + O2 (g)
Kc = 5.9 x 103 at 200°C
a) Determine the numerical value for Kp.
b) Determine the numerical value of Kc for: 2H2 (g) + O2 (g) <--> 2H2O (g)
c) If you start the original reaction above with 0.4 mol of H2O, 0.35 mol of H2, and 0.5 mol O2 in a 2.5 L container, how would you calculate the equilibrium concentrations for all species?
* You may stop once you have placed all values into the equilibrium expression.
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