1) 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?
1) 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: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter5: Thermochemistry
Section: Chapter Questions
Problem 5.83QE: Calculate H when a 38-g sample of glucose, C6H12O6(s), burns in excess O2(g) to form CO2(g) and...
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1) 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?
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