Consider the following endothermic reaction at 345.0 °C HBr (g) = > H2 (g) + Bi2 (g) Kp=4.18×10^-9 A reaction vessel initially contains a partial pressure of HBr of 0.20 atm. Calculate: 1) the equilibrium pressure of HBr2(g) in atm 2) the equilibrium constant kc for this reaction at this temperature
Consider the following endothermic reaction at 345.0 °C HBr (g) = > H2 (g) + Bi2 (g) Kp=4.18×10^-9 A reaction vessel initially contains a partial pressure of HBr of 0.20 atm. Calculate: 1) the equilibrium pressure of HBr2(g) in atm 2) the equilibrium constant kc for this reaction at this temperature
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter16: Spontaneity, Entropy, And Free Energy
Section: Chapter Questions
Problem 77E
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Consider the following endothermic reaction at 345.0 °C
HBr (g) = > H2 (g) + Bi2 (g)
Kp=4.18×10^-9
A reaction vessel initially contains a partial pressure of HBr of 0.20 atm. Calculate:
1) the equilibrium pressure of HBr2(g) in atm
2) the equilibrium constant kc for this reaction at this temperature
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