The reaction 2 NO(g) + Br₂ (g) = 2 NOBr(g) has Kp = 109 at 25°C. If the equilibrium partial pressure of Br2 is 0.0270 atm and the equilibrium partial pressure of NOBr is 0.0600 atm, calculate the partial pressure of NO at equilibrium. Partial pressure = atm

The reaction 2 NO(g) + Br₂ (g) = 2 NOBr(g) has Kp = 109 at 25°C. If the equilibrium partial pressure of Br2 is 0.0270 atm and the equilibrium partial pressure of NOBr is 0.0600 atm, calculate the partial pressure of NO at equilibrium. Partial pressure = atm

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

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 118CP: Consider the decomposition equilibrium for dinitrogen pentoxide: 2N2O5(g)4NO2(g)+O2(g) At a certain...

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Question

The reaction
2 NO(g) + Br₂ (g) = 2 NOBr(g)
has
Kp = 109 at 25°C. If the equilibrium partial pressure of
Br2 is 0.0270 atm and the equilibrium partial pressure of
NOBr is 0.0600 atm, calculate the partial pressure of
NO at equilibrium.
Partial pressure =
Submit Answer
atm
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