The equilibrium constant, Kp, for the following
reaction is 0.160 at 298K.
2NOBr(g)
2NO(g) +
Br2(g)
If an equilibrium mixture of the three gases in a
19.9 L container at 298K contains
NOBr at a pressure of 0.297 atm
and NO at a pressure of 0.251
atm, the equilibrium partial pressure of
Br2 is ? atm.
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The equilibrium constant, Kp, for the following reaction is 0.160 at 298K. 2NOBr(g) 2NO(g) + Br2(g)...
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Consider the following reaction: 2NO(g)+Br2(g)⇌2NOBr(g) ,Kp=28.4, at 298 K In a reaction mixture at equilibrium, the partial pressure of NO is 102 torr and that of Br2 is 134 torr . Part A What is the partial pressure of NOBr in this mixture? Express your answer in torrs to three significant figures.
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Consider the reaction: 2NO(g)+Br2(g)⇌2NOBr(g) Kp=28.4 at 298 K In a reaction mixture at equilibrium, the partial pressure of NO is 101 torr and that of Br2 is 150 torr . What is the partial pressure of NOBr in this mixture? Express your answer using three significant figures.
Consider the reaction: 2NO(g)+Br2(g)⇌2NOBr(g) Kp=28.4 at 298 K. In a reaction mixture at equilibrium, the partial pressure of NO is 108 torr and that of Br2 is 158 torr . What is the partial pressure of NOBr in this mixture?
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