Problem: Consider the following reaction:2NO(g) + Br2(g) ⇌ 2NOBr(g)Kp= 28.4 at 298 KIn a reaction mixture at equilibrium, the partial pressure of NO is 107 torr and that of Br2 is 166 torr.What is the partial pressure of NOBr in this mixture? 

FREE Expert Solution

asdasdKp can be calculated as:

Kp = productsreactantsKp = pNOBr2pNO2 × pBr228.4 = pNOBr21072× 166pNOBr = 28.4(1072× 166)

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Problem Details

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 107 torr and that of Br2 is 166 torr.

What is the partial pressure of NOBr in this mixture?

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