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tia_tia [17]
3 years ago
5

Consider the following reaction: Consider the reaction 2NO(g)+Br2(g)⇌2NOBr(g) ,Kp=28.4 at 298 K In a reaction mixture at equilib

rium, the partial pressure of NO is 119 torr and that of Br2 is 151 torr . What is the partial pressure of NOBr in this mixture?
Chemistry
1 answer:
Vitek1552 [10]3 years ago
4 0

Answer:  partial pressure of NOBr is 7792 atm

Explanation:

Equilibrium constant is the ratio of the concentration of products to the concentration of reactants each term raised to its stochiometric coefficients.

2NO(g)+Br_2(g)\rightleftharpoons 2NOBr(g)

Equilibrium constant is given as:

K_{p}=\frac{[p_{NOBr}]^2}{[p_{NO}]^2\times [p_{Br_2}]^1}

28.4=\frac{[p_{NOBr}]^2}{[(119)^2\times (151)^1}

[p_{NOBr}]=7792 atm

Partial pressure of NOBr is 7792 atm

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