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Consider the reaction. Upper n subscript 2 (g) plus 3 upper H subscript 2 (g) double-headed arrow 2 upper N upper H subscript 3 (g). At equilibrium, the concentrations of the different species are as follows. [NH3] = 0. 105 M [N2] = 1. 1 M [H2] = 1. 50 M What is the equilibrium constant for the reaction at this temperature? 0. 0030 0. 030 34 340.

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The equilibrium constant of the reaction is 0.0030.

The equation of the reaction is given as;

N2(g) + 3H2(g) ⇆ 2NH3 (g)

We have the following information at equilibrium;

[NH3] = 0.105 M

[N2] = 1.1 M

[H2] = 1.50 M

Hence, we can calculate the equilibrium constant using the relation;

K = [NH3]^2/ [N2]  [H2]^3

Substituting values;

K = [0.105]^2/[ 1.1] [1.50]^3

K =0.011025 /3.7125

K= 0.0030

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