Problem: Consider the reaction:    N2(g) + O2(g) ⇌ 2 NO(g)for which Kc = 0.10 at 2,000 °C. Starting with initial concentrations of 0.15 M N2 and 0.15 M O2, determine the equilibrium concentration of NO.A. 0.020 M B. 0.13 M C. 0.0071 M D. 0.014 ME. 0.041 M

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We’re being asked to calculate the equilibrium concentration of NO, given the following reaction:

N2(g) + O2(g) ⇌ 2 NO(g);  Kc = 0.10


We're given the initial concentrations of the reactants:

[N2] = 0.15 M
[O2] = 0.15 M

From this, we can construct an ICE table:


The Kc expression for the reaction is:

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Problem Details

Consider the reaction:    N2(g) + O2(g) ⇌ 2 NO(g)
for which Kc = 0.10 at 2,000 °C. Starting with initial concentrations of 0.15 M N2 and 0.15 M O2, determine the equilibrium concentration of NO.

A. 0.020 M 

B. 0.13 M 

C. 0.0071 M 

D. 0.014 M

E. 0.041 M

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