The pollutant NO forms in car engines via N2(g) + O2(g) 2NO(g), with Kc = 16 at 2300 K. If both N2 and O2 start at 1.5 M at 2300 K, what is the equilibrium concentration of N2 (in M)?

Question

The pollutant NO forms in car engines via N2(g) + O2(g) <-> 2NO(g), with Kc = 16 at 2300 K. If both N2 and O2 start at 1.5 M at 2300 K, what is the equilibrium concentration of N2 (in M)?

Accepted Answer

0.5 M. Solving Kc = (2x)²/((1.5-x)²) = 16 gives 2x/(1.5-x) = 4, so x = 1.0 M, leaving [N2] = 1.5 - 1.0 = 0.5 M.

The pollutant NO forms in car engines via N2(g) + O2(g) <-> 2NO(g), with Kc = 16 at 2300 K. If both N2 and O2 start at 1.5 M at 2300 K, what is the equilibrium concentration of N2 (in M)?

Solution

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