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Ch.15 - Chemical Equilibrium
All textbooksMcMurry 8th EditionCh.15 - Chemical EquilibriumProblem 93
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Chapter 15, Problem 93

The air pollutant NO is produced in automobile engines from the high-temperature reaction N2(g) + O2(g) ⇌ 2 NO(g); Kc = 1.7 * 10^-3 at 2300 K. If the initial concentrations of N2 and O2 at 2300 K are both 1.40 M, what are the concentrations of NO, N2, and O2 when the reaction mixture reaches equilibrium?

Verified step by step guidance
1
Step 1: Write the balanced chemical equation for the reaction: N2(g) + O2(g) ⇌ 2 NO(g).
Step 2: Set up an ICE (Initial, Change, Equilibrium) table to track the concentrations of N2, O2, and NO. Initially, [N2] = 1.40 M, [O2] = 1.40 M, and [NO] = 0 M.
Step 3: Define the change in concentration for the reaction. Let x be the change in concentration of N2 and O2 that reacts. Therefore, the change for NO will be +2x, and for N2 and O2, it will be -x.
Step 4: Express the equilibrium concentrations in terms of x: [N2] = 1.40 - x, [O2] = 1.40 - x, and [NO] = 2x.
Step 5: Substitute the equilibrium concentrations into the expression for the equilibrium constant Kc: Kc = ([NO]^2) / ([N2][O2]) = (2x)^2 / ((1.40 - x)(1.40 - x)) and solve for x.
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