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At 600 K, 2 mol NO are mixed with 1 mol O2 and the reaction 2NO(g) + O2(g) <=> 2NO2(g) reaches equilibrium at a total pressure of 1 atm. Analysis shows 0.6 mol O2 present at equilibrium. Calculate the equilibrium constant Kp for the reaction (nearest integer).

1. 1.93 atm⁻¹
2. 0.52 atm⁻¹
3. 5.0 atm⁻¹
4. 21 atm⁻¹

Correct answer: 1.93 atm⁻¹

Solution

O2 reacted = 0.4 mol, so NO reacted = 0.8 mol (NO left 1.2), NO2 formed = 0.8 mol. Total moles = 2.6. Converting to partial pressures at 1 atm and substituting gives Kp ~= 1.93 atm⁻¹.

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