Calculate the value of the equilibrium constant for the reaction 4 NH31g2 + 3 O21g2 ∆ 2 N21g2 + 6 H2O1g2
given the following equilibrium constants at a certain temperature.
2 H21g2 + O21g2 ∆ 2 H2O1g2 Kc = 3.2 * 1081
N21g2 + 3 H21g2 ∆ 2 NH31g2 Kc = 3.5 * 108

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Identify the given reactions and their equilibrium constants. The first reaction is 2 H2(g) + O2(g) ⇌ 2 H2O(g) with Kc = 3.2 * 10^8, and the second reaction is N2(g) + 3 H2(g) ⇌ 2 NH3(g) with Kc = 3.5 * 10^8.

Write the target reaction: 4 NH3(g) + 3 O2(g) ⇌ 2 N2(g) + 6 H2O(g).

Break down the target reaction into reactions that involve the given equilibrium constants. This can be done by reversing the second given reaction and multiplying it by 2, and using the first given reaction multiplied by 3.

Calculate the equilibrium constant for the reversed reaction of NH3 formation by taking the reciprocal of the given Kc for that reaction, since reversing a reaction inverts its equilibrium constant (Kc' = 1/Kc).

Combine the equilibrium constants of the adjusted reactions using the rule that when reactions are added, their equilibrium constants are multiplied. For the reversed reaction, use the reciprocal value calculated in the previous step.

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