Problem: What is the value of the equilibrium constant at 500 °C for the formation of NH3 according to the following equation?N2(g) + 3 H2(g) ⇌ 2 NH3(g)An equilibrium mixture of NH3(g), H2(g), and N2(g) at 500 °C was found to contain 1.35 M H2, 1.15 M N2, and 4.12 × 10−1 M NH3.

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FREE Expert Solution

We’re being asked to determine the equilibrium constant at 500˚C for this reaction:

N2(g) + 3 H2(g)  2 NH3(g)


Recall that the equilibrium constant is the ratio of the products and reactants

We use Kp when dealing with pressure and Kc when dealing with concentration:


Kp=PproductsPreactants     Kc=[products][reactants]


Note that solid and liquid compounds are ignored in the equilibrium expression.


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Problem Details

What is the value of the equilibrium constant at 500 °C for the formation of NH3 according to the following equation?

N2(g) + 3 H2(g) ⇌ 2 NH3(g)

An equilibrium mixture of NH3(g), H2(g), and N2(g) at 500 °C was found to contain 1.35 M H2, 1.15 M N2, and 4.12 × 10−1 M NH3.

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Based on our data, we think this problem is relevant for Professor Xie's class at HOWARDCC.

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Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.