For the reaction
N2(g) + 3 H2(g) 2 NH3(g)
Kc = 0.0600 at a certain temperature. In an equilibrium mixture of the three gases, [NH3] = 0.242 M and [ H2] = 1.03 M. What is the concentration of N2 in this system?

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BlackTom AI · Accepted Answer

We’re given the reaction N2(g) + 3 H2(g) ⇌ 2 NH3(g) with Kc = 0.0600 at a certain temperature. The equilibrium concentrations are [NH3] = 0.242 M and [H2] = 1.03 M. We need to determine [N2].

First, write the expression for the equilibrium constant in terms of concentrations: Kc = [NH3]^2 / ([N2][H2]^3).

Rearrange to solve for [N2]: [N2] = [NH3]^2 / (Kc × [H2]^3).

Compute the numerator: [NH3]^2 = (0.242)^2. 0.242 × 0.242 = 0.058564.

Compute the denominator: [H2]^3 = (1.03)^3. 1.03^2 = 1.0609, and 1.0609 × 1.03 = 1.092727. Then Kc × [H2]^3 = 0.0600 × 1.092727 = 0.06556362.

Now divide: [N2] = 0.058564 / 0.06556362 ≈ 0.893.

Accounting for significant figures from the given data (three or four sig figs in Kc and concentrations), the result is about 0.89 M.

Note: The answer options are not provided in this dataset, so this value is derived directly from the given Kc and concentrations using the standard expression for the equilibrium constant of this reaction. If there were multiple choices, each would be checked against this calculation to identify the closest value.

For the reaction N2(g) + 3 H2(g) 2 NH3(g) Kc = 0.0600 at a certain temperature. In an equilibrium mixture of the three gases, [NH3] = 0.242 M and [ H2] = 1.03 M. What is the concentration of N2 in this system?

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