Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [N2]eq = 1.1 M, [H2]eq = 1.5 M, [NH3]eq = 0.47 M.

N2(g) + 3 H2(g) 2 NH3(g)

Question

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [N2]eq = 1.1 M, [H2]eq = 1.5 M, [NH3]eq = 0.47 M.

N2(g) + 3 H2(g)  2 NH3(g)

BlackTom AI · Accepted Answer

We start by identifying the balanced chemical equation and the expression for Kc: N2 + 3 H2 ⇌ 2 NH3. For Kc we use the concentrations at equilibrium: Kc = [NH3]^2 / ([N2][H2]^3).

Next, plug in the given equilibrium concentrations: [NH3]eq = 0.47 M, [N2]eq = 1.1 M, [H2]eq = 1.5 M.

Compute the numerator: [NH3]^2 = (0.47)^2 = 0.2209.

Compute the denominator: [N2][H2]^3 = (1.1) × (1.5)^3. First, (1.5)^3 = 3.375. Then multiply by 1.1: 1.1 × 3.375 = 3.7125.

Form the ratio: Kc = 0.2209 / 3.7125 ≈ 0.0595.

Rounding considerations: depending on the required significant figures, this value is commonly expressed as about 5.95×10^-2 or 0.060 when rounded to three significant figures. Since no multiple-choice options were provided in the prompt, the calculated value corresponds to the numerical result you’d select if given a list of close values.

Conceptual check: note that the reaction produces ammonia, so a relatively small Kc here indicates the equilibrium lies toward the reactants at these concentrations, which is consistent with a Kc on the order of 10^-2. If you had different concentration units or a different reaction quotient setup, you’d recompute accordingly, but the method remains the same: substitute equilibrium concentrations into the Kc expression and perform the algebra carefully.

CHM-1020-LD01.2025SU PS I- Part II (Equilibrium)

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [N2]eq = 1.1 M, [H2]eq = 1.5 M, [NH3]eq = 0.47 M. N2(g) + 3 H2(g) 2 NH3(g)

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