Given the reaction N_2(g) + 3H_2(g) ightarrow 2NH_3(g), and the following equilibrium concentrations obtained from a graph: [N_2] = 0.20 M, [H_2] = 0.60 M, [NH_3] = 1.20 M, estimate the value of the equilibrium constant K_c for this reaction.

• A. K_c = 100
• B. K_c = 10
• C. K_c = 0.1
• D. K_c = 1

Answer: (A)

Verified step by step guidance

1. Write the balanced chemical equation: \(\mathrm{N_2(g) + 3H_2(g) \rightarrow 2NH_3(g)}\).
2. Recall the expression for the equilibrium constant \(K_c\) in terms of concentrations: \(K_c = \frac{[\mathrm{NH_3}]^2}{[\mathrm{N_2}][\mathrm{H_2}]^3}\).
3. Substitute the given equilibrium concentrations into the expression: \(K_c = \frac{(1.20)^2}{(0.20)(0.60)^3}\).
4. Calculate the powers and products in the denominator and numerator separately, keeping track of each step carefully.
5. Divide the numerator by the denominator to find the numerical value of \(K_c\), which estimates the equilibrium constant for the reaction.