Multiple Choice
What does a very small equilibrium constant (K << 1) indicate about a chemical reaction at equilibrium?
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16. Chemical Equilibrium
Equilibrium Constant K
Multiple Choice
For the reaction N_2(g) + 3H_2(g) ightarrow 2NH_3(g), the equilibrium concentrations at 500 K are [N_2] = 0.20 M, [H_2] = 0.60 M, and [NH_3] = 1.2 M. What is the value of the equilibrium constant K_c for this reaction in correct scientific notation?
A
K_c = 2.8 imes 10^1
B
K_c = 5.0 imes 10^{-1}
C
K_c = 2.2 imes 10^2
D
K_c = 1.7 imes 10^0
Verified step by step guidance1
Write the balanced chemical equation: \(\mathrm{N_2(g) + 3H_2(g) \rightarrow 2NH_3(g)}\).
Recall the expression for the equilibrium constant \(K_c\) in terms of concentrations:
\(K_c = \frac{[\mathrm{NH_3}]^2}{[\mathrm{N_2}][\mathrm{H_2}]^3}\).
Substitute the given equilibrium concentrations into the expression:
\(K_c = \frac{(1.2)^2}{(0.20)(0.60)^3}\).
Calculate the numerator and denominator separately:
Numerator = \((1.2)^2\), Denominator = \((0.20) \times (0.60)^3\).
Divide the numerator by the denominator to find \(K_c\), then express the result in correct scientific notation.
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