Multiple Choice
For the reaction 2 R (g) ⇌ Q (g), if the equilibrium concentration of R is 0.776 M and that of Q is 1.22 M at 25 °C, what is the value of the equilibrium constant K at this temperature?
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16. Chemical Equilibrium
Equilibrium Constant K
Multiple Choice
The Keq for the equilibrium below is 5.4 x 10^13 at 480.0°C.2NO (g) + O2 (g) ↔ 2NO2 (g)What is the value of Keq at this temperature for the following reaction?NO (g) + 1/2 O2 (g) ↔ NO2 (g)
A
7.3 x 10^6
B
2.3 x 10^7
C
1.1 x 10^14
D
2.3 x 10^13
Verified step by step guidance1
Understand that the equilibrium constant (Keq) is dependent on the stoichiometry of the balanced chemical equation. The given Keq is for the reaction: 2NO (g) + O2 (g) ↔ 2NO2 (g).
Recognize that the new reaction, NO (g) + 1/2 O2 (g) ↔ NO2 (g), is essentially half of the original reaction. This means the stoichiometry has been halved.
Recall that when the stoichiometry of a reaction is changed, the equilibrium constant is affected. Specifically, if the coefficients of a balanced equation are divided by a factor, the equilibrium constant is raised to the power of that factor.
Apply the rule for adjusting Keq: Since the stoichiometry is halved, the new Keq is the square root of the original Keq. Mathematically, this can be expressed as:
Calculate the square root of the original Keq value to find the new Keq for the reaction NO (g) + 1/2 O2 (g) ↔ NO2 (g). This will give you the correct answer.
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