Multiple Choice
For the reaction A ⇌ B at equilibrium, if the concentration of A is 0.5 M and the concentration of B is 2.0 M, what is the value of the equilibrium constant Kc?
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16. Chemical Equilibrium
Equilibrium Constant K
Multiple Choice
How is the equilibrium constant (K) expressed for the reaction: 8 Cs(s) + 8 H2O(l) ⇌ 8 CsOH(aq) + 4 H2(g)?
A
K = [CsOH]^8[H2]^4
B
K = [CsOH][H2]^4 / [H2O]
C
K = [CsOH]^8[H2]^4 / [H2O]^8
D
K = [CsOH]^4[H2]^8
Verified step by step guidance1
Identify the balanced chemical equation for the reaction: 8 Cs(s) + 8 H2O(l) ⇌ 8 CsOH(aq) + 4 H2(g).
Recognize that the equilibrium constant expression, K, is based on the concentrations of the products and reactants raised to the power of their stoichiometric coefficients.
Note that pure solids and liquids do not appear in the equilibrium constant expression. Therefore, Cs(s) and H2O(l) are not included in the expression.
Write the equilibrium constant expression using the concentrations of the aqueous and gaseous species: K = [CsOH]^8[H2]^4.
Ensure that the expression reflects the stoichiometry of the balanced equation, where the coefficients of CsOH and H2 are used as exponents in the expression.
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