Multiple Choice
The equilibrium constant, Kp, equals 3.40 at 25°C for the isomerization reaction: cis-2-butene ⇌ trans-2-butene. If a flask initially contains 1.00 atm of each gas, in what direction will the system shift to reach equilibrium?
16. Chemical Equilibrium
Intro to Chemical Equilibrium
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The following two isomers of C3H7NO exist in equilibrium with each other in solution: If K_c = 0.57 at 25°C and the initial concentration of the reactant is 0.50 M and the product is 0.70 M, what are the concentrations of the reactant and product at equilibrium?
A
Reactant: 0.50 M, Product: 0.70 M
B
Reactant: 0.60 M, Product: 0.60 M
C
Reactant: 0.45 M, Product: 0.75 M
D
Reactant: 0.40 M, Product: 0.80 M
Verified step by step guidance1
Identify the initial concentrations of the reactant and product. The initial concentration of the reactant is 0.50 M and the product is 0.70 M.
Write the expression for the equilibrium constant, K_c, for the reaction: K_c = [Product]/[Reactant].
Set up an ICE (Initial, Change, Equilibrium) table to track the changes in concentrations. Let x be the change in concentration of the reactant that shifts to the product.
Express the equilibrium concentrations in terms of x: [Reactant] = 0.50 - x and [Product] = 0.70 + x.
Substitute the equilibrium concentrations into the K_c expression: 0.57 = (0.70 + x)/(0.50 - x). Solve for x to find the equilibrium concentrations of the reactant and product.
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