Question

Initially, 0.840 mol of A is present in a 4.50 L solution. 2A(aq)↽−−⇀2B(aq)+C(aq) At equilibrium, 0.100 mol of C is present. Calculate K.

a. 0.00217
b. 0.00450
c. 0.02250
d. 0.01125

Answer 1

The equilibrium constant, K, can be calculated using the concentrations of the reactants and products at equilibrium. In this case, the equation is 2A(aq)→2B(aq)+C(aq). Correct answer is b. 0.00450.

Step-by-step explanation:

The equilibrium constant, K, can be calculated using the concentrations of the reactants and products at equilibrium. In this case, the equation is 2A(aq)→2B(aq)+C(aq). Since the equation is balanced, the equilibrium constant expression is K = [B]²[C] / [A]². We can plug in the values given in the question: [A] = 0.840 mol and [C] = 0.100 mol.

Substituting these values into the equation and solving for K gives us K = (0.100 mol) / (0.840 mol)² = 0.00450. Therefore, Correct answer is b. 0.00450.