Question

Consider the following endothermic reaction. A(aq) + B(aq) equilibrium reaction arrow C(aq) + D(aq) K = 1 ✕ 100 A solution is prepared in which the initial concentrations of A and B are each 1.0 M. At equilibrium, the concentration of B would be about M, and the concentration of C would be about M. The concentration of C could be increased by which of the following? (Select all that apply.) adding A adding D increasing the temperature removing A removing D

a) 0.50 M
b) 1.00 M
c) 1.50 M
d) 2.00 M

Answer 1

The equilibrium of an endothermic reaction can be shifted to increase the concentration of product C by adding reactants A or D, increasing the temperature, or removing product D, following Le Chatelier's Principle.

Step-by-step explanation:

When considering an endothermic reaction of the form A(aq) + B(aq) ⇌ C(aq) + D(aq) with an equilibrium constant (K) of 1×100 and starting concentrations of A and B at 1.0 M each, we can analyze changes in concentration using the ICE table method (Initial, Change, Equilibrium). Adding 0.50 moles of A to the mixture will shift the equilibrium to the right in favor of products C and D due to Le Chatelier's Principle. As more reactants A and B are converted into products, the concentration of C will increase. The equilibrium can be further disturbed by several factors such as adding A or D, increasing the temperature (favorable for endothermic reactions), or removing A or D, which will all lead to an increase in the concentration of C according to Le Chatelier's Principle.