Question

1. how would an increase in temperature affect the equilibrium of an exothermic reaction?

a. equilibrium shifts left
c. no effect on equilibrium
b. equilibrium shifts right
d. reaction goes to completion

1. how would dissolving nacl in the system affect the equilibrium of the reaction agcl(s) ⇌ ag⁺(aq) + cl⁻(aq)?

a. equilibrium shifts left
c. no effect on equilibrium
b. equilibrium shifts right
d. reaction goes to completion

Explanation:

• For question 9: According to Le - Chatelier's principle, in an exothermic reaction (\(\Delta H<0\)), heat is a product. Increasing temperature (adding heat) will cause the system to shift in the direction that consumes heat. The reverse reaction (left - hand side) is endothermic (consumes heat), so the equilibrium shifts left.
• For question 10: The reaction is \(AgCl(s)

ightleftharpoons Ag^{+}(aq)+Cl^{-}(aq)\). When \(NaCl\) is dissolved, it dissociates as \(NaCl = Na^{+}+Cl^{-}\). This increases the concentration of \(Cl^{-}\) (a product). According to Le - Chatelier's principle, the system will shift in the direction that reduces the concentration of \(Cl^{-}\). The reverse reaction (left - hand side) consumes \(Cl^{-}\), so the equilibrium shifts left.

Answer:

1. a. equilibrium shifts left
2. a. equilibrium shifts left