Question

Consider this reaction: Zn(s) + 2HCl(aq) ZnCl2(aq) + H2(g). Which change could decrease the rate of production of ZnCl2?

Answer 1

Adding more hydrogen gas to the system or decreasing the volume of the container that the system is in. Le Chatelier's principle supports this.

Answer 2

Step-by-step explanation:

In reaction:

`Zn(s)+2HCl(aq)-> ZnCl_2(aq)+H_2(g)`

We know according to Le Chatelier's principle or "The Equilibrium Law" states that when a system experiences a disturbance (such as concentration, temperature, or pressure changes), it will respond to restore a new equilibrium state.

In this case rate of production of
`ZnCl_2` decreases when:

1. When concentration of HCl decreases.

2. When concentration of either
`ZnCl_2` or
`H_2` increases.

3. Increase in temperature because it is exothermic reaction.