To understand how the rate of the reaction changes when more heat is removed from the reaction, we need to consider Le Chatelier's Principle.
Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.
The given reaction is:
[tex]\[ \text{Zn} + 2 \text{HCl} \leftrightharpoons \text{ZnCl}_2 + \text{H}_2 + \text{heat} \][/tex]
In this reaction, heat is a product, which means it is an exothermic reaction. When more heat is removed from the reaction mixture, the system will try to produce more heat to counteract the loss. According to Le Chatelier's Principle, the equilibrium will shift to the right, towards the production of more products (ZnCl_2 and H_2), thereby increasing the rate of the forward reaction.
This shift produces more of the products to balance the removal of heat.
Therefore, the correct selections are:
- The rate of the forward reaction increases and produces more ZnCl_2 and H_2.
