To understand how the rate of the reaction changes when heat is removed, we need to apply Le Chatelier's Principle. Le Chatelier's Principle states that if a system at equilibrium experiences a change in conditions (such as temperature, pressure, or concentration of reactants/products), the system will adjust to counteract that change and restore equilibrium.
The given reaction is:
[tex]\[ \text{Zn} + 2 \text{HCl} \rightleftharpoons \text{ZnCl}_2 + \text{H}_2 + \text{heat} \][/tex]
This reaction is exothermic, meaning it releases heat as a product.
### Step-by-Step Explanation:
1. Identifying the Change:
- According to the question, heat is being removed from the system.
2. Applying Le Chatelier's Principle:
- When heat is removed from an exothermic reaction, the system will try to produce more heat to counteract the reduction in temperature.
- To produce more heat, the reaction will shift in the forward direction (to the right).
3. Resultant Reaction Direction:
- The rate of the forward reaction will increase to generate more heat, thereby opposing the removal of heat.
4. Formation of Products:
- As the reaction shifts forward, it will produce more of the products: [tex]\(\text{ZnCl}_2\)[/tex], [tex]\(\text{H}_2\)[/tex], and heat.
### Conclusion:
When heat is removed from the reaction, the rate of the forward reaction increases to produce more [tex]\(\text{ZnCl}_2\)[/tex], [tex]\(\text{H}_2\)[/tex], and heat.
Therefore, the completed sentence should be:
> The rate of the forward reaction increases and produces more [tex]\(\text{ZnCl}_2\)[/tex], [tex]\(\text{H}_2\)[/tex], and heat.
