Sure, let's analyze the given chemical reaction and determine how the equilibrium would change if the temperature were increased:
[tex]\[ \text{SO}_2(g) + \text{NO}_2(g) \rightleftharpoons \text{NO}(g) + \text{SO}_3(g) + \text{heat} \][/tex]
### Analysis:
1. Examine the Nature of the Reaction:
The reaction provided is exothermic, as indicated by the release of heat on the product side. This means that the forward reaction releases heat. Conversely, the reverse reaction is endothermic (it absorbs heat).
2. Application of Le Chatelier's Principle:
According to Le Chatelier's Principle, if a system at equilibrium experiences a disturbance (such as a change in temperature), the system will adjust itself to counteract the disturbance and re-establish equilibrium.
3. Effect of Increasing Temperature:
- When the temperature is increased, heat is added to the system.
- The system will counteract this by favoring the reaction that absorbs heat, which is the endothermic reaction. In this case, the endothermic reaction is the reverse reaction.
4. Impact on Concentrations:
- Favoring the reverse reaction means that the reactants ([tex]$\text{SO}_2$[/tex] and [tex]$\text{NO}_2$[/tex]) will be produced in higher amounts.
- The products ([tex]$\text{NO}$[/tex] and [tex]$\text{SO}_3$[/tex]) will be consumed and thus their amounts will decrease.
From this detailed analysis, the correct conclusion is:
D. The amount of [tex]$NO_2$[/tex] and [tex]$SO_2$[/tex] would increase.
This is because the equilibrium shifts towards the reactants (endothermic direction) to absorb the added heat when the temperature is increased.
