Let's analyze the chemical equilibrium reaction:
[tex]\[ 2\text{NO}(g) + \text{O}_2(g) \rightleftharpoons 2\text{NO}_2(g) + 113.06 \text{kJ} \][/tex]
The problem tells us that the reaction is shifting to the left, which indicates that the equilibrium is moving towards the reactants' side of the reaction. This shift can be a result of changes in concentration, pressure, temperature, or other factors affecting the equilibrium.
To understand what happens to the amount of NO, consider the direction of the shift:
1. When the reaction shifts to the left, it means that the products are being converted back into reactants.
2. This causes an increase in the concentration of the reactants and a decrease in the concentration of the products.
3. Specifically, as the reaction shifts leftwards, more [tex]\(\text{NO}_2\)[/tex] and some energy (113.06 kJ) will be used to form more [tex]\(\text{NO}\)[/tex] and [tex]\(\text{O}_2\)[/tex].
4. Therefore, the concentration of [tex]\(\text{NO}\)[/tex] will increase because [tex]\(\text{NO}_2\)[/tex] is being converted back into [tex]\(\text{NO}\)[/tex].
In conclusion, the shift to the left in this equilibrium reaction will result in an increase in the amount of [tex]\(\text{NO}\)[/tex].
So, the correct answer is:
C. The amount of NO goes up.
