QuestionWhat happens to the equilibrium reaction when heated? $2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{~g})+113.06 \mathrm{~kJ}$ A. Shift right, increase $\mathrm{NO}_{2}$ ; B. No change; C. Shift left, decrease $\mathrm{NO}$ , $\mathrm{O}_{2}$ ; D. Shift left, decrease $\mathrm{NO}_{2}$ .

Studdy Solution

STEP 1

Assumptions1. The reaction is at equilibrium. . The system is closed, meaning no matter is being added or removed.
3. The system is being heated, which means energy is being added to the system.
4. The reaction is exothermic, as indicated by the positive heat term on the product side of the equation.

STEP 2

We need to understand the principle of Le Chatelier. According to Le Chatelier's principle, if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.

STEP 3

In this case, the system is being heated. According to Le Chatelier's principle, the system will react by shifting the equilibrium to the side that absorbs the heat to counteract this change.

STEP 4

Since the reaction is exothermic (releases heat), the heat is considered a product of the reaction. Therefore, adding heat to the system will shift the equilibrium to the left, towards the reactants.

STEP 5

This shift towards the reactants will result in a decrease in the concentration of the product, $\mathrm{NO}_{2}$ , and an increase in the concentrations of the reactants, $\mathrm{NO}$ and $\mathrm{}_{2}$ .
So, the correct answer is D. The reaction will shift toward the reactants (left) and decrease the concentration of $\mathrm{NO}_{2}$ .

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