Predict the effect of increasing the temperature on the amount(s) of product(s) in the following reactions: (a) \(\mathrm{CO}(g)+2 \mathrm{H}_{2}(g) \rightleftharpoons \mathrm{CH}_{3} \mathrm{OH}(g)\) \(\Delta H_{\mathrm{rxn}}^{\circ}=-90.7 \mathrm{~kJ}\) (b) \(\mathrm{C}(s)+\mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons \mathrm{CO}(g)+\mathrm{H}_{2}(g) \quad \Delta H_{\mathrm{rxn}}^{\circ}=131 \mathrm{~kJ}\) (c) \(2 \mathrm{NO}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g)\) (endothermic) (d) \(2 \mathrm{C}(s)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{CO}(g)\) (exothermic)

Exothermic reactions release energy into their surroundings as heat or light. In these reactions, the reactants have more energy than the products. This means energy is given off during the reaction. We can identify an exothermic reaction in a chemical equation by a negative \(\Delta H\) value.

For example, an exothermic reaction looks like this:
\(\text{A} + \text{B} \rightarrow \text{C} + \text{D} \) with \(\Delta H = -90.7 \text{~kJ}\). Here, 'A' and 'B' release 90.7 kJ of energy when they form 'C' and 'D'.

According to Le Chatelier's Principle, if we increase the temperature of an exothermic reaction, the equilibrium position shifts to oppose this change. Since exothermic reactions release heat, adding more heat will shift the equilibrium towards the reactants. The system tries to absorb some of the extra heat by favoring the reverse reaction.

Endothermic reactions absorb energy from their surroundings. Unlike exothermic reactions, the products have more energy than the reactants. This means energy is taken in during the reaction. We can identify an endothermic reaction by a positive \(\Delta H\) value.

An example of an endothermic reaction looks like this:
\(\text{A} + \text{B} \rightarrow \text{C} + \text{D} \) with \(\Delta H = 131 \text{~kJ}\) Here, 'A' and 'B' absorb 131 kJ of energy to form 'C' and 'D'.

According to Le Chatelier's Principle, increasing the temperature of an endothermic reaction shifts the equilibrium position towards the products. Since endothermic reactions absorb heat, adding more heat will favor the forward reaction, helping the system take in the excess energy.

Le Chatelier's Principle explains how a system at equilibrium responds to changes. When a change occurs, the system shifts to counteract that change, seeking to establish a new equilibrium.

In the case of temperature changes:

• For exothermic reactions, increasing the temperature shifts the equilibrium towards the reactants (left).
• For endothermic reactions, increasing the temperature shifts the equilibrium towards the products (right).

This principle helps us understand how an equilibrium system will react to different conditions and can be applied to predict the effects on the position of equilibrium when conditions are changed.

Let's review the provided example reactions:

• For reaction (a): Exothermic reaction shifting left on temperature increase.
• For reaction (b): Endothermic reaction shifting right on temperature increase.
• For reaction (c): Endothermic reaction shifting right on temperature increase.
• For reaction (d): Exothermic reaction shifting left on temperature increase.