Answer:
1. The concentration of N₂O₄ decrease as the temperature of the system increased.
2. The formation of products was favored by the addition of heat.
3. The reaction going from right to left is exothermic.
4. N₂O₄ → 2NO₂; HR = +14 kcal.
Explanation:
Equation of the reaction is as follows: N₂O₄ ⇄ 2NO₂
The forward reaction proceeds with an increase in temperature. As the temperature of the reaction was increased, more of the N₂O₄ decomposed to form NO₂. Therefore, the concentration of N₂O₄ deceased.
2. The formation of products, that is the forward reaction leading to formation of NO₂ was favored by the addition of heat. Thus, with increase in temperature, the concentration of NO₂ increased.
3. An endothermic reaction is a type of reaction which requires energy input in the form of heat in order to proceed.
From the observations during the reaction, an increase in temperature by the addition of heat resulted in an increase in the forward reaction, therefore, the forward reaction is endothermic and the backward reaction is exothermic. Thus, the reaction in which colorless N₂O₄ is produced, is an exothermic reaction.
4. The change in enthalpy of a reaction is the difference in the heat content of reactants and products. For exothermic reactions, enthalpy change is negative, whereas for endothermic reactions, enthalpy change is positive.
The decomposition of N₂O₄ to NO₂ is an endothermic reaction. Hence, the correct chemical equation is: N₂O₄ → 2NO₂; HR = +14 kcal.
.............(1)
..............(2)