🤓 Based on our data, we think this question is relevant for Professor Hinton's class at UTOLEDO.
At constant V and T, P will drop since there are 3 moles of gases in the reactant compared to 2 moles of gases in products
Reaction is exothermic since we are releasing energy once NO and O2 reacts
ΔH < 0 (losing energy to the surroundings)
Suppose that the gas-phase reaction 2NO(g) + O2(g) → 2NO2(g) were carried out in a constant-volume container at constant temperature.
(a) Would the measured heat change represent ΔH or ΔE?
(b) If there is a difference, which quantity is larger for this reaction?