Problem: 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?

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FREE Expert Solution

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)

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Problem Details

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?