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?

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)

99% (482 ratings)
View Complete Written Solution
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?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Internal Energy concept. You can view video lessons to learn Internal Energy. Or if you need more Internal Energy practice, you can also practice Internal Energy practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Hinton's class at UTOLEDO.