Question Detail

CHM 101 CHM 101 Past Questions Objective Question
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Question

For the reaction 2H₂(g) + O₂(g) → 2H₂O(l) with ΔH = -572 kJ, which statement is true?
Options
A The enthalpy change would be the same if gaseous water were produced.
B The enthalpy of the products is lower than the potential energy of the reactants.
Correct Answer
C The products occupy a larger volume than the reactants.
D The reaction is endothermic.
Correct Answer

Option B is the correct answer.

Detailed Explanation

ΔH is negative, so the reaction is exothermic, meaning the products have lower enthalpy. If H₂O(g) were produced, ΔH would be less negative (more energy required to vaporize water). Reactants have 3 moles of gas, products have 0 moles of gas (liquid water), so products occupy a smaller volume.

Hint

Consider the sign of ΔH and the physical states of products and reactants.

Question Info

Course: CHM 101
Topic: CHM 101 Past Questions
Type: Objective
Difficulty: Not specified
Question 1204 of 1872
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