Question

a chemist measures the energy change δh during the following reaction: 2 h₂o(l) → 2 h₂(g) + o₂(g) δh = 572. kj use the information to answer the following questions. this reaction is... ∘ endothermic. ∘ exothermic. suppose 36.6 g of h₂o react. will any heat be released or absorbed? ∘ yes, absorbed. ∘ yes, released. ∘ no. if you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. round your answer to 3 significant digits. ∘ kj

Explanation:

Step1: Identify reaction type

Endothermic (ΔH positive: 572 kJ).

Step2: Determine heat flow

Endothermic reactions absorb heat.

Step3: Calculate moles of H₂O

Molar mass of H₂O = 18.02 g/mol. Moles = 36.6 g / 18.02 g/mol ≈ 2.031 mol.

Step4: Relate moles to ΔH

2 mol H₂O absorb 572 kJ. Heat for 2.031 mol = (2.031/2)×572 ≈ 581 kJ.

Answer:

1. endothermic.
2. Yes, absorbed.
3. 581 kJ