Problem: When H2(g) and O2(g) react to form H2O(l), heat is released to the surroundings. Consider the reverse reaction, namely, the formation of H2(g) and O2(g) from H2O(l): 2 H2O(l) → 2 H2(g) + O2(g). Is this reaction exothermic or endothermic?

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When H2(g) and O2(g) react to form H2O(l), heat is released to the surroundings. Consider the reverse reaction, namely, the formation of H2(g) and O2(g) from H2O(l): 2 H2O(l) → 2 H2(g) + O2(g). Is this reaction exothermic or endothermic?
A diagram shows that the initial state (H2 (gas) and O2 (gas)) has higher internal energy (E) than the final state (H2O (liquid)).  E sub initial is greater than E sub final; therefore, energy is released from the system to the surroundings during the reaction and delta-E is less than 0.

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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 Endothermic & Exothermic Reactions concept. If you need more Endothermic & Exothermic Reactions practice, you can also practice Endothermic & Exothermic Reactions practice problems.

What professor is this problem relevant for?

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