QuestionMay 28, 2025

Given the two combustion reactions shown below: CH_(4)(g)+O_(2)(g)arrow CO_(2)(g)+H_(2)O(g) III CH_(4)(g)+O_(2)(g)arrow CO_(2)(g)+H_(2)O(l) The two reactions have identical values of Delta H a TRUE b FALSE

Given the two combustion reactions shown below: CH_(4)(g)+O_(2)(g)arrow CO_(2)(g)+H_(2)O(g) III CH_(4)(g)+O_(2)(g)arrow CO_(2)(g)+H_(2)O(l) The two reactions have identical values of Delta H a TRUE b FALSE
Given the two combustion reactions shown below:
CH_(4)(g)+O_(2)(g)arrow CO_(2)(g)+H_(2)O(g)
III CH_(4)(g)+O_(2)(g)arrow CO_(2)(g)+H_(2)O(l)
The two reactions have identical values of Delta H
a TRUE
b FALSE

Solution
4.3(112 votes)

Answer

b FALSE Explanation 1. Identify Reaction States The reactions differ in the state of H_2O: one is gas (g), the other is liquid (l). 2. Consider Enthalpy Change **Enthalpy change (\Delta H)** depends on the states of products and reactants. The phase change from gas to liquid releases energy (latent heat). 3. Compare \Delta H for Both Reactions Since H_2O(g) has higher energy than H_2O(l), the reaction forming H_2O(l) will have a more negative \Delta H.

Explanation

1. Identify Reaction States<br /> The reactions differ in the state of $H_2O$: one is gas (g), the other is liquid (l).<br /><br />2. Consider Enthalpy Change<br /> **Enthalpy change ($\Delta H$)** depends on the states of products and reactants. The phase change from gas to liquid releases energy (latent heat).<br /><br />3. Compare $\Delta H$ for Both Reactions<br /> Since $H_2O(g)$ has higher energy than $H_2O(l)$, the reaction forming $H_2O(l)$ will have a more negative $\Delta H$.
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