The heat of formation of water is 260 kJ. Ho | vedclass

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(C) The reaction for the formation of water is as follows:$H_2(g) + \frac{1}{2} O_2(g) \longrightarrow H_2O(l); \quad \Delta H = -260 \ kJ$For the dec

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$0.5$

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(C) The reaction for the formation of water is as follows:$H_2(g) + \frac{1}{2} O_2(g) \longrightarrow H_2O(l); \quad \Delta H = -260 \ kJ$For the decomposition of water,the reaction is reversed:$H_2O(l) \longrightarrow H_2(g) + \frac{1}{2} O_2(g); \quad \Delta H = +260 \ kJ$This means that $260 \ kJ$ of heat is required to decompose $1 \ mol$ of $H_2O$.Therefore,the amount of $H_2O$ decomposed by $130 \ kJ$ of heat is:$	ext{Moles of } H_2O = \frac{1 \ mol}{260 \ kJ} 	imes 130 \ kJ = 0.5 \ mol$

The heat of formation of water is $260 \ kJ$. How much $H_2O$ is decomposed by $130 \ kJ$ of heat (in $mol$)?

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