Calculate the heat of combustion (in kJ) of m | vedclass

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(A) The combustion reaction for methane is: $CH_{4(g)} + 2O_{2(g)} \rightarrow CO_{2(g)} + 2H_2O_{(l)} \quad \Delta H = ?$To obtain this,we manipulate

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$-891.1$

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(A) The combustion reaction for methane is: $CH_{4(g)} + 2O_{2(g)} ightarrow CO_{2(g)} + 2H_2O_{(l)} \quad \Delta H = ?$To obtain this,we manipulate the given equations:$1$. Reverse equation $(i)$: $CH_{4(g)} ightarrow C_{	ext{(graphite)}} + 2H_{2(g)} \quad \Delta H = +74.8 \ kJ$$2$. Keep equation (ii) as is: $C_{	ext{(graphite)}} + O_{2(g)} ightarrow CO_{2(g)} \quad \Delta H = -393.5 \ kJ$$3$. Multiply equation (iii) by $2$: $2H_{2(g)} + O_{2(g)} ightarrow 2H_2O_{(l)} \quad \Delta H = 2 	imes (-286.2) = -572.4 \ kJ$Adding these equations gives the target reaction:$\Delta H = 74.8 + (-393.5) + (-572.4) = -891.1 \ kJ$

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