The heats of combustion of C_{(s)},H_{2(g)},a | vedclass

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(B) The combustion reactions are:$I. C_{(s)} + O_{2(g)} \longrightarrow CO_{2(g)} \quad \Delta H_{1} = -x_{1}$$II. H_{2(g)} + \frac{1}{2} O_{2(g)} \lo

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$-2x_{1} - 3x_{2} + x_{3}$

Vedclass · Answer

(B) The combustion reactions are:$I. C_{(s)} + O_{2(g)} \longrightarrow CO_{2(g)} \quad \Delta H_{1} = -x_{1}$$II. H_{2(g)} + \frac{1}{2} O_{2(g)} \longrightarrow H_{2}O_{(l)} \quad \Delta H_{2} = -x_{2}$$III. C_{2}H_{6(g)} + \frac{7}{2} O_{2(g)} \longrightarrow 2CO_{2(g)} + 3H_{2}O_{(l)} \quad \Delta H_{3} = -x_{3}$We need the heat of formation of $C_{2}H_{6(g)}$:$2C_{(s)} + 3H_{2(g)} \longrightarrow C_{2}H_{6(g)} \quad \Delta H_f = ?$Perform the operation: $(2 	imes I) + (3 	imes II) - III$$\Delta H_f = 2(-x_{1}) + 3(-x_{2}) - (-x_{3})$$\Delta H_f = -2x_{1} - 3x_{2} + x_{3}$

Column-$I$	Column-$II$
$(A) \; CO_{2(s)} \to CO_{2(g)}$	$(p) \; \text{Transition state}$
$(B) \; CaCO_{3(s)} \to CaO_{(s)} + CO_{2(g)}$	$(q) \; \text{Allotropic change}$
$(C) \; 2H^{\cdot} \to H_{2(g)}$	$(r) \; \Delta H > 0$
$(D) \; P_{\text{(white solid)}} \to P_{\text{(red solid)}}$	$(s) \; \Delta S > 0$
	$(t) \; \Delta S < 0$

The heats of combustion of $C_{(s)}$,$H_{2(g)}$,and $C_{2}H_{6(g)}$ are $-x_{1}$,$-x_{2}$,and $-x_{3}$ respectively. The heat of formation of $C_{2}H_{6(g)}$ is:

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