Given the following thermochemical equations: | vedclass

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(D) The target reaction is: $2N_{2(g)} + 5O_{2(g)} ightarrow 2N_2O_{5(g)}$.We can obtain this by manipulating the given equations:$2 	imes (iii)$ $

Vedclass · Accepted Answer

$26.8$

Vedclass · Answer

(D) The target reaction is: $2N_{2(g)} + 5O_{2(g)} ightarrow 2N_2O_{5(g)}$.We can obtain this by manipulating the given equations:$2 	imes (iii)$ $\Rightarrow 2N_{2(g)} + 6O_{2(g)} + 2H_{2(g)}$ $ightarrow 4HNO_{3(l)}; \Delta H = 2 	imes (-348.2) = -696.4 	ext{ kJ}$$2 	imes (ii) 	ext{ reversed}$ $\Rightarrow 4HNO_{3(l)}$ $ightarrow 2N_2O_{5(g)} + 2H_2O_{(l)}; \Delta H = -2 	imes (-76.6) = +153.2 	ext{ kJ}$$2 	imes (i) 	ext{ reversed}$ $\Rightarrow 2H_2O_{(l)}$ $ightarrow 2H_{2(g)} + O_{2(g)}; \Delta H = -2 	imes (-285) = +570 	ext{ kJ}$Adding these equations:$(2N_{2(g)} + 6O_{2(g)} + 2H_{2(g)}) + (4HNO_{3(l)}) + (2H_2O_{(l)})$ $ightarrow (4HNO_{3(l)}) + (2N_2O_{5(g)} + 2H_2O_{(l)}) + (2H_{2(g)} + O_{2(g)})$Simplifying gives: $2N_{2(g)} + 5O_{2(g)} ightarrow 2N_2O_{5(g)}$$\Delta H = -696.4 + 153.2 + 570 = 26.8 	ext{ kJ}$.

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