A,B,C and D are some compounds. The enthalpy | vedclass

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(A) Given:$\Delta H_f(A) = 9.7 \ kJ \ mol^{-1}$$\Delta H_f(B) = -110 \ kJ \ mol^{-1}$$\Delta H_f(C) = 81 \ kJ \ mol^{-1}$$\Delta H_f(D) = -393 \ kJ \

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$-777.7$

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(A) Given:$\Delta H_f(A) = 9.7 \ kJ \ mol^{-1}$$\Delta H_f(B) = -110 \ kJ \ mol^{-1}$$\Delta H_f(C) = 81 \ kJ \ mol^{-1}$$\Delta H_f(D) = -393 \ kJ \ mol^{-1}$Reaction: $A_{(g)} + 3B_{(g)} \longrightarrow C_{(g)} + 3D_{(g)}$$\Delta_r H = \sum \Delta H_f(	ext{products}) - \sum \Delta H_f(	ext{reactants})$$\Delta_r H = [\Delta H_f(C) + 3 	imes \Delta H_f(D)] - [\Delta H_f(A) + 3 	imes \Delta H_f(B)]$$\Delta_r H = [81 + 3 	imes (-393)] - [9.7 + 3 	imes (-110)]$$\Delta_r H = [81 - 1179] - [9.7 - 330]$$\Delta_r H = -1098 - (-320.3)$$\Delta_r H = -1098 + 320.3$$\Delta_r H = -777.7 \ kJ \ mol^{-1}$

$A$,$B$,$C$ and $D$ are some compounds. The enthalpy of formation of $A_{(g)}$,$B_{(g)}$,$C_{(g)}$ and $D_{(g)}$ is $9.7, -110, 81$ and $-393 \ kJ \ mol^{-1}$ respectively. What is $\Delta_r H$ (in $kJ \ mol^{-1}$) for the given reaction?
$A_{(g)} + 3B_{(g)} \longrightarrow C_{(g)} + 3D_{(g)}$

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$A$,$B$,$C$ and $D$ are some compounds. The enthalpy of formation of $A_{(g)}$,$B_{(g)}$,$C_{(g)}$ and $D_{(g)}$ is $9.7, -110, 81$ and $-393 \ kJ \ mol^{-1}$ respectively. What is $\Delta_r H$ (in $kJ \ mol^{-1}$) for the given reaction?$A_{(g)} + 3B_{(g)} \longrightarrow C_{(g)} + 3D_{(g)}$