Given:C + 2S to CS_2 ; Delta H_f^o = +117.0 , | vedclass

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(B) To find the heat of reaction for $CS_2 + 3O_2 	o CO_2 + 2SO_2$, we use Hess's Law.We need to manipulate the given equations:$1$. Reverse equation

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$-1104$

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(B) To find the heat of reaction for $CS_2 + 3O_2 	o CO_2 + 2SO_2$, we use Hess's Law.We need to manipulate the given equations:$1$. Reverse equation $(1)$: $CS_2 	o C + 2S ; \Delta H = -117.0 \, kJ \, mol^{-1}$$2$. Keep equation $(2)$ as is: $C + O_2 	o CO_2 ; \Delta H = -393 \, kJ \, mol^{-1}$$3$. Multiply equation $(3)$ by $2$: $2S + 2O_2 	o 2SO_2 ; \Delta H = 2 	imes (-297) = -594 \, kJ \, mol^{-1}$Adding these three equations:$(CS_2 	o C + 2S) + (C + O_2 	o CO_2) + (2S + 2O_2 	o 2SO_2)$$CS_2 + 3O_2 	o CO_2 + 2SO_2$$\Delta H_{reaction} = -117.0 - 393 - 594 = -1104 \, kJ \, mol^{-1}$

$H-H$ bond energy	$431.37 \text{ kJ mol}^{-1}$
$C=C$ bond energy	$606.10 \text{ kJ mol}^{-1}$
$C-C$ bond energy	$336.49 \text{ kJ mol}^{-1}$
$C-H$ bond energy	$410.50 \text{ kJ mol}^{-1}$

Given:
$C + 2S \to CS_2 ; \Delta H_f^o = +117.0 \, kJ \, mol^{-1} \dots (1)$
$C + O_2 \to CO_2 ; \Delta H_f^o = -393 \, kJ \, mol^{-1} \dots (2)$
$S + O_2 \to SO_2 ; \Delta H_f^o = -297 \, kJ \, mol^{-1} \dots (3)$
The heat of reaction for $CS_2 + 3O_2 \to CO_2 + 2SO_2$ is:
.....$kJ \, mol^{-1}$

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$\frac{1}{2} N_{2(g)} + \frac{1}{2} O_{2(g)} \rightarrow NO_{(g)}; \Delta_r H^{\ominus} = 90 \, kJ \, mol^{-1}$
$NO_{(g)} + \frac{1}{2} O_{2(g)} \rightarrow NO_{2(g)}; \Delta_r H^{\ominus} = -74 \, kJ \, mol^{-1}$

The bond energy is the energy required to

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Given:$C + 2S \to CS_2 ; \Delta H_f^o = +117.0 \, kJ \, mol^{-1} \dots (1)$$C + O_2 \to CO_2 ; \Delta H_f^o = -393 \, kJ \, mol^{-1} \dots (2)$$S + O_2 \to SO_2 ; \Delta H_f^o = -297 \, kJ \, mol^{-1} \dots (3)$The heat of reaction for $CS_2 + 3O_2 \to CO_2 + 2SO_2$ is:.....$kJ \, mol^{-1}$