The enthalpy of combustion of carbon disulfide $(CS_2)$ is $-110.2 \, kJ \, mol^{-1}$. If the enthalpies of formation of $SO_2$ and $CO_2$ are $-297.4 \, kJ \, mol^{-1}$ and $-394.5 \, kJ \, mol^{-1}$ respectively,the enthalpy of formation of carbon disulfide is:
- A$-823.3 \, kJ \, mol^{-1}$
- B$-825.4 \, kJ \, mol^{-1}$
- C$-840.7 \, kJ \, mol^{-1}$
- D$-879.1 \, kJ \, mol^{-1}$
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$C_{(s)} + O_{2(g)} \longrightarrow CO_{2(g)}$
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$C_{(s)} + O_{2(g)} \longrightarrow CO_{2(g)}$
Given that:
$H_2O_{(g)} + C_{(s)} \longrightarrow CO_{(g)} + H_{2(g)} ; \Delta H = +131 \ kJ$
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