The heat of combustion of C, S and $C S_{2}$ are -393.3kJ, -293.7kJ and -1108.76 kJ. What will be the heat of formation of $C S_{2}$ ?

-128.02 kJ

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+970 kJ

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+1108.7kJ

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+12 kJ

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Solution

The correct option is A -128.02 kJ
$C + 2 S \to C S_{2}$
$Δ H = \sum Δ H_{P} - \sum Δ H_{R}$ = -128.02 kJ

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The heat of combustion of C, S and CS2 are -393.3kJ, -293.7kJ and -1108.76 kJ. What will be the heat of formation of CS2?

The correct option is A -128.02 kJC+2S→CS2ΔH=∑ΔHP−∑ΔHR = -128.02 kJ

The heat of combustion of C, S and $C S_{2}$ are -393.3kJ, -293.7kJ and -1108.76 kJ. What will be the heat of formation of $C S_{2}$ ?

The correct option is A -128.02 kJ
$C + 2 S \to C S_{2}$
$Δ H = \sum Δ H_{P} - \sum Δ H_{R}$ = -128.02 kJ