The heat of combustion of acetaldehyde to car | vedclass

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(A) The chemical formula of acetaldehyde is $CH_3CHO$. The molar mass of $CH_3CHO = (2 	imes 12) + (4 	imes 1) + 16 = 44 \ g \ mol^{-1}$.Given that

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$1758$

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(A) The chemical formula of acetaldehyde is $CH_3CHO$. The molar mass of $CH_3CHO = (2 	imes 12) + (4 	imes 1) + 16 = 44 \ g \ mol^{-1}$.Given that the heat of combustion for $1 \ mol$ $(44 \ g)$ of $CH_3CHO$ is $-1172 \ kJ \ mol^{-1}$.For $66 \ g$ of $CH_3CHO$,the number of moles $n = \frac{66 \ g}{44 \ g \ mol^{-1}} = 1.5 \ mol$.The heat liberated = $n 	imes \Delta H = 1.5 \ mol 	imes 1172 \ kJ \ mol^{-1} = 1758 \ kJ$.Therefore,the amount of heat liberated is $1758 \ kJ$.

The heat of combustion of acetaldehyde to carbon dioxide and water is $-1172 \ kJ \ mol^{-1}$. Calculate the amount of heat liberated when $66 \ g$ of acetaldehyde is completely oxidised. (Atomic mass: $C=12, H=1, O=16$) (in $kJ$)

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