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(A) The formation reaction is: $2C(s) + 2H_2(g) + \frac{1}{2}O_2(g) \longrightarrow CH_3CHO(g)$The enthalpy of formation $\Delta H_f$ is calculated us

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$-200 \ kJ \ mol^{-1}$

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(A) The formation reaction is: $2C(s) + 2H_2(g) + \frac{1}{2}O_2(g) \longrightarrow CH_3CHO(g)$The enthalpy of formation $\Delta H_f$ is calculated using the formula: $\Delta H_f = \Sigma \Delta H_{	ext{sublimation/atomization}} - \Sigma BE_{	ext{products}}$$\Delta H_f = [2 	imes \Delta H_f(C) + 2 	imes \Delta H_f(H) + \frac{1}{2} 	imes \Delta H_f(O_2)] - [3 	imes BE(C-H) + 1 	imes BE(C-C) + 1 	imes BE(C=O)]$Note: $\Delta H_f(O_2) = 2 	imes 250 = 500 \ kJ \ mol^{-1}$$\Delta H_f = [(2 	imes 700) + (2 	imes 200) + (\frac{1}{2} 	imes 500)] - [(3 	imes 400) + (1 	imes 350) + (1 	imes 700)]$$\Delta H_f = [1400 + 400 + 250] - [1200 + 350 + 700]$$\Delta H_f = 2050 - 2250 = -200 \ kJ \ mol^{-1}$

Bond	Bond Enthalpy $(kJ \ mol^{-1})$	Enthalpy of formation $(kJ \ mol^{-1})$
$C-H$	$400$	$C(g): 700$
$C-C$	$350$	$H(g): 200$
$C=O$	$700$	$O(g): 250$

Use the data from the table to estimate the enthalpy of formation of $CH_3CHO$.
Bond Bond Enthalpy $(kJ \ mol^{-1})$ Enthalpy of formation $(kJ \ mol^{-1})$
$C-H$ $400$ $C(g): 700$
$C-C$ $350$ $H(g): 200$
$C=O$ $700$ $O(g): 250$

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Use the data from the table to estimate the enthalpy of formation of $CH_3CHO$.BondBond Enthalpy $(kJ \ mol^{-1})$Enthalpy of formation $(kJ \ mol^{-1})$$C-H$$400$$C(g): 700$$C-C$$350$$H(g): 200$$C=O$$700$$O(g): 250$