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(C) The standard enthalpy change of the reaction is calculated using the formula: $\Delta_{r}H^{\circ} = \sum \Delta_{f}H^{\circ}(	ext{products}) - \

Vedclass · Accepted Answer

$-1355.00 \ kJ \ mol^{-1}$

Vedclass · Answer

(C) The standard enthalpy change of the reaction is calculated using the formula: $\Delta_{r}H^{\circ} = \sum \Delta_{f}H^{\circ}(	ext{products}) - \sum \Delta_{f}H^{\circ}(	ext{reactants})$.For the reaction $C_2H_5OH_{(\ell)} + 3O_{2_{(g)}} ightarrow 2CO_{2_{(g)}} + 3H_2O_{(\ell)}$,the expression is:$\Delta_{r}H^{\circ} = [2 	imes \Delta_{f}H^{\circ}(CO_2) + 3 	imes \Delta_{f}H^{\circ}(H_2O)] - [\Delta_{f}H^{\circ}(C_2H_5OH) + 3 	imes \Delta_{f}H^{\circ}(O_2)]$.Since $\Delta_{f}H^{\circ}(O_2) = 0 \ kJ \ mol^{-1}$ (standard state of an element),we have:$\Delta_{r}H^{\circ} = [2(-390) + 3(-285)] - [-280 + 3(0)]$.$\Delta_{r}H^{\circ} = [-780 - 855] - [-280]$.$\Delta_{r}H^{\circ} = -1635 + 280 = -1355 \ kJ \ mol^{-1}$.

Process	$\Delta H \ (kJ/mol)$
$I. \ \frac{1}{2} A \rightarrow B$	$+150$
$II. \ 3B \rightarrow 2C + D$	$-125$
$III. \ E + A \rightarrow 2D$	$+350$

Similar Questions

Calculate the heat required to convert $9 \ g$ of liquid water to water vapor using the following equations:
$H_{2(g)} + 1/2 O_{2(g)} \longrightarrow H_2O_{(g)} \quad \Delta H = -57 \ kCal$
$H_{2(g)} + 1/2 O_{2(g)} \longrightarrow H_2O_{(l)} \quad \Delta H = -68.3 \ kCal$ (in $kCal$)

The standard enthalpy of formation $(\Delta_f H^{\circ})$ of ammonia is $-46.2 \ kJ \ mol^{-1}$. What is the $\Delta_r H^{\circ}$ of the following reaction?
$N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$

Consider the following processes:

Process $\Delta H \ (kJ/mol)$

$I. \ \frac{1}{2} A \rightarrow B$ $+150$

$II. \ 3B \rightarrow 2C + D$ $-125$

$III. \ E + A \rightarrow 2D$ $+350$

For $B + D \rightarrow E + 2C, \Delta H$ will be ............. $kJ/mol$

The heat of formation of $H_2O$ is $-286 \, kJ/mol$ and $H_2O_2$ is $-188 \, kJ/mol$. The enthalpy change for the reaction $2H_2O_2 \to 2H_2O + O_2$ is......$kJ$.

If the bond formation energy of the $H-H$ bond is $-433 \ kJ \ mol^{-1}$,find the bond dissociation energy for $0.5 \ mol$ of $H_{2(g)}$. (in $kJ$)

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