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Byju's Answer

Standard XII

Chemistry

Hess' Law

Use the given...

Question

Use the given standard enthalpies of formation to determine the heat of reaction of the following reaction:
$C_{2} H_{5} O H (l) + 3 O_{2} (g) ⟶ 2 C O_{2} (g) + 3 H_{2} O (g)$
$Δ H_{f} C_{2} H_{5} O H (l) = - 277.7 k J / m o l e$
$Δ H_{f} C O_{2} (g) = - 393.5 k J / m o l e$
$Δ H_{f} H_{2} O (g) = - 241.8 k J / m o l e$

-1456.3

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-1234.7

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-1034

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Solution

The correct option is B -1234.7
$Δ H_{r} = [2 {(Δ H_{f})}_{C O_{2}} + 3 {(Δ H_{f})}_{H_{2} O} - {(Δ H_{f})}_{C_{2} H_{5} O H}]$
$Δ H_{r} = [2 (- 393.5) - 3 (241.8) + 277.7]$
$Δ H_{r} = - 1234.7 k J / m o l e$

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Similar questions

Q. Use the given standard enthalpies of formation to determine the heat of reaction of the following reaction:

2 L i O H + C O_{2} (g) ⟶ {L i}_{2} C O_{3} (s) + H_{2} O (l)

Δ H_{f} L i O H (s) = - 487.23 k J / m o l e

Δ H_{f} {L i}_{2} C O_{3} (s) = - 1215.6 k J / m o l e

Δ H_{f} H_{2} O (l) = - 285.85 k J / m o l e

Δ H_{f} C O_{2} (g) = - 393.5 k J / m o l e

Q. Use the given standard enthalpies of formation to determine the heat of reaction of the following reactions:

T i C l_{4} (g) + 2 H_{2} O (g) \to T i O_{2} (g) + 4 H C l (G)

△ H_{f}^{\circ} T i C l_{4} (g) = - 736.2 k J / m o l e △ H_{f}^{\circ} T i O_{2} (g) = - 944.7 k J / m o l e

△ H_{f}^{\circ} H_{2} O (g) = - 241.8 k J / m o l e △ H_{f}^{\circ} H C l (g) = - 92.3 k J / m o l e

Q. If

Δ E

is the heat of reaction for

C_{2} H_{5} O H (l) + 3 O_{2} (g) ⟶ 2 C O_{2} (g) + 3 H_{2} O (l)

at constant volume, the

Δ H

(heat of reaction at constant pressure), at constant temperature is:

Q. If

Δ E

is the heat of rection for

C_{2} H_{5} O H (l) + 3 O_{2} (g) ⟶ 2 {C O}_{2} (g) + 3 H_{2} O (l)

at constant volume, the

Δ H

(heat of reaction at constant pressure), at constant temperature is:

The $Δ H_{f}^{\circ}$ for $C O_{2} (g), C O (g)$ and $H_{2} O (g)$ are $- 393.5, - 110.5$ and $- 241.8 k J m o l e^{- 1}$ respectively. The standard enthalpy change in kJ for the reaction $C O_{2} (g) + H_{2} (g) \to C O (g) + H_{2} O (g)$ is

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Use the given standard enthalpies of formation to determine the heat of reaction of the following reaction: C2H5OH(l)+3O2(g)⟶2CO2(g)+3H2O(g)ΔHfC2H5OH(l)=−277.7kJ/moleΔHfCO2(g)=−393.5kJ/moleΔHfH2O(g)=−241.8kJ/mole

The correct option is B -1234.7ΔHr=[2(ΔHf)CO2+3(ΔHf)H2O−(ΔHf)C2H5OH]ΔHr=[2(−393.5)−3(241.8)+277.7]ΔHr=−1234.7kJ/mole

The correct option is B -1234.7
$Δ H_{r} = [2 {(Δ H_{f})}_{C O_{2}} + 3 {(Δ H_{f})}_{H_{2} O} - {(Δ H_{f})}_{C_{2} H_{5} O H}]$
$Δ H_{r} = [2 (- 393.5) - 3 (241.8) + 277.7]$
$Δ H_{r} = - 1234.7 k J / m o l e$