For complete combustion of ethanol
$C_{2} H_{2} O H (l) + 3 O_{2} (g) (g i v e s) 2 C O_{2} (g) + 3 H_{2} O (l)$ in $O_{2}$ , the amount of heat produced as measured in bomb calorimeter, is $1364.47 k J / m o l$ at $298 K$ . Assuming ideality, calculate the enthalpy of combustion, $Δ H c$ , for the reaction.

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Solution

Heat produced $(Δ U) = - 1364.47$ kJ/mol
(exothermic)
$Δ H_{C} = Δ U + Δ n R T \to$ entahlpy of combustion
$Δ n =$ (gaseous moles of product) $-$ (gaseous moles of reactants)
$= 2 - 3$
$Δ n = - 1$
$∴ Δ H_{C} = - 1364.47 - 1 \times 8.314 \times 298 \times 10^{- 3}$
$= (- 1364.47 - 2.48)$
$Δ H_{C} = - 1366.95$ kJ/mol
Given equation: $C_{2} H_{5} O H (l) + 3 O_{2} (g) \to 2 C O_{2} (g) + 3 H_{2} O (l)$ .

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Q. For complete combustion of ethanol,

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

the amount of heat produced as measured in bomb calorimeter, is 1364.47 kJ

m o l^{- 1} a t 25^{o} C .

Assuming ideality the enthalpy of combustion,

△_{C} H,

for the reaction will be:
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Q. For the complete combustion of ethanol,

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

, the amount of heat produced as measured in bomb calorimeter, is

1364.47 k J m o l^{- 1} a t 25^{\circ} C

. Assuming ideality the enthalpy of combustion,

Δ_{c} H

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(R = 8.314 J k^{- 1} m o l^{- 1})

For complete combustion of ethanol, the amount of heat produced as measured in a bomb calorimeter is

1364.47 k J m o l^{- 1}

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

Assuming ideality the enthalpy of combustion,

Δ_{c} H,

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

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For the complete combustion of ethanol, $C_{2} H_{s} O H (l) + 3 O_{2} (g) \to + 2 C O_{2} + 2 H_{2} O (l)$ the amount of heat produced as measured inthe bomb calorimeter is 1364.47 kJ $m o l^{- 1} a t 25^{\circ} C .$ Assuming ideality, the enthalpy of combustion $Δ_{c} H$ for the reaction will be [ R = 8.314 $J K^{- 1} m o l^{- 1}$ ]

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For complete combustion of ethanolC2H2OH(l)+3O2(g)(gives)2CO2(g)+3H2O(l) in O2, the amount of heat produced as measured in bomb calorimeter, is 1364.47 kJ/mol at 298 K. Assuming ideality, calculate the enthalpy of combustion, ΔHc, for the reaction.

Heat produced (ΔU)=−1364.47 kJ/mol(exothermic)ΔHC=ΔU+ΔnRT→ entahlpy of combustionΔn=(gaseous moles of product)−(gaseous moles of reactants)=2−3Δn=−1∴ΔHC=−1364.47−1×8.314×298×10−3=(−1364.47−2.48)ΔHC=−1366.95 kJ/molGiven equation: C2H5OH(l)+3O2(g)→2CO2(g)+3H2O(l).