For the complete combustion of ethanol- C 2 H s OH l -3 O 2 g -2 CO 2-2 H 2 O l the amount of heat produced as measuredinthe bomb calorimeter is 1364-47 kJ mol -1 at 25- C- Assuming ideality- the enthalpy of combustion - C H for the reaction will be - R -8-314 -JK -1 mol -1-A- -1350-50 kJ mol -1B- -1366-95 kJ mol -1C- 1361-95 kJ mol -1D- 1460-50 kJ mol -1

The correct option is B – 1366.95 kJ mol^−1 C_2 H_5 OH (l) + 3 O_2 (g) → + 2CO_2 + 3H_2O (l) Amount of heat produced in the bomb calorimeter = ΔU = 1364.47 kJ ...

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Byju's Answer

Standard XII

Chemistry

Enthalpy

For the compl...

Question

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 $J K^{- 1} m o l^{- 1}$ ]

$- 1366.95 k J m o l^{- 1}$

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$1361.95 k J m o l^{- 1}$

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$1460.50 k J m o l^{- 1}$

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$- 1350.50 k J m o l^{- 1}$

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Solution

The correct option is A
$- 1366.95 k J m o l^{- 1}$

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

Amount of heat produced in the bomb calorimeter = $Δ$ U =- 1364.47 kJ $m o l^{- 1}$

Enthalpy of a combustion reaction is: $Δ H = Δ U + Δ n_{g} R T$

Where , $Δ$ U = internal energy

$Δ n_{g}$ = moles of gas (products -reacants), R = Gas constant=, T = Temperature in K

As per the equation,

$Δ n_{g} = 2 - 3 = - 1$

$T = 25^{\circ} C = 25 + 273 K$

$\Rightarrow T = 298 K$

Thus, $Δ H = - 1364.47 + [\frac{(- 1) \times 8.314 \times 298}{1000}]$

$Δ H = - 1364.47 - 2.477 = - 1366.947 k J m o l^{- 1}$

Hence, they enthalpy of combustion , $Δ_{c} H$ for the given reaction will be - 1366.95 kJ $m o l^{- 1}$

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Similar questions

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

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Δ_{c} H

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For the complete combustion of ethanol, C2HsOH(l)+3O2(g)→+2CO2+2H2O(l) the amount of heat produced as measured inthe bomb calorimeter is 1364.47 kJ mol−1 at 25∘C. Assuming ideality, the enthalpy of combustion ΔcH for the reaction will be [ R = 8.314 JK−1mol−1 ]