For complete combustion of ethanol- the amount of heat produced as measured in a bomb calorimeter is 1364-47 kJ mol-1 at 25-C- C2H5OHl-3O2g- 2CO2g-3H2Ol Assuming ideality the enthalpy of combustion- - cH- for the reaction will be- -R-8-314 J mol-1-

The correct option is A 1366.95 kJ mol^ 1 C_2H_5OH(l)+3O_2(g)→ 2CO_2(g)+3H_2O(l), Δ E= 1364.47 kJ mol^ 1 Δ H=? T=298K Δ n_g= 1 ...

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Byju's Answer

Standard XII

Chemistry

Difference between Internal Energy and Enthalpy

For complete ...

Question

For complete combustion of ethanol, the amount of heat produced as measured in a bomb calorimeter is $1364.47 k J m o l^{- 1}$ at $25^{\circ} C$ .

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

Assuming ideality the enthalpy of combustion, $Δ_{c} H,$ for the reaction will be:
$[R = 8.314 J m o l^{- 1}]$

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

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

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

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

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Solution

The correct option is A $- 1366.95 k J m o l^{- 1}$
$C_{2} H_{5} O H (l) + 3 O_{2} (g) \to 2 C O_{2} (g) + 3 H_{2} O (l),$

$Δ E = - 1364.47 k J m o l^{- 1}$
$Δ H = ?$
$T = 298 K$
$Δ n_{g} = - 1$ $∵$ complete combution

$R = 8.314 J m o l^{- 1} = \frac{8.314}{1000} k J m o l^{- 1}$

$∵ Δ H = Δ E + P Δ V$

but, $P Δ V = Δ n_{g} R T$

$∵ Δ H = Δ E + Δ n_{g} R T$

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

$Δ H = - 1366.95 k J m o l^{- 1}$

Hence, the correct option is $C$

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