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 ...

You visited us 17 times! Enjoying our articles? Unlock Full Access!

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}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

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

No worries! We‘ve got your back. Try BYJU‘S free classes today!

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

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

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

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

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 $C$

Suggest Corrections

Similar questions

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