You visited us 1 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard XI

Chemistry

Difference between Internal Energy and Enthalpy

For complete ...

Question

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:
(R = 8.314 kJ mol^{-1})

-1460.50 kJ

m o l^{- 1}

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

-1350.50 kJ

m o l^{- 1}

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

-1366.95 kJ

m o l^{- 1}

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

-1361.95 kJ

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 C -1366.95 kJ $m o l^{- 1}$
$C_{2} H_{5} O H (1) + 3 O_{2} (g) \to 2 C O_{2} (g) + 3 H_{2} O (l)$
$△ U = - 1364.47 k J / m o l e$
$△ H = ?$
T = 298 K
$△ n_{g} = (2 - 3 = - 1)$
$∵ △ H = △ U + △ n_{g} R T$
So, $△ H$ = -1366.95 kJ/mole

Suggest Corrections

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

. Assuming ideality the enthalpy of combustion,

Δ_{c} H

, for the reaction will be

(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}

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}]

Q. For complete combustion of ethanol

C_{2} H_{5} O H (l) + 3 O_{2} (g) ⟶ 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}

25^{o} C

. Assuming ideality the enthalpy of combustion,

Δ_{c} H

for the reaction will be:

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

Q. 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)

O_{2}

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

1364.47 k J / m o l

298 K

. Assuming ideality, calculate the enthalpy of combustion,

Δ H c

, for the reaction.

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

Join BYJU'S Learning Program

For complete combustion of ethanol, C2H5OH(l)+3O2(g)→2CO2(g)+3H2O(l), the amount of heat produced as measured in bomb calorimeter, is 1364.47 kJ mol−1 at 25oC. Assuming ideality the enthalpy of combustion, △CH, for the reaction will be: (R = 8.314 kJ mol^{-1})

The correct option is C -1366.95 kJ mol−1C2H5OH(1)+3O2(g)→2CO2(g)+3H2O(l) △U=−1364.47kJ/mole △H=? T = 298 K △ng=(2−3=−1) ∵△H=△U+△ngRT So, △H = -1366.95 kJ/mole

The correct option is C -1366.95 kJ $m o l^{- 1}$
$C_{2} H_{5} O H (1) + 3 O_{2} (g) \to 2 C O_{2} (g) + 3 H_{2} O (l)$
$△ U = - 1364.47 k J / m o l e$
$△ H = ?$
T = 298 K
$△ n_{g} = (2 - 3 = - 1)$
$∵ △ H = △ U + △ n_{g} R T$
So, $△ H$ = -1366.95 kJ/mole