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Standard XII

Chemistry

Enthalpy of Combustion

For the compl...

Question

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

- 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 $- 1366.95 k J m o l^{- 1}$
$C_{2} H_{5} O H (l) + 3 O_{2} (g) \to 2 C O_{2} (g) + 3 H_{2} O (l)$
$Δ U = - 1364.47 k J / m o l$
$Δ H = Δ U + Δ n_{g} R T$
$Δ n_{g} = - 1$
$Δ H = - 1364.47 + \frac{- 1 \times 8.314 \times 298}{1000}$
[Here, value of R in unit of J must be converted into kJ]
$= - 1364.47 - 2.4776 = - 1366.9476 k J / m o l$
or =-1366.95 kJ/mol

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Similar questions

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:
(R = 8.314 kJ mol^{-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}

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. Assuming ideality the enthalpy of combustion,

Δ_{c} H

for the reaction will be:

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

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)

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For the 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 25∘C. Assuming ideality the enthalpy of combustion, ΔcH, for the reaction will be (R=8.314 Jk−1mol−1)

The correct option is A −1366.95 kJ mol−1C2H5OH(l)+3O2(g)→2CO2(g)+3H2O(l) ΔU=−1364.47 kJ/mol ΔH=ΔU+ΔngRT Δng=−1 ΔH=−1364.47+−1×8.314×2981000 [Here, value of R in unit of J must be converted into kJ] =−1364.47−2.4776=−1366.9476kJ/mol or =-1366.95 kJ/mol