The heat of combustion of ethanol determined by a bomb calorimeter is -670-48 kcal mol-1 at 250C- What is - U 250C for the following reaction- C2H5OHl-72O2g- 2CO2g-3H2Og

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Standard XII

Chemistry

Enthalpy of Combustion

The heat of c...

Question

The heat of combustion of ethanol determined by a bomb calorimeter is $- 670.48 k c a l m o l^{- 1}$ at $25^{0} C$ . What is $Δ U 25^{0} C$ for the following reaction?
$C_{2} H_{5} O H (l) + \frac{7}{2} O_{2} (g) \to 2 C O_{2} (g) + 3 H_{2} O (g)$

-335.24 kcal

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-669.28 kcal

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-670.48 kcal

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+670.48 kcal

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Solution

The correct option is A -335.24 kcal
$Δ H = Δ E + n_{g} R T$
$Δ E = Δ H - n_{g} R T$
$Δ E = - 670.48 + 2 \times 2 \times 298 = - 335.24 K c a l$

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Similar questions

Q. The heat of combustion of ethanal determined in a bomb calorimeter is

- 670.48 K

Cals

{m o l e}^{- 1}

25^{o} C

.What is

Δ H

25^{o} C

for the reaction:

Q. The heat of formation of

C_{2} H_{5} O H (l)

- 66 k c a l m o l^{- 1}

. The heat of combustion of

C H_{3} O C H_{3} (g)

- 348 k c a l m o l^{- 1}

△ H_{f}

for

H_{2} O

and

C O_{2}

are

- 68 k c a l m o l^{- 1}

and

- 94 k c a l m o l^{- 1}

respectively.
Then, the

△ H

for the reaction

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

is:

Q. The heat of formation of

C_{2} H_{5} O H (l)

is -66 kcal/mole. The heat of combustion of

C H_{3} O C H_{3} (g)

is -348 kcal mole,

Δ H_{f}

for

H_{2} O

and

C O_{2}

are - 68 kcal/mole and -94 kcal/mole respectively. Then determine the

Δ H

for the isomerisation reaction

C_{2} H_{5} O C H_{3} (g)

, and

Δ E

for the same are at T = 25

^{\circ}

Q. For combustion of 1 mole of benzene at

25^{0} C

, the heat of reaction at constant pressure is - 780.9 kcal. What will be the heat of reaction at constant volume?

C_{6} H_{6 (I)} + 7 \frac{1}{2} O_{2 (g)} \to 6 C O_{2 (g)} + 3 H_{2} O_{(l)}

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}]

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The heat of combustion of ethanol determined by a bomb calorimeter is −670.48kcalmol−1 at 250C. What is ΔU250C for the following reaction? C2H5OH(l)+72O2(g)→2CO2(g)+3H2O(g)

The correct option is A -335.24 kcalΔH=ΔE+ngRTΔE=ΔH−ngRTΔE=−670.48+2×2×298=−335.24Kcal

The heat of combustion of ethanol determined by a bomb calorimeter is $- 670.48 k c a l m o l^{- 1}$ at $25^{0} C$ . What is $Δ U 25^{0} C$ for the following reaction?
$C_{2} H_{5} O H (l) + \frac{7}{2} O_{2} (g) \to 2 C O_{2} (g) + 3 H_{2} O (g)$

The correct option is A -335.24 kcal
$Δ H = Δ E + n_{g} R T$
$Δ E = Δ H - n_{g} R T$
$Δ E = - 670.48 + 2 \times 2 \times 298 = - 335.24 K c a l$