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Standard XII

Chemistry

Characteristics of Equilibrium Constant

Find enthalpy...

Question

Find enthalpy change for the reaction:

$C_{3} H_{8} (g) + H_{2} (g) \to C_{2} H_{6} (g) + C H_{4} (g)$

at $25^{\circ} C$ . The enthalpy of combustion of $H_{2}$ & $C H_{4}$ are $- 285.8$ & $- 890.0 k J / m o l$ respectively.

[Use : $Δ H_{c o m b (C_{2} H_{6}) (g)} = - 1560 k J / m o l$ ; $Δ H_{s u b (C) (s)} = 393.5 k J / m o l$ and $Δ H_{f (C_{3} H_{8}) (g)} = - 103.8 k J / m o l$ ]

-55.7

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-65.7

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-75.7

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65.7

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Solution

The correct option is A -55.7

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Similar questions

Q. The enthalpy change for the reaction

C_{3} H_{8} (g) + H_{2} (g) \to C_{2} H_{6} (g) + C H_{4} (g)

25^{o}

is -55.7 kJ / mol . Calculate the enthalpy of combustion of

C_{2} H_{6} (g)

. The enthalpy of combustion of propane is

- 2220 k J m o l^{- 1}

and enthalpy of

H_{2}

and

C H_{4}

are -285.8 KJ/mol and -890 KJ/mol respectively.

Q. The enthalpy change for the reaction

C_{3} H_{8} (g) + H_{2} (g) ⟶ C_{2} H_{6} (g) + {C H}_{4} (g)

at 25C is -55.7 KJ/mol. Calculate the enthalpy of combustion of

C_{2} H_{6} (g)

. The enthalpy of combustion of

H_{2}

and

{C H}_{4}

are -285.8 and -890.0 KJ/mol respectively. Enthalpy of combustion of propane is -2220

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

Q. Determine the enthalpy of the reaction

C_{3} H_{8} (g) + H_{2} (g) ⟶ C_{2} H_{6} (g) + C H_{4} (g)

25^{\circ} C

using the given heat of combustion values under standard conditions. The standard heat of formation of

C_{3} H_{8} (g)

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

Compound:	$H_{2} (g)$	$C H_{4} (g)$	$C_{2} H_{6} (g)$	$C (g r a p h i t e)$
$Δ H^{⊖} (k J m o l^{- 1}) :$	$- 285.8$	$- 890.0$	$- 1560.0$	$- 393.5$

Q. The enthalpy of combustion of methane graphite and dihydrogen at

298 K

are

- 890.3

m o l^{- 1}

and

- 285.8

m o l^{- 1}

respectively. Enthalpy of formation of

C H_{4} (g)

will be:

Standard enthalpy of combustion of $C H_{4}$ is $- 890 k J m o l^{- 1}$ and standard enthalpy of vaporisation of water is 40.5 kJ $m o l^{- 1}$ . Calculate the enthalpy change for the reaction :
$C H_{4 (g)} + 2 O_{2 (g)} \to C O_{2 (g)} + 2 H_{2} O_{(g)}$

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Find enthalpy change for the reaction: C3H8(g)+H2(g)→C2H6(g)+CH4(g) at 25∘C. The enthalpy of combustion of H2 & CH4 are −285.8 & −890.0kJ/mol respectively. [Use : ΔHcomb(C2H6)(g)=−1560kJ/mol; ΔHsub(C)(s)=393.5kJ/mol and ΔHf(C3H8)(g)=−103.8kJ/mol]

The correct option is A -55.7