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Enthalpy of Combustion

Which of the ...

Question

Which of the following equations corresponds to the enthalpy of combustion at $298 K$ ?

C_{2} H_{6} (g) + 7 / 2 O_{2} (g) ⟶ 2 C O_{2} (g) + 3 H_{2} O (g)

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2 C_{2} H_{6} (g) + 7 O_{2} (g) ⟶ 4 C O_{2} (g) + 6 H_{2} O (g)

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C_{2} H_{6} (g) + 7 / 2 O_{2} (g) ⟶ 2 C O_{2} (g) + 3 H_{2} O (l)

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2 C_{2} H_{6} (g) + 7 O_{2} (g) ⟶ 4 C O_{2} (g) + 6 H_{2} O (l)

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Solution

The correct option is C $C_{2} H_{6} (g) + 7 / 2 O_{2} (g) ⟶ 2 C O_{2} (g) + 3 H_{2} O (l)$
As we know, combustion of one mole of reactants gives products in standard state or most stable state.
$C_{2} H_{6} (g) + 7 / 2 O_{2} (g) ⟶ 2 C O_{2} (g) + 3 H_{2} O (l)$

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Similar questions

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

δ E - δ H

27^{0}

27^{o}

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

Δ E - Δ H

27^{o}

25^{o} C

C_{2} H_{6} (g) + 7 / 2 O_{2} (g) \to 2 C O_{2} (g) + 3 H_{2} O (1); Δ G^{o} = - 1467 k J

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

25^{0} C

Δ U 25^{0} C

C_{2} H_{5} O H (l) + \frac{7}{2} O_{2} (g) \to 2 C O_{2} (g) + 3 H_{2} O (g)

1 a t m

298 K

C_{4} H_{10} (g) + \frac{13}{2} O_{2} (g) \to 4 C O_{2} (g) + 5 H_{2} O (l) △ G^{\circ} = - 2746 k J / m o l

E^{\circ}

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