At 27^° C , the combustion of ethane takes place according to the reaction C_2H_{6(g)} + 7/2 O_{2(g)}→2CO_{2(g)} +3H_2O_{(l)} △ E-△ H for this reactio at 27^° C will be a) +1247.1J b) -1247.1J c) -6235.5J d) +6235.5

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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}

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}

Δ H

Δ E

27^{o}

2 C H_{3} C O O^{-} ⟶ C_{2} H_{6} (g) + 2 C O_{2} (g) + 2 e^{-}

80 %

27^{\circ} C

740 t o r r

0.5 a m p

96.45

:For the reaction

$C_{2} H_{4} (g) + 3 O_{2} (g) \to 2 C O_{2} (g) + 2 H_{2} O (l);$

$Δ$ $E$ = $- 1415 k J$ . The $Δ$ H at 27 $^{0}$ C is

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