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Electrochemical Cells, Galvanic Cells

The enthalpy ...

Question

The enthalpy change for the reaction
$C_{2} H_{4} (g) + H_{2} (g) ⟶ C_{2} H_{6}$
is $- 620 J$ when 100ml of ethylene and 100 ml of $H_{2}$ react. Calculate volume work and $Δ U .$

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Solution

$C_{2} H_{4} (g) + H_{2} (g) ⟶ C_{2} H_{6} (g) I n i t i a l - 100 m l 100 m l 100 m l f i n a l - 00100 m l Δ H = - 620 J Δ H = Δ U + Δ n g R T - (P Δ V)$

$W o r k = 1 (100 - (100 + 100)) \times 10^{- 3} = 100 \times 10^{- 3} = 0.1 L a t m = 10.13 J [1 L a t m = 101.35]$

$∴ Δ U = - 620 + 10.13 = - 609.9 J$

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