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The complete combination of ethane C₂H₄(g) + 3O₂(g) → 2CO₂(g) + 2H₂O(l) the amount of heat produced as measured in bomb calorimeter is 1406 kJ mol^-1 at 300K. The minimum value of $T ∆ S$ needed to reach equilibrium is (-)…..kJ (Nearest integer) given R = 8.3JK^-1mol^-1

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answer is 1411.

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Detailed Solution

$\begin{array}{l} ΔH = ΔE + ΔnRT \\ \begin{array}{l} = - 1406 + (- 2) \times 8.3 \times 10^{- 3} \times 300 (∵ Δn = 2 - 4 = - 2) \\ = - 1406 - 4.98 \Rightarrow ΔH = - 1411 kJ \end{array} \end{array}$

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