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For combustion of one mole of magnesium in an open container at 300 K and 1 bar pressure, Δ C H ⊖ = - 601 . 70 kJ mol - 1 , the magnitude of change in internal energy for the reaction is kJ . (Nearest integer) (Given : R = 8 . 3 J K - 1 mol - 1 )

Correct answer

0

Step-by-step solution

Mg s + 1 2 O 2 G ⟶ MgO S ΔH c ° = - 601 . 70 KJ / Mole ΔH ° = ΔU + ΔngRT - 601 . 70 = ΔU + - 1 2 × 8 . 3 × 300 × 10 - 3 - 601 . 7 = ΔU - 1 . 245 ΔU = - 599 . 455 KJ ΔU = 599 . 455 KJ ≈ 600

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