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

Question

For combustion of one mole of magnesium in an open container at

300K

and

1

bar pressure,

{\Delta}_{C}{H}^{⊖} = - 601 . 70kJ{mol}^{- 1}

, the magnitude of change in internal energy for the reaction is

kJ

. (Nearest integer)
(Given :

R = 8 . 3J{K}^{- 1}{mol}^{- 1}

)

Quantrex Academy · Accepted Answer

Correct answer: 0

Mg _ (s) + (1)/(2) O _ 2(G) ⟶ MgO(S) Δ H _ c ^ ° = - 601 . 70KJ / Mole Δ H ° = Δ U + Δ ngRT - 601 . 70 = Δ U + [(- (1)/(2)) × 8 . 3 × 300] × 10 ^ - 3 - 601 . 7 = Δ U - 1 . 245 Δ U = - 599 . 455KJ |Δ U| = 599 . 455KJ 600

For combustion of one mole of magnesium in an open container at...

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