The Haber-s process for production of ammonia involves the equilibrium- N2g-3H2g- 2NH3gAssuming -Ho and -So for the reaction do not change with temperature- which of the statements is true- -Ho-95kJ and -So-190J K -1

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Standard XII

Chemistry

Entropy

The Haber's p...

Question

The Haber's process for production of ammonia involves the equilibrium:
$N_{2} (g) + 3 H_{2} (g) ⇌ 2 {N H}_{3} (g)$
Assuming $Δ H^{o}$ and $Δ S^{o}$ for the reaction do not change with temperature, which of the statements is true?
( $Δ H^{o} = - 95 k J$ and $Δ S^{o} = - 190 J K^{- 1}$ )

Ammonia dissociates spontaneously below

500 K

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Ammonia dissociates spontaneously above

500 K

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Ammonia dissociates at all temperatures

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Ammonia does not dissociate at any temperature

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Solution

The correct option is A Ammonia dissociates spontaneously below $500 K$
$Δ G^{o} = Δ H^{o} - T Δ S^{o}$
$= - 95 \times 1000 - 500 \times (- 90)$
$= 0$
Thus at temperatures below 500K, $Δ G < 0$ .

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The Haber's process for production of ammonia involves the equilibrium:N2(g)+3H2(g)⇌2NH3(g)Assuming ΔHo and ΔSo for the reaction do not change with temperature, which of the statements is true?(ΔHo=−95kJ and ΔSo=−190JK−1)

The correct option is A Ammonia dissociates spontaneously below 500KΔGo=ΔHo−TΔSo=−95×1000−500×(−90)=0Thus at temperatures below 500K, ΔG<0.

The Haber's process for production of ammonia involves the equilibrium:
$N_{2} (g) + 3 H_{2} (g) ⇌ 2 {N H}_{3} (g)$
Assuming $Δ H^{o}$ and $Δ S^{o}$ for the reaction do not change with temperature, which of the statements is true?
( $Δ H^{o} = - 95 k J$ and $Δ S^{o} = - 190 J K^{- 1}$ )

The correct option is A Ammonia dissociates spontaneously below $500 K$
$Δ G^{o} = Δ H^{o} - T Δ S^{o}$
$= - 95 \times 1000 - 500 \times (- 90)$
$= 0$
Thus at temperatures below 500K, $Δ G < 0$ .