Standard enthalpy and standard entropy change for the oxidation of ${N H}_{3}$ at $298 K$ are ${- 382.64 k J m o l}^{- 1}$ and ${- 145.6 J m o l}^{- 1}$ respectively. The standard Gibbs energy change for the same reaction at $298 K$ is:

{- 221.1 k J m o l}^{- 1}

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{- 339.3 k J m o l}^{- 1}

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{- 439.3 k J m o l}^{- 1}

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{- 523.2 k J m o l}^{- 1}

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Solution

The correct option is B ${- 339.3 k J m o l}^{- 1}$
${Δ G}^{o} = {Δ H}^{o} - {T Δ S}^{o}$

$= - 382.64 - 298 \times (- 145.6 \times 10^{- 3})$

$= - 339.3 k J {m o l}^{- 1}$

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Similar questions

Q. Standard enthalpy and standard entropy changes for the oxidation of ammonia at 298 K are382.64 kJ mol

^{- 1}

and 145.6 JK

^{- 1}

mol

^{- 1}

, respectively. Standard Gibbs energy change for the same reaction at 298 K is:

Standard enthalpy and standard entropy for the oxidation of $N H_{3}$ at $298$ K are $- 382.64$ $kJ {mol}^{- 1}$ and $- 145.6$ $J {mol}^{- 1} K^{- 1}$ respectively. Standard free energy change (in ${kJ mol}^{- 1}$ ) for the same reaction at $298$ K is: