The values of Delta H and Delta S for the rea | vedclass

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(B) For a reaction to be spontaneous,the Gibbs free energy change $\Delta G$ must be negative $(\Delta G < 0)$.Given: $\Delta H = 170 \ kJ = 170000 \

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$1110$

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(B) For a reaction to be spontaneous,the Gibbs free energy change $\Delta G$ must be negative $(\Delta G Given: $\Delta H = 170 \ kJ = 170000 \ J$ and $\Delta S = 170 \ J \ K^{-1}$.Using the relation $\Delta G = \Delta H - T \Delta S$,for spontaneity:$\Delta H - T \Delta S $\Delta H $T > \frac{\Delta H}{\Delta S}$$T > \frac{170000 \ J}{170 \ J \ K^{-1}}$$T > 1000 \ K$.Among the given options,the reaction becomes spontaneous at temperatures above $1000 \ K$,and $1110 \ K$ is the only value satisfying this condition.

The values of $\Delta H$ and $\Delta S$ for the reaction,$C_{(graphite)} + CO_{2(g)} \rightarrow 2CO_{(g)}$ are $170 \ kJ$ and $170 \ J \ K^{-1}$ respectively. This reaction will be spontaneous at temperatures greater than ............ $K$.

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