Consider the values for ΔH∘ in kJ mol−1 and for ΔS∘ in Jmol−1K−1 ) given for four different reactions. For which reactions will ΔG∘ increase the most (becoming more positive ) when the temperature is increased from 0∘C to 25∘C?

For ΔG∘ to become more positive, dΔG∘dT=−ΔS∘More-ve the ΔS∘, more will be the increase of ΔG∘ with temperature.

Consider the values for ΔH∘ in kJ mol−1 and for ΔS∘ in Jmol−1K−1 ) given for four different reactions. For which reactions will ΔG∘ increase the most (becoming more positive ) when the temperature is increased from 0∘C to 25∘C?

For ΔG∘ to become more positive, dΔG∘dT=−ΔS∘More-ve the ΔS∘, more will be the increase of ΔG∘ with temperature.

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Consider the values for $Δ H^{\circ} (in kJ {mol}^{- 1})$ and for $Δ S^{\circ} (in {Jmol}^{- 1} K^{- 1})$ given for four different reactions. For which reactions will $Δ G^{\circ}$ increase the most (becoming more positive ) when the temperature is increased from $0^{\circ} C$ to $25^{\circ} C$ ?

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$Δ H^{\circ} = 90, Δ S^{\circ} = 20$

$Δ H^{\circ} = - 90, Δ S^{\circ} = - 20$

$Δ H^{\circ} = - 20, Δ S^{\circ} = - 50$

$Δ H^{\circ} = 50, Δ S^{\circ} = 50$

answer is C.

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Detailed Solution

For $Δ G^{\circ}$ to become more positive, $\frac{d (Δ G^{\circ})}{d T} = - Δ S^{\circ}$

More-ve the $Δ S^{\circ}$ , more will be the increase of $Δ G^{\circ}$ with temperature.

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Consider the values for ΔH∘ in kJ mol−1 and for ΔS∘ in Jmol−1K−1 ) given for four different reactions. For which reactions will ΔG∘ increase the most (becoming more positive ) when the temperature is increased from 0∘C to 25∘C?

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