Given Delta S_{Total} = -40 kJ/mol cdot K,De | vedclass

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(A) The relationship between total entropy change and system entropy change is given by: $\Delta S_{Total} = \Delta S_{System} + \Delta S_{Surrounding

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$-35$

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(A) The relationship between total entropy change and system entropy change is given by: $\Delta S_{Total} = \Delta S_{System} + \Delta S_{Surroundings}$.We know that $\Delta S_{Surroundings} = -\frac{\Delta H_{System}}{T}$.Substituting the values: $\Delta S_{Surroundings} = -\frac{2000 \ kJ/mol}{400 \ K} = -5 \ kJ/mol \cdot K$.Now,$\Delta S_{Total} = \Delta S_{System} + \Delta S_{Surroundings}$.$-40 \ kJ/mol \cdot K = \Delta S_{System} + (-5 \ kJ/mol \cdot K)$.$\Delta S_{System} = -40 + 5 = -35 \ kJ/mol \cdot K$.

Given $\Delta S_{Total} = -40 \ kJ/mol \cdot K$,$\Delta H_{System} = 2000 \ kJ/mol$,and $T = 400 \ K$. Find the value of $\Delta S_{System}$ in $kJ/mol \cdot K$.

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