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A reaction has $\Delta H = -100$ kJ and $\Delta S = +200$ J/K. At $T = 298$ K, $\Delta G$ is:
A$+100$ kJ, ignoring the entropy term in the formula
B$-59.6$ kJ, taking $T\Delta S$ with the wrong sign
C$-159.6$ kJ, since $\Delta G = -100 - 298\cdot 0.2 = -159.6$
D$+59.6$ kJ, summing two positive terms together here
Answer & Solution
Correct answer: C. $-159.6$ kJ, since $\Delta G = -100 - 298\cdot 0.2 = -159.6$
$\Delta G = -100 - 298\cdot 0.2 = -100 - 59.6 = -159.6$ kJ.
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