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10 questions from this quiz
ΔG<0\Delta G < 0ΔG<0
ΔG=ΔH−TΔS\Delta G = \Delta H - T\Delta SΔG=ΔH−TΔS
0.1610.1610.161 kJ K⁻¹ mol⁻¹
298 K
ΔH\Delta HΔH negative, ΔS\Delta SΔS positive
ΔH\Delta HΔH positive, ΔS\Delta SΔS negative
It becomes larger and more significant
T=ΔH/ΔST = \Delta H / \Delta ST=ΔH/ΔS
The reaction rate or mechanism
No effect - catalysts don't change ΔG\Delta GΔG
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