The temperature in K at which \(\Delta G = 0\), for a given reaction with \(\Delta H = -20.5 \text{ kJ mol}^{-1}\) and \(\Delta S = -50.0 \text{ J K}^{-1} \text{ mol}^{-1}\) is:
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Always double-check your unit scales! Mixing \(\text{kJ}\) and \(\text{J}\) is a classic trap. Notice that if you forgot to multiply by \(1000\), you would evaluate \(\frac{-20.5}{-50} = 0.41\), or if you inverted the fraction, you would get \(2.44\) (matching choice 3). Keeping track of your unit multipliers keeps these calculation slip-ups at bay.