Open Question
For the reaction 2 Hg(l) O2 → 2HgO(s), ∆H = -43 kcal/mol (-180 kJ/mol).Under what conditions would you expect this process to be spontaneous?
7. Energy, Rate and Equilibrium
Gibbs Free Energy (Simplified)
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A particular reaction has ΔG = –350 kJ and ΔS = –350 J/K at 24°C. How much heat will be released/absorbed?
A
–1.04×105 kJ
B
–454 kJ
C
–8.75×103 kJ
D
246 kJ
E
+454 kJ
F
–246 kJ
Verified step by step guidance1
First, convert the temperature from Celsius to Kelvin. The formula is: T(K) = T(°C) + 273.15. So, 24°C becomes 297.15 K.
Next, convert the entropy change (ΔS) from J/K to kJ/K to match the units of ΔG. Since 1 kJ = 1000 J, divide ΔS by 1000: ΔS = -350 J/K ÷ 1000 = -0.35 kJ/K.
Use the Gibbs free energy equation: ΔG = ΔH - TΔS, where ΔG is the change in Gibbs free energy, ΔH is the change in enthalpy (heat released or absorbed), and T is the temperature in Kelvin.
Rearrange the equation to solve for ΔH: ΔH = ΔG + TΔS.
Substitute the known values into the equation: ΔH = -350 kJ + (297.15 K)(-0.35 kJ/K). Calculate the result to find the amount of heat released or absorbed.
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