7. Energy, Rate and Equilibrium
Gibbs Free Energy (Simplified)
7. Energy, Rate and Equilibrium
Gibbs Free Energy (Simplified)
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Practice this topic
- Multiple Choice
What are the signs of ∆H, ∆S and ∆G for the spontaneous conversion of a solid into gas?
221views1rank - Multiple Choice
Consider the combustion of butane gas and predict the signs of ΔS, ΔH and ∆G.
C4H10(g) + 13/2 O2(g) ⟶ 4 CO2(g) + 5 H2O(g)
252views1rank - Multiple Choice
A particular reaction has ΔG = –350 kJ and ΔS = –350 J/K at 24°C. How much heat will be released/absorbed?
235views1rank - Multiple Choice
For a reaction in which ΔH = 125 kJ and ΔS = 325 J/K, determine the temperature in Celsius above which the reaction is spontaneous.
258views - Textbook QuestionThe change of state from liquid H2O to gaseous H2O has ∆H = +9.72 kcal/mol(+40.7 kJ/mol) and ∆S = -26.1 cal/(mol • K) [-109 J/(mol •K)]. Is the change from liquid to gaseous H2O favored or unfavored by ∆H? By ∆S?181views
- Textbook QuestionThe change of state from liquid H2O to gaseous H2O has ∆H = +9.72 kcal/mol(+40.7 kJ/mol) and ∆S = -26.1 cal/(mol • K) [-109 J/(mol •K)]. What are the values of ∆H and ∆S (in kcal/mol and kJ/mol) for the change from gaseous to liquid H2O?248views
- Textbook QuestionTwo curves are shown in the following energy diagram:
Which curve represents the spontaneous reaction, and which the nonspontaneous? 363views - Textbook QuestionThe following diagram portrays a reaction of the type A(s) → B(g) + C(g), where the different-colored spheres represent different molecular structures. Assume that the reaction has ∆H = +9.1 kcal/mol (+38.1 kJ/mol). Is the reaction likely to be spontaneous at all temperatures, nonspontaneous at all temperatures, or spontaneous at some but nonspontaneous at others?338views