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Which of the following is the formula to calculate Gibbs free energy change, ΔG?
Which of the following is the formula to calculate Gibbs free energy change, ΔG?
For reaction 1 with ΔS = +200 J/K and ΔH = 600 kJ, what can be concluded about the spontaneity of the reaction?
For reaction 1 with ΔS = +200 J/K and ΔH = 600 kJ, what can be concluded about the spontaneity of the reaction?
For reaction 2 with ΔS = -200 J/K and ΔH = -600 kJ, what can be concluded about the spontaneity of the reaction?
For reaction 2 with ΔS = -200 J/K and ΔH = -600 kJ, what can be concluded about the spontaneity of the reaction?
For reaction 3: 2N2O(g) + 3O2(g) → 4NO2(g) + 7.9 kJ, what does the positive value of ΔG indicate?
For reaction 3: 2N2O(g) + 3O2(g) → 4NO2(g) + 7.9 kJ, what does the positive value of ΔG indicate?
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For reaction 4: 2 HCl(g) + 185 kJ → H2 Starter(g) + 2 Cl2(g), what can be concluded about the spontaneity of the reaction?
For reaction 4: 2 HCl(g) + 185 kJ → H2 Starter(g) + 2 Cl2(g), what can be concluded about the spontaneity of the reaction?
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Which of the following is the formula to calculate Gibbs free energy change, ΔG?
Which of the following is the formula to calculate Gibbs free energy change, ΔG?
Signup and view all the answers
For reaction 1 with ΔS = +200 J/K and ΔH = 600 kJ, what can be concluded about the spontaneity of the reaction?
For reaction 1 with ΔS = +200 J/K and ΔH = 600 kJ, what can be concluded about the spontaneity of the reaction?
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For reaction 2 with ΔS = -200 J/K and ΔH = -600 kJ, what can be concluded about the spontaneity of the reaction?
For reaction 2 with ΔS = -200 J/K and ΔH = -600 kJ, what can be concluded about the spontaneity of the reaction?
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For reaction 3: 2N2O(g) + 3O2(g) → 4NO2(g) + 7.9 kJ, what does the positive value of ΔG indicate?
For reaction 3: 2N2O(g) + 3O2(g) → 4NO2(g) + 7.9 kJ, what does the positive value of ΔG indicate?
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For reaction 4: 2 HCl(g) + 185 kJ → H2 Starter(g) + 2 Cl2(g), what can be concluded about the spontaneity of the reaction?
For reaction 4: 2 HCl(g) + 185 kJ → H2 Starter(g) + 2 Cl2(g), what can be concluded about the spontaneity of the reaction?
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Study Notes
Gibbs Free Energy (ΔG)
- The formula to calculate Gibbs free energy change is ΔG = ΔH - TΔS, where ΔH is the enthalpy change, T is the temperature in Kelvin, and ΔS is the entropy change.
Reaction 1 Analysis
- For reaction 1, ΔS = +200 J/K and ΔH = 600 kJ.
- A positive ΔS suggests an increase in disorder, while the large positive ΔH indicates an input of energy.
- The spontaneity of the reaction cannot be conclusively determined without temperature; however, at high temperatures, the reaction may become spontaneous.
Reaction 2 Analysis
- For reaction 2, ΔS = -200 J/K and ΔH = -600 kJ.
- The negative ΔS indicates a decrease in disorder, while the negative ΔH suggests the reaction releases energy.
- This combination typically favors spontaneity, so the reaction is likely spontaneous.
Reaction 3 Analysis
- Reaction 3: 2N2O(g) + 3O2(g) → 4NO2(g) + 7.9 kJ results in a positive ΔG.
- A positive ΔG indicates that the reaction is non-spontaneous under standard conditions, meaning it requires energy input to proceed.
Reaction 4 Analysis
- Reaction 4: 2 HCl(g) + 185 kJ → H2 Starter(g) + 2 Cl2(g) involves inputting energy (185 kJ).
- The need for energy input generally indicates the reaction is non-spontaneous as written; it will require external energy to occur.
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Description
Test your knowledge of Gibbs Free Energy with this quiz! Calculate the free energy change and determine whether reactions are spontaneous or nonspontaneous based on given values of ΔH, ΔS, and temperature. Put your skills to the test and see how well you understand the concept of free energy change!
