Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

19. Chemical Thermodynamics

Gibbs Free Energy Calculations

General Chemistry

19. Chemical Thermodynamics

Gibbs Free Energy Calculations

Previous problemNext problem

Struggling with General Chemistry?

Join thousands of students who trust us to help them ace their exams!Watch the first video

Multiple Choice

Calculate the Gibbs free energy change associated with the formation of 2.0 g of CO2 from the reaction: 2 CO(g) + O2(g) -> 2 CO2(g); given ΔG° = -514.4 kJ for the formation of 2 moles of CO2.

-11.7 kJ

-514.4 kJ

-23.4 kJ

-257.2 kJ

Previous problemNext problem

Verified step by step guidance

First, understand that the Gibbs free energy change (ΔG°) given is for the formation of 2 moles of CO2. We need to calculate the ΔG for the formation of 2.0 g of CO2.

Calculate the molar mass of CO2. The molar mass of carbon (C) is approximately 12.01 g/mol and that of oxygen (O) is approximately 16.00 g/mol. Therefore, the molar mass of CO2 is 12.01 + 2(16.00) = 44.01 g/mol.

Determine the number of moles of CO2 in 2.0 g. Use the formula: \( \text{moles of CO2} = \frac{\text{mass of CO2}}{\text{molar mass of CO2}} \). Substitute the values: \( \frac{2.0 \text{ g}}{44.01 \text{ g/mol}} \).

Calculate the Gibbs free energy change for the formation of the calculated moles of CO2. Use the proportion: \( \Delta G = \Delta G^\circ \times \frac{\text{moles of CO2}}{2 \text{ moles}} \). Substitute the values: \( -514.4 \text{ kJ} \times \frac{\text{moles of CO2}}{2} \).

Finally, solve the equation to find the Gibbs free energy change for the formation of 2.0 g of CO2. This will give you the desired ΔG value.