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

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Multiple Choice

Consider the following reaction: CO2(g) + CCl4(g) ⇌ 2COCl2(g). Calculate ΔG for this reaction at 25 °C under these conditions: PCO2 = 0.140 atm, PCCl4 = 0.185 atm, PCOCl2 = 0.755 atm. Given that ΔG°f for CO2(g) is −394.4 kJ/mol, what is the value of ΔG?

5.2 kJ/mol

0.0 kJ/mol

−10.5 kJ/mol

−5.2 kJ/mol

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Verified step by step guidance

Identify the reaction: CO2(g) + CCl4(g) ⇌ 2COCl2(g). We need to calculate the Gibbs free energy change (ΔG) for this reaction under non-standard conditions.

Use the equation ΔG = ΔG° + RT ln(Q), where ΔG° is the standard Gibbs free energy change, R is the universal gas constant (8.314 J/mol·K), T is the temperature in Kelvin, and Q is the reaction quotient.

Convert the temperature from Celsius to Kelvin: T = 25 °C + 273.15 = 298.15 K.

Calculate the reaction quotient Q using the partial pressures: Q = (P_COCl2^2) / (P_CO2 * P_CCl4). Substitute the given pressures: P_CO2 = 0.140 atm, P_CCl4 = 0.185 atm, P_COCl2 = 0.755 atm.

Calculate ΔG° for the reaction using the standard Gibbs free energy of formation: ΔG° = 2ΔG°f(COCl2) - (ΔG°f(CO2) + ΔG°f(CCl4)). Since ΔG°f for CCl4 and COCl2 are not provided, assume they are needed to find ΔG° and proceed with the calculation of ΔG using the equation from step 2.