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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

16. Chemical Equilibrium

Equilibrium Constant K

General Chemistry

16. Chemical Equilibrium

Equilibrium Constant K

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Multiple Choice

What is the equilibrium constant, Kp, for the reaction MgCO3(s) ⇌ MgO(s) + CO2(g) at 25 °C given that ΔG° = 48.2 kJ?

Kp = 1.0 x 10^-8

Kp = 1.0 x 10^8

Kp = 1.0 x 10^3

Kp = 1.0 x 10^-3

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Verified step by step guidance

Understand that the equilibrium constant Kp is related to the Gibbs free energy change (ΔG°) of the reaction. The relationship is given by the equation:

K_{p} = e^{- \frac{ΔG°}{RT}}

, where R is the universal gas constant and T is the temperature in Kelvin.

Convert the temperature from Celsius to Kelvin. Since the temperature is given as 25 °C, use the conversion formula:

T = 25 + 273.15

Identify the value of the universal gas constant R. For calculations involving energy, R is typically

8.314 J / (mol \cdot K)

. Ensure that ΔG° is in the same units, so convert ΔG° from kJ to J by multiplying by 1000.

Substitute the values of ΔG°, R, and T into the equation for Kp:

K_{p} = e^{- \frac{48200}{8.314 \times 298.15}}

Calculate the exponent in the equation and then find the value of Kp by evaluating the expression. This will give you the equilibrium constant for the reaction at the specified temperature.