Multiple Choice
Calculate the value of ΔG° at 281.0 °C for the formation of calcium chloride from its constituent elements: Ca(s) + Cl2(g) → CaCl2(s), given that at 25.0 °C, ΔH° is -795.8 kJ/mol and ΔG° is -748.1 kJ/mol.
19. Chemical Thermodynamics
Gibbs Free Energy Calculations
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What is the equilibrium constant (K) at 305 K when the standard Gibbs free energy change (ΔG°) is +1.61 kJ/mol?
A
1.25
B
0.78
C
0.45
D
0.62
Verified step by step guidance1
Understand the relationship between Gibbs free energy change (ΔG°) and the equilibrium constant (K) using the equation: ΔG° = -RT ln(K), where R is the universal gas constant (8.314 J/mol·K) and T is the temperature in Kelvin.
Convert the standard Gibbs free energy change (ΔG°) from kJ/mol to J/mol by multiplying by 1000, since the gas constant R is in J/mol·K.
Rearrange the equation to solve for the equilibrium constant (K): K = e^(-ΔG° / RT).
Substitute the given values into the equation: ΔG° = 1610 J/mol, R = 8.314 J/mol·K, and T = 305 K.
Calculate the value of K by evaluating the expression: K = e^(-1610 / (8.314 * 305)).
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