At 298 K, ΔH° for this reaction is -137.5 kJ/mol, and ΔS° is +120.5 J/K. What is the value of ΔG° (in kJ/mol) at 25 °C for the following the reaction? C₂H₄ (g) + H₂ (g) → C₂H₆ (g)
At 298 K, ΔH° for this reaction is -137.5 kJ/mol, and ΔS° is +120.5 J/K. What is the value of ΔG° (in kJ/mol) at 25 °C for the following the reaction? C₂H₄ (g) + H₂ (g) → C₂H₆ (g)
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Chapter18: Thermodynamics And Equilibrium
Section: Chapter Questions
Problem 18.104QP
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1. At 298 K, ΔH° for this reaction is -137.5 kJ/mol, and ΔS° is +120.5 J/K. What is the value of ΔG° (in kJ/mol) at 25 °C for the following the reaction?
C₂H₄ (g) + H₂ (g) → C₂H₆ (g)
2.
Consider the boiling of liquid water at –10°C. For this process what are the signs for ∆H, ∆S, and ∆G? (Hint: The normal boiling point of water is 100°C.)
A) ∆H is +, ∆S is -, and ∆G is 0.
B) ∆H is -, ∆S is +, and ∆G is 0.
C) ∆H is -, ∆S is +, and ∆G is -.
D) ∆H is +, ∆S is +, and ∆G is +.
E) ∆H is -, ∆S is -, and ∆G is -.
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