Dessicants (drying agents) can often be regenerated by heating, although it is generally not economically worthwhile to do so. A dessicant that is commonly regenerated is CaSO42H2O: CaSO4⋅2H2O(s) → CaSO4(s) + 2H2O(g) ΔH∘298 =25.1 kJ/mol, ΔS∘298 =69.3 J/(mol⋅K) Regeneration is carried out at 250°C. What is ΔG° (kJ/mol) for this reaction? What is the equilibrium constant at 25°C? What is the ratio K250°C/K25°C? What is the equilibrium constant at 250°C?
Dessicants (drying agents) can often be regenerated by heating, although it is generally not economically worthwhile to do so. A dessicant that is commonly regenerated is CaSO42H2O: CaSO4⋅2H2O(s) → CaSO4(s) + 2H2O(g) ΔH∘298 =25.1 kJ/mol, ΔS∘298 =69.3 J/(mol⋅K) Regeneration is carried out at 250°C. What is ΔG° (kJ/mol) for this reaction? What is the equilibrium constant at 25°C? What is the ratio K250°C/K25°C? What is the equilibrium constant at 250°C?
General Chemistry - Standalone book (MindTap Course List)
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Chapter6: Thermochemisty
Section: Chapter Questions
Problem 6.132QP
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Dessicants (drying agents) can often be regenerated by heating, although it is generally not economically worthwhile to do so. A dessicant that is commonly regenerated is CaSO42H2O:
CaSO4⋅2H2O(s) → CaSO4(s) + 2H2O(g)
ΔH∘298 =25.1 kJ/mol, ΔS∘298 =69.3 J/(mol⋅K)
Regeneration is carried out at 250°C.
- What is ΔG° (kJ/mol) for this reaction?
- What is the equilibrium constant at 25°C?
- What is the ratio K250°C/K25°C?
- What is the equilibrium constant at 250°C?
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