Chemistry - Thermodynamics - II Question with Solution | TestHub
ChemistryThermodynamics - IIFree Energy and EquilibriumMedium2 minQB
ChemistryMediumnumerical
The diamonds are formed from graphite under very high pressure. Calculate the equilibrium pressure (in 10⁴ bar) at which graphite is converted into diamond at 25°C. The densities of graphite and diamond are 2.0 and 3.0 g/cm³, respectively, and are independent of pressure. ΔG° for the conversion of graphite into diamond is 4.0 kJ/mol.
Answer:
2.00
Solution:
At equilibrium ΔG(P) = ΔG° + ΔV·P = 0. ΔV = 12/3.0 − 12/2.0 = 4.0 − 6.0 = −2.0 cm³ mol⁻¹ = −2.0×10⁻⁶ m³ mol⁻¹. P = −ΔG°/ΔV = 4000/2.0×10⁻⁶ = 2.0×10⁹ Pa = 2.0×10⁴ bar. In units of 10⁴ bar: 2.
Stream:JEESubject:ChemistryTopic:Thermodynamics - IISubtopic:Free Energy and Equilibrium
⏱ 2mℹ️ Source: QB
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