Chemical Thermodynamics
Intensive and extensive properties; state functions; first law; internal energy, work (PV only) and heat; enthalpy; heat capacity; standard state; Hess's law; enthalpy of reaction, fusion, vaporization, lattice enthalpy; second law; entropy; Gibbs energy; criteria of equilibrium and spontaneity.
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Take a full mock →Q1 · Chemical Thermodynamics · MEDIUM
For a reaction at 300 K, ΔH° = -60 kJ/mol and ΔS° = -200 J/K·mol. The reaction will be spontaneous when:
Q2 · Chemical Thermodynamics · HARD
For a reaction, ΔH = -120 kJ and ΔS = -400 J/K at 298 K. The minimum temperature (in K) above which the reaction becomes non-spontaneous is:
Q3 · Chemical Thermodynamics · HARD
For a reaction at 298 K, ΔH° = –92.4 kJ mol⁻¹ and ΔS° = –198.0 J K⁻¹ mol⁻¹. At what temperature (in K) will the reaction become non-spontaneous? (Answer as an integer)
Q4 · Chemical Thermodynamics · MEDIUM
For an ideal gas undergoing isothermal reversible expansion, which of the following is TRUE?
Q5 · Chemical Thermodynamics · MEDIUM
A reaction at 298 K has ΔH = −60 kJ/mol and ΔS = −150 J/(mol·K). Determine whether the reaction is spontaneous at this temperature.