Chemical Thermodynamics
Fundamentals of thermodynamics — system and surroundings, types of system; first law of thermodynamics; concept of work, heat, internal energy and enthalpy; Hess's law; standard enthalpies of formation, combustion, neutralisation; bond dissociation enthalpy; second law of thermodynamics; entropy; Gibbs energy; spontaneity; relation between ΔG and equilibrium constant.
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Take a full mock →Q1 · Chemical Thermodynamics · EASY
A system absorbs 500 J of heat and performs 200 J of work on the surroundings. What is the change in internal energy of the system?
Q2 · Chemical Thermodynamics · MEDIUM
Given the following reactions: C(s) + O2(g) → CO2(g), ΔH = -393.5 kJ/mol H2(g) + (1/2)O2(g) → H2O(l), ΔH = -285.8 kJ/mol C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(l), ΔH = -1367 kJ/mol What is the standard enthalpy of formation of ethanol C2H5OH(l)?
Q3 · Chemical Thermodynamics · MEDIUM
For a reaction at 298 K, ΔH = +50 kJ/mol and ΔS = +150 J/(mol·K). At what temperature will the reaction become spontaneous?
Q4 · Chemical Thermodynamics · MEDIUM
For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), ΔG° = -33.0 kJ/mol at 298 K. What is the equilibrium constant K for this reaction? (R = 8.314 J/(mol·K), ln(K) = -ΔG°/RT)
Q5 · Chemical Thermodynamics · HARD
For a reaction at equilibrium, ΔG° = +5.7 kJ/mol at 298 K. The equilibrium constant K for this reaction is approximately: (R = 8.314 J/mol·K, ln 10 = 2.303)