Medical University Entrance Examination (Bulgaria) · General and Inorganic Chemistry

Chemical Thermodynamics, Kinetics, and Equilibrium

35 practice questions, each with the answer and an explanation.

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Random questions from this topic, one at a time. You see the answer and the explanation straight after each one.

All 35 questions

  1. What thermodynamic criterion determines whether a chemical process is spontaneous at constant temperature and pressure?
  2. Under which thermodynamic conditions is a chemical reaction spontaneous at all temperatures?
  3. How does adding a chemical catalyst accelerate the rate of a chemical reaction?
  4. What are the units of the rate constant (k) for a second-order chemical reaction?
  5. If doubling the concentration of reactant A quadruples the initial rate of reaction, what is the reaction order with respect to A?
  6. According to the Arrhenius equation (k = A * e^(-Ea / RT)), what graph yields a straight line whose slope equals -Ea / R?
  7. For the exothermic Haber process reaction: N2(g) + 3 H2(g) <=> 2 NH3(g) (Delta H = -92 kJ/mol), how will increasing the total pressure at constant temperature affect the equilibrium position?
  8. How does an increase in temperature affect the equilibrium constant (Kc) of an endothermic chemical reaction (Delta H > 0)?
  9. What is the pH of an aqueous 0.0010 M hydrochloric acid (HCl) solution at 25 degrees Celsius?
  10. What is the pH of an aqueous 0.010 M sodium hydroxide (NaOH) solution at 25 degrees Celsius (where Kw = 1.0 x 10^-14)?
  11. What is the Henderson-Hasselbalch equation used to calculate the pH of a buffer solution composed of weak acid HA and conjugate base A-?
  12. Which combination of substances forms an effective buffer solution resistant to pH changes upon addition of small amounts of strong acid or base?
  13. What is the aqueous pH of a 0.10 M sodium acetate (CH3COONa) solution at 25 degrees Celsius?
  14. What is the solubility product expression (Ksp) for silver chromate (Ag2CrO4) dissolving in pure water?
  15. How does adding sodium chloride (NaCl) affect the molar solubility of silver chloride (AgCl) in water?
  16. In the standard galvanic cell Zn(s) | Zn2+(aq) || Cu2+(aq) | Cu(s), where do oxidation and reduction take place?
  17. Given standard reduction potentials E°(Zn2+/Zn) = -0.76 V and E°(Cu2+/Cu) = +0.34 V, what is the standard electromotive force (E°cell) of the Daniell cell?
  18. What is the function of the salt bridge in a galvanic (voltaic) electrochemical cell?
  19. How does the cell potential (Ecell) change as a galvanic cell discharges and approaches dynamic chemical equilibrium?
  20. According to the Bronsted-Lowry definition, what is a conjugate acid-base pair in the reaction: NH3 + H2O <=> NH4+ + OH-?
  21. Which definition identifies a Lewis acid as an electron-pair acceptor?
  22. What is the relationship between Delta G° and the equilibrium constant K at temperature T?
  23. What is the half-life equation for a first-order chemical reaction with rate constant k?
  24. How many coulombs of electric charge correspond to one Faraday of charge (one mole of electrons)?
  25. Which acid is classified as diprotic, meaning it can donate two protons per molecule in aqueous solution?
  26. What happens to the ionization constant of water (Kw) as the temperature increases from 25 degrees Celsius to 50 degrees Celsius?
  27. What is the standard state enthalpy of formation (Delta H°f) for any pure chemical element in its most stable reference physical form at 298 K?
  28. Which state function change is calculated by Hess's law by summing the enthalpies of intermediate reaction steps?
  29. What is the term for a solution that contains the maximum possible concentration of dissolved solute in dynamic equilibrium with undissolved solid at a given temperature?
  30. In a redox titration, which chemical species undergoes reduction while causing another species to be oxidized?
  31. What is the oxidation number of oxygen in hydrogen peroxide (H2O2)?
  32. Which law states that the total entropy of an isolated system always increases over time in any spontaneous thermodynamic process?
  33. What is the molar solubility (s) of barium sulfate (BaSO4) in pure water if its solubility product constant Ksp is 1.0 x 10^-10 at 25 degrees Celsius?
  34. What chemical color change is observed when phenolphthalein indicator is added to an aqueous sodium hydroxide solution?
  35. Why does a mixture of copper turnings and concentrated nitric acid produce a dark brown gas rather than hydrogen gas?

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