Physical Chemistry II Past Paper PDF

Physical Chemistry II - Q2 2. What is surface chemistry? (1 Point) A) Study of reactions only in bulk solutions B) Study of reactions at interfaces C) Study of the rate of reactions in gases D) Study of reaction mechanisms in all phases 3. Which of the following is NOT a t...

Physical Chemistry II - Q2 2. What is surface chemistry? (1 Point) A) Study of reactions only in bulk solutions B) Study of reactions at interfaces C) Study of the rate of reactions in gases D) Study of reaction mechanisms in all phases 3. Which of the following is NOT a type of adsorption? (1 Point) A) Physical adsorption B) Chemical adsorption C) Internal adsorption D) Electrostatic adsorption 4. In physical adsorption, the adsorbate molecules are held on the surface by which type of force? (1 Point) A) Covalent bonds B) Van der Waals forces C) Ionic bonds D) Hydrogen bonds 5. Which of the following factors does NOT affect the extent of adsorption? (1 Point) A) Temperature B) Nature of adsorbent C) Particle size of adsorbent D) Shape of the container 6. Which of the following is commonly used as a catalyst in the hydrogenation of oils? (1 Point) A) Platinum B) Nickel C) Copper D) Iron 7. Which of these statements is true for chemisorption? (1 Point) A) It is non-specific. B) It is reversible. C) It involves strong chemical bonds. D) It has no temperature dependence. 8. The Langmuir adsorption isotherm assumes that: (1 Point) A) Adsorption is multilayer. B) Adsorption occurs at specific homogeneous sites on the surface. C) Adsorption heat varies with surface coverage. D) Adsorption is always exothermic. 9. The process of increasing the surface area of a catalyst is called: (1 Point) A) Activation B) Condensation C) Deactivation D) Passivation 10. Which of the following methods is NOT used to study surface area? (1 Point) A) BET method B) X-ray diffraction C) Mercury porosimetry D) Gas adsorption 11. In the Langmuir isotherm, which of the following assumptions is NOT true? (1 Point) A) Adsorption occurs on a homogeneous surface. B) There are no interactions between adsorbed molecules. C) Adsorption can occur in multiple layers. D) Each adsorption site can hold only one molecule. 12. In the Langmuir isotherm, the constant b typically has units of: (1 Point) A) mol/Kg B) Kg/mol C) /atm D) /mol 13. Given the following chemical reaction, identify the correct stoichiometric matrix from the provided options. (1 Point) A) Option 1 B) Option 2 C) Option 3 D) Option 4 14. What is the corresponding propensity vector of the following chemical reaction? (1 Point) A 15. It is defined as the change in concentration of a reactant or product with time. (1 Point) A) rate law B) reaction rate C) reaction milage D) extent of reaction 16. Expresses the relationship of the rate of a reaction to the rate constant and the concentrations of the reactants raised to some powers (1 Point) A) rate law B) rate proportion C) law of limiting rate D) law of reaction 17. For the overall reaction, the order of each reactant is not related to the stoichiometric coefficient. However for what type of reaction does the stoichiometric coefficient is related to the order? (1 Point) A) bimolecular reaction B) unimolecular reaction C) zero order reaction D) elementary reactions 18. Question 5pointIf the half-life of a chemical species stays the same for a series of decomposition events under observation, what does it tell us about the order of reaction? (1 Point) A) no order B) zero order C) first order D) second order 19. If the half-life if doubled every time from successive events of decomposition, what is the order of reaction? (1 Point) A) zero order B) first order C) second order D) no order 20. The minimum amount of energy required to initiate a reaction. (1 Point) A) reaction initiation energy B) activation energy C) reaction step energy D) bond dissociation energy 21. For a chemical reaction to occur, the active sites of the reacting species must come into contact, but mere contact alone isn't sufficient. What additional conditions must be met for the reaction to proceed effectively? (1 Point) A) just contact and sufficient energy B) proper orientation and sufficient energy C) sufficient energy alone D) improper orientation alone 22. A chemical species that is formed in early elementary steps and consumed in later elementary step. (1 Point) A) enzyme B) intermediate C) chaperones D) mRNA 23. An approximation where the rate of change of some reactants is assumed to be zero. (1 Point) A) steady-state B) balanced-state C) equilibrium-state D) no-state 24. Which of the following equations is true for the first-order chemical reaction, A -> B with rate constant k1 (1 Point) B 25. Which of the following equations is equivalent to (1 Point) D 26. Which of the following statements about the Langmuir isotherm constant a is correct? (1 Point) A) It represents the maximum adsorption capacity per unit mass. B) It represents the temperature dependence of adsorption. C) It is the equilibrium constant of adsorption. D) It is the inverse of the adsorption rate. 27. A type of catalysis where one of the products of a reaction catalyzes itself or a related reaction, leading to an increase in the reaction rate over time (1 Point) A) Heterogeneous catalysis B) Homogenous catalysis C) Autocatalysis D) Self-catalysis 28. The study of the detailed molecular-level steps and mechanisms of chemical reactions, including the transition states and reaction intermediates involved. (1 Point) A) Microkinetics B) Macrokinetics C) Thermokinetics D) MechanoKinetics 29. The phenomenon where the rate of a chemical reaction differs when one or more isotopes of the reactants are substituted with heavier isotopes, due to differences in bond strengths and vibrational frequencies (1 Point) A) Isotope mass effect B) Light Isotope Effect C) Heavy Isotope Effect D) Kinetic Isotope Effect 30. An equation that relates the rate constant of a reaction to the temperature and activation energy of the reaction. (1 Point) A) Antoine equation B) Einstein equation C) Arrhenius equation D) Schrodinger equation 31. A high-energy, unstable state that occurs at the peak of the potential energy surface during a chemical reaction, representing the maximum energy point along the reaction pathway. (1 Point) A) Activated state B) Intermediate state C) Unstable state D) Transition state 32. A reaction where one reactant is present in excess, and its concentration remains effectively constant, allowing the rate to depend only on the concentration of the limiting reactant. (1 Point) A) Pseudo-First-Order Reaction B) Pseudo-Half-Order Reaction C) Normal-First-Order reaction D) First order reaction 33. In a Langmuir isotherm, what happens to x/m when the pressure P is very low (close to zero)? (1 Point) A) x/m is approximately zero B) x/m is approximately a/b C) x/m is approximately aP D) x/m approaches infinity 34. The Freundlich isotherm is used to describe: (1 Point) A) Monolayer adsorption on a homogeneous surface B) Multilayer adsorption on a heterogeneous surface C) Adsorption with strong adsorbate-adsorbate interactions D) Adsorption only at high pressures 35. The Chemical Master Equation (CME) is used to describe: (1 Point) A) The quantum mechanical behavior of molecules B) The macroscopic properties of chemical reactions C) The stochastic evolution of molecule populations in reaction networks D) The thermodynamics of reversible reactions 36. In the context of the CME, which of the following best describes the term "state"? (1 Point) A) The temperature and pressure of the system B) The set of species and their concentrations C) The set of species and their discrete molecular counts D) The rate constants of the reactions 37. The CME is particularly useful for systems where: (1 Point) A) The concentration of reactants is high B) The number of molecules is low C) The reactions are at equilibrium D) The reactions are strictly deterministic 38. Which of the following mathematical approaches is typically used to solve the CME for complex systems? (1 Point) A) Gillespie’s algorithm B) Classical differential equations C) Thermodynamic equilibrium calculations D) Quantum mechanics 39. the CME describes changes in the probability distribution of molecular counts over time. This is represented by: (1 Point A) A single differential equation B) A set of coupled differential equations C) A reaction rate equation D) A Hamiltonian equation 40. Which of the following is an assumption in the derivation of the CME? (1 Point) A) The number of molecules is infinite. B) The system is in macroscopic thermodynamic equilibrium. C) Molecules are continuously distributed. D) Reactions are stochastic events 41. The CME is often approximated by the Fokker-Planck equation when: (1 Point) A) The reaction network is deterministic. B) The reactions are at low pressure. C) The system is at high energy and with few molecules D) large number of molecules with small fluctuations 42. What is the main limitation of the CME in practical applications? (1 Point) A) It only applies to macroscopic systems. B) It ignores the discrete nature of molecules C) requires extensive computing resources for complex networks. D) It can only be solved exactly for single-molecule systems. 43. Which algorithm is commonly used to simulate the stochastic trajectories implied by the CME? (1 Point) A) Newton-Raphson method B) Euler's method C) stochastic simulation algorithm (SSA) D) Finite element method 44. The CME typically requires knowledge of: (1 Point) A) Macroscopic concentrations rather than discrete molecule counts B) Quantum states of each reactant C) Pressure, temperature, and rate constants only D) Rate constants and molecular populations of reactants 45. The Chemical Langevin Equation (CLE) is used to describe: (1 Point) A) The deterministic behavior of chemical reactions B) The stochastic dynamics of molecular populations with noise C) Quantum mechanical effects in chemical systems D) The thermodynamic equilibrium of reactions 46. The CLE can be seen as an approximation to: (1 Point) A) The Schrodinger Equation B) The Chemical Master Equation (CME) C) The Arrhenius Equation D) The Ideal Gas Law 47. The Chemical Langevin Equation includes a noise term to account for: (1 Point) A) The average rate of reaction B) Quantum fluctuations C) Thermal noise and fluctuations in molecule numbers D) Pressure changes 48. Which of the following methods is commonly used to numerically solve the Chemical Langevin Equation? (1 Point) A) Runge-Kutta method B) Euler-Maruyama method C) Newton’s method D) Fourier transform 49. The CLE is derived by adding noise to which type of equations? (1 Point) A) Quantum mechanics equations B) Deterministic rate equation C) Schrodinger equations D) Gas laws 50. Deterministic chemical kinetics generally describes? (1 Point) A) The probabilistic behavior of individual molecules B) The average behavior of large numbers of molecules C) Quantum mechanical effects in reactions D) Non-chemical systems only 51. In deterministic kinetics, reaction rates are typically described using: (1 Point) A) Probability distributions B) Rate equations or ordinary differential equations (ODEs) C) Random number generators D) Quantum wavefunctions 52. The rate of a reaction, according to deterministic chemical kinetics, depends on: (1 Point) A) The number of collisions only B) The concentration of reactants C) The final product concentration D) Temperature only 53. Transport processes primarily deal with: (1 Point) A) The movement of particles due to external fields B) The transfer of mass, energy, or momentum C) The creation of new chemical compound D) The transformation of matter into energy 54. In diffusion, molecules move from: (1 Point) A) Areas of low concentration to high concentration B) Low temperatures to high temperatures C) Areas of high concentration to low concentration D) Solid state to gas state 55. Which equation is commonly used to describe diffusion? (1 Point) A) Arrhenius equation B) Fick's law C) Ideal gas law D) Boltzmann equation 56. Which of the following is NOT a type of transport process? (1 Point) A) Diffusion B) Conduction C) Radiation D) Synthesis