First law of thermodynamics, internal energy and enthalpy, heat capacity, Hess's law, enthalpies of dissociation combustion formation atomization sublimation phase transition hydration ionization and solution - One Line Questions

1. The enthalpy of neutralization of a strong acid by a strong base is approximately: — -57.3 kJ/mol
2. Heat capacity (C) is defined as the amount of heat required to raise the temperature of a substance by: — 1 degree Celsius or 1 Kelvin
3. Specific heat capacity is defined as the amount of heat required to raise the temperature of 1 gram of a substance by: — 1 degree Celsius
4. Molar heat capacity is defined as the amount of heat required to raise the temperature of 1 mole of a substance by: — 1 Kelvin
5. Enthalpy of formation (ΔH_f°) is defined as the enthalpy change when: — 1 mole of a compound is formed from its constituent elements in their standard states.
6. Enthalpy of combustion (ΔH_c°) is the enthalpy change when: — 1 mole of a substance reacts completely with oxygen.
7. Enthalpy of solution (ΔH_sol) is the enthalpy change when: — 1 mole of solute dissolves in a solvent.
8. The enthalpy of atomization of methane (CH4) is 1660 kJ/mol. What is the average bond enthalpy of the C-H bond? — 415 kJ/mol
9. If a system absorbs 50 J of heat and does 20 J of work on the surroundings, what is the change in internal energy? — 30 J
10. Enthalpy of phase transition refers to the enthalpy change during: — A change of state (e.g., melting, boiling).
11. Enthalpy of sublimation (ΔH_sub) is the enthalpy change when: — A solid changes directly into a gas.
12. The standard enthalpy of formation of an element in its most stable form is: — Zero
13. For an ideal gas, the relationship between C_p,m and C_v,m is: — C_p,m - C_v,m = R
14. Which of the following processes typically has a positive enthalpy change (endothermic)? — Sublimation of dry ice (solid CO2)
15. Which of the following statements best describes the First Law of Thermodynamics? — Energy can neither be created nor destroyed, only converted from one form to another.
16. Which of the following is NOT a state function? — Heat
17. The enthalpy change for the reaction A(g) → A(g) + e⁻ is known as: — Enthalpy of ionization
18. If ΔH_f°(CO2) = -393.5 kJ/mol, this means that the formation of 1 mole of CO2 from graphite and oxygen releases 393.5 kJ of energy. This is an example of: — Enthalpy of formation
19. The process of breaking all the bonds in 1 mole of gaseous molecules to form gaseous atoms is described by: — Enthalpy of dissociation
20. Consider the reaction: H2O(l) → H2O(g). The enthalpy change for this reaction is: — Enthalpy of vaporization
21. Which of the following terms represents the energy required to convert 1 mole of a solid into 1 mole of a gas at a constant temperature and pressure? — Enthalpy of sublimation
22. The enthalpy change for the process A(g) → A(l) is called: — Enthalpy of condensation
23. If a reaction can be carried out in a number of steps, the total enthalpy change is the sum of the enthalpy changes for each step. This statement is the basis of: — Hess's Law
24. Enthalpy of atomization (ΔH_atom) is the enthalpy change for: — Formation of 1 mole of gaseous atoms from 1 mole of substance in its standard state.
25. Enthalpy of ionization (ΔH_ion) is the enthalpy change for: — Formation of 1 mole of gaseous ions from 1 mole of gaseous atoms.
26. Which of the following is typically an endothermic process? — Melting of ice
27. What is the relationship between enthalpy (H) and internal energy (U) for a system at constant pressure? — H = U + PV
28. When a dilute solution of a strong acid is neutralized by a dilute solution of a strong base, the heat evolved is mainly due to the reaction: — H⁺(aq) + OH⁻(aq) → H₂O(l)
29. Which of the following is a state function? — Internal Energy
30. Which of the following is a state function and depends on both temperature and pressure? — Enthalpy
31. In the equation ΔU = q + w, what does 'w' represent? — Work done on the system
32. For the dissolution process, ΔH_sol = ΔH_lattice + ΔH_hydration. If ΔH_lattice is large and positive, and ΔH_hydration is large and negative, the dissolution is likely to be: — Dependent on temperature only
33. Which thermodynamic quantity is defined as H = U + PV? — Enthalpy
34. Which of the following statements is INCORRECT regarding internal energy? — It is always equal to enthalpy.
35. The heat capacity of a substance is dependent on its: — All of the above
36. If a process is exothermic, the enthalpy change (ΔH) is: — Negative
37. If a process is endothermic, the enthalpy change (ΔH) is: — Positive
38. Hess's Law of Constant Heat Summation states that: — The enthalpy change of a reaction is independent of the path taken and depends only on the initial and final states.
39. Enthalpy of hydration (ΔH_hyd) is the enthalpy change associated with: — The dissolution of 1 mole of gaseous ions in a large amount of water.
40. The enthalpy of solution of NaCl in water is slightly positive (endothermic), meaning: — The hydration energy is less than the lattice energy.
41. Enthalpy of dissociation is the energy required to break 1 mole of a specific type of bond in a molecule. — True, for gaseous state
42. Hess's Law is a direct consequence of which law of thermodynamics? — First Law
43. At constant volume, the heat exchanged (q_v) is equal to: — ΔU
44. At constant pressure, the heat exchanged (q_p) is equal to: — ΔH
45. For a reaction where Δn_g (change in moles of gas) is positive, the difference between ΔH and ΔU is: — ΔH - ΔU = Δn_g RT
46. For an ideal gas at constant volume, the molar heat capacity (C_v,m) is related to the change in internal energy by: — ΔU = n C_v,m ΔT
47. For an ideal gas at constant pressure, the molar heat capacity (C_p,m) is related to the change in enthalpy by: — ΔH = n C_p,m ΔT
48. According to the First Law of Thermodynamics, the change in internal energy (ΔU) of a system is given by: — ΔU = q + w
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E-Book First law of thermodynamics, internal energy and enthalpy, heat capacity, Hess's law, enthalpies of dissociation combustion formation atomization sublimation phase transition hydration ionization and solution Online Test First law of thermodynamics, internal energy and enthalpy, heat capacity, Hess's law, enthalpies of dissociation combustion formation atomization sublimation phase transition hydration ionization and solution Question Bank First law of thermodynamics, internal energy and enthalpy, heat capacity, Hess's law, enthalpies of dissociation combustion formation atomization sublimation phase transition hydration ionization and solution