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Test Details :
Test Name JOURNEY TO MBBS Chemistry Test: 6 Thermo-chemistry
Test Id 250919080038
Generate 2025-09-19 14:33:48 (IST)
Q1. The environment in which a system is studied is:
(a) State function
(b) Phase
(c) Surrounding
(d) State
1. A
2. B
3. C
4. D
Q2. Anything which depends upon the initial and final state of a system is:
(a) Environment
(b) Surrounding
(c) State function
(d) Enthalpy
1. A
2. B
3. C
4. D
Q3. Which of the following is a state function?
(a) Pressure
(b) Temperature
(c) Enthalpy
(d) All of the above
1. A
2. B
3. C
4. D
Q4. Most of thermodynamics parameters are:
(a) System
(b) Surrounding
(c) Phase
(d) State function
1. A
2. B
3. C
4. D
Q5. Change in enthalpy (H) of a system can be calculated by:
(a) ΔH = ΔE + PΔV
(b) ΔH = ΔE – PV
(c) ΔH = ΔE + q
(d) ΔH = ΔE – q
1. A
2. B
3. C
4. D
Q6. Two fundamental ways to transfer energy are:
(a) Heat and work
(b) Pressure and volume
(c) Pressure and temperature
(d) Heat and volume
1. A
2. B
3. C
4. D
Q7. Which of the following equation is correct?
(a) qp > qv
(b) ΔE < ΔH
(c) ΔE > ΔH
(d) Both a, b
1. A
2. B
3. C
4. D
Q8. If there is interconversion of solid and liquid states then:
(a) ΔV = 0
(b) ΔH = ΔE
(c) ΔH > ΔE
(d) Both a and b
1. A
2. B
3. C
4. D
Q9. The exchange of heat energy during chemical reaction at constant temperature and
pressure occurs in the form of:
(a) Free energy
(b) Internal energy
(c) Enthalpy
(d) Bond energy
1. A
2. B
3. C
4. D
Q10. At constant P and T which statement is correct for the reaction CO + ½ O₂ → CO₂?
(a) ΔH = ΔE
(b) ΔH < ΔE
(c) ΔH > ΔE
(d) ΔH is independent of physical state
1. A
2. B
3. C
4. D
Q11. ΔH for the formation of H₂ (g) will be:
(a) Zero
(b) +ve
(c) –ve
(d) ∞
1. A
2. B
3. C
4. D
Q12. The heat changes for the reaction H₂O(l) → H₂O(g) is called:
(a) Heat of solution
(b) Heat of fusion
(c) Heat of vaporization
(d) Heat of formation
1. A
2. B
3. C
4. D
Q13. The word "standard" in standard molar enthalpy change implies:
(a) Temperature 298 K
(b) Pressure 1 atm
(c) Temperature 298 K and pressure 1 atm
(d) Temperature and all pressures
1. A
2. B
3. C
4. D
Q14. Hess's law is used in determination of:
(a) Heat of reaction
(b) Heat of transition
(c) Heat of formation
(d) All of these
1. A
2. B
3. C
4. D
Q15. For which of the following substance the standard heat enthalpy is zero?
(a) C(graphite)
(b) C(diamond)
(c) CO₂
(d) O₃
1. A
2. B
3. C
4. D
Q16. The heat change in chemical reaction at constant volume is given by:
(a) ΔH
(b) ΔE
(c) Δt
(d) ΔV
1. A
2. B
3. C
4. D
Q17. The enthalpy change of a reaction does not depend on:
(a) State of reactants and products
(b) Nature of reactants and products
(c) Different intermediate reactions
(d) Initial and final enthalpy change
1. A
2. B
3. C
4. D
Q18. For the reaction C₃H₈ + 5O₂ → 3CO₂ + 4H₂O at constant T, ΔH – ΔE is:
(a) +RT
(b) –3RT
(c) +3RT
(d) –RT
1. A
2. B
3. C
4. D
Q19. When ammonium chloride is dissolved in water, the solution becomes cold, the change
is:
(a) Endothermic
(b) Exothermic
(c) Super cooling
(d) None of these
1. A
2. B
3. C
4. D
Q20. The standard heat of formation of diamond is:
(a) Same as that of graphite
(b) Greater than graphite
(c) Less than graphite
(d) Taken as zero
1. A
2. B
3. C
4. D
Q21. An equation which indicates physical states of the reactants and products in addition to
numerical value of heat of reaction is called:
(a) Chemical equation
(b) Thermochemical equation
(c) Ionic equation
(d) Skeletal equation
1. A
2. B
3. C
4. D
Q22. In which change ΔH is negative?
(a) Na(s) → Na(g)
(b) ½ Cl₂ → Cl(g)
(c) Na(g) → Na⁺(g) + e⁻
(d) Cl(g) + e⁻ → Cl⁻(g)
1. A
2. B
3. C
4. D
Q23. Which of the following is not standard condition for thermochemical measurement?
(a) A pressure of 1 atm
(b) A temperature of zero K
(c) Substances in their normal physical states
(d) Concentration of 1.0 M
1. A
2. B
3. C
4. D
Q24. Heat given to a system under isochoric process is equal to:
(a) W
(b) q
(c) ΔE
(d) ΔH
1. A
2. B
3. C
4. D
Q25. An example of extensive property is:
(a) Temperature
(b) Internal energy
(c) Viscosity
(d) Surface tension
1. A
2. B
3. C
4. D
Q26. All of the following enthalpy changes have positive or negative value except:
(a) ΔHf°
(b) ΔHsoln°
(c) ΔHlattice E°
(d) ΔHn°
1. A
2. B
3. C
4. D
Q27. Which of the following is exothermic reaction?
(a) Combustion of ethane
(b) Electrolysis of molten NaCl
(c) Decomposition of H₂O
(d) Conversion of graphite to diamond
1. A
2. B
3. C
4. D
Q28. Which of the following has same units?
(a) Work
(b) Heat
(c) Energy
(d) All of these
1. A
2. B
3. C
4. D
Q29. Temperature and heat are:
(a) Extensive properties
(b) Intensive properties
(c) Extensive and intensive properties
(d) Intensive and extensive properties
1. A
2. B
3. C
4. D
Q30. Heat content of the system is called:
(a) E
(b) H
(c) G
(d) S
1. A
2. B
3. C
4. D
Q31. The value of ΔH for the process K(s) → K⁺(g) + e⁻ is equal to:
(a) ΔH₁st LE° of K
(b) ΔHv° of K
(c) ΔH₁st IE° + ΔH₁st E.A of K
(d) ΔHat° + ΔH₁st IE° of K
1. A
2. B
3. C
4. D
Q32. Heat of formation of MgO is given as:
Mg + ½ O₂ → MgO, ΔH = –692.0 kJ mol⁻¹. This means:
(a) The product is very stable
(b) The reaction is endothermic
(c) The product is highly unstable
(d) The reactants are very stable
1. A
2. B
3. C
4. D
Q33. The equation that represents enthalpy of atomization of hydrogen is:
(a) ½ H₂O → H₂ + ½ O₂ + 218 kJ mol⁻¹
(b) ½ H₂O → H₂ + ½ O₂ – 218 kJ mol⁻¹
(c) ½ H₂ → H + 218 kJ mol⁻¹
(d) ½ H₂ → H – 218 kJ mol⁻¹
1. A
2. B
3. C
4. D
Q34. ½ H₂ → H, ΔH = 218 kJ mol⁻¹. In this reaction ΔH will be called:
(a) Enthalpy of atomization
(b) Enthalpy of formation
(c) Enthalpy of decomposition
(d) Enthalpy of dissociation
1. A
2. B
3. C
4. D
Q35. Mg + ½ O₂ → MgO + –692 kJ mol⁻¹ at STP. Enthalpy of above reaction will be:
(a) ΔHn°
(b) ΔHsoln°
(c) ΔHat°
(d) ΔHf°
1. A
2. B
3. C
4. D
Q36. For the reaction CH₃COOH + NaOH → CH₃COONa + H₂O, the change in enthalpy is
called:
(a) Enthalpy of solution
(b) Enthalpy of hydration
(c) Enthalpy of neutralization
(d) Enthalpy of formation
1. A
2. B
3. C
4. D
Q37. Which of the following shows twice the enthalpy change of neutralization as HCl +
NaOH → NaCl + H₂O?
(a) H₂SO₄ + Mg(OH)₂ → MgSO₄ + 2H₂O
(b) MgCO₃ + 2HCl → MgCl₂ + CO₂ + H₂O
(c) NH₄Cl + NaOH → NaCl + H₂O + NH₃
(d) KOH + HCl → KCl + H₂O
1. A
2. B
3. C
4. D
Q38. Lattice energy of an ionic crystal is the enthalpy of:
(a) Combustion
(b) Dissolution
(c) Dissociation
(d) Formation
1. A
2. B
3. C
4. D
Q39. A spontaneous process is:
(a) Unidirectional and irreversible
(b) Unidirectional and real
(c) Irreversible and real
(d) All of the above
1. A
2. B
3. C
4. D
Q40. TvAll will be given positive sign in:
(a) Dissociation reaction
(b) Decomposition reaction
(c) Endothermic reactions
(d) All
1. A
2. B
3. C
4. D
Q41. Which of the following enthalpy change is always exothermic?
(a) Enthalpy of solution
(b) Enthalpy of formation
(c) Enthalpy of combustion
(d) Enthalpy of atomization
1. A
2. B
3. C
4. D
Q42. When one mole of H⁺ from acid and one mole of OH⁻ from base react together to form
water, the enthalpy is called:
(a) Atomization
(b) Neutralization
(c) Formation
(d) Solution
1. A
2. B
3. C
4. D
Q43. The enthalpy change remains the same whether reaction takes place in one or more
steps. This is in accordance with:
(a) Law of mass action
(b) Hess's law
(c) Joule's law
(d) First law of thermodynamics
1. A
2. B
3. C
4. D
Q44. Which of the following is an extensive property?
(a) Density
(b) Temperature
(c) Pressure
(d) Enthalpy
1. A
2. B
3. C
4. D
Q45. Enthalpy of formation of compound is:
(a) Always > 0
(b) Always < 0
(c) Can be > 0
(d) = 0 at standard state
1. A
2. B
3. C
4. D
Q46. Born Haber cycle is an application of:
(a) Raoult's law
(b) Hess's law
(c) Law of mass action
(d) None
1. A
2. B
3. C
4. D
Q47. In Hess's law, sum of enthalpy change of a closed cycle is equal to:
(a) Zero
(b) Greater than zero
(c) Less than zero
(d) None
1. A
2. B
3. C
4. D
Q48. Born Haber cycle is used to find out the enthalpy of:
(a) Atomization
(b) Neutralization
(c) Solution
(d) Lattice energy
1. A
2. B
3. C
4. D
Q49. If value of ΔH in a reaction is positive then the reaction is called:
(a) Exothermic
(b) Endothermic
(c) Polymorphic
(d) None
1. A
2. B
3. C
4. D
Q50. The spontaneity of a process is decided by:
(a) Enthalpy change (ΔH) only
(b) Entropy change (ΔS) only
(c) Gibbs free energy change (ΔG)
(d) Internal energy change (ΔE)
1. A
2. B
3. C
4. D
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