MDCAT XI Chemistry Thermochemistry Online Test-2

496

Created on July 17, 2025 By

📚 Test Details

Subject: Chemistry
Class: 1st year / XI
Chapter: Thermochemistry
Test: 2
Book: Sindh Textbook
Total No. Of MCQs: 50 MCQs
Time Allowed: 50 Minutes

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Price: Free

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1 / 50

1. The standard enthalpy change for a reaction is calculated using:

a) Bond dissociation energies only

b) Hess’s law

c) First law

d) Le Chatelier’s principle

2 / 50

2. A process where no heat is exchanged is called:

a) Isothermal

b) Adiabatic

c) Isobaric

d) Isochoric

3 / 50

3. Energy required to remove an electron from an atom is:

a) Lattice energy

b) Ionization energy

c) Bond enthalpy

d) Electronegativity

4 / 50

4. Which of these processes is endothermic?

a) Condensation

b) Freezing

c) Melting

d) Combustion

5 / 50

5. Which is not involved in thermochemistry?

a) Heat

b) Temperature

c) Moles

d) Speed

6 / 50

6. Which one is a thermodynamic process?

a) Fusion

b) Combustion

c) Expansion

d) All

7 / 50

7. ΔHf° of O₂ (g) is:

a) 0

b) 1

c) -1

d) -298

8 / 50

8. Internal energy is:

a) Path function

b) State function

c) Constant always

d) Not measurable

9 / 50

9. When a system does work on the surroundings:

a) w is positive

b) w is zero

c) w is negative

d) q is negative

10 / 50

10. ΔU = q + w represents:

a) Second law

b) First law

c) Third law

d) Zeroth law

11 / 50

11. Standard enthalpy of combustion is:

a) Always positive

b) Always zero

c) Always negative

d) Sometimes positive

12 / 50

12. A spontaneous exothermic reaction has:

a) ΔH > 0

b) ΔH < 0

c) ΔG > 0

d) No energy change

13 / 50

13. ΔH of sublimation is equal to:

a) ΔH of fusion + vaporization

b) ΔH of formation

c) ΔH of vaporization

d) ΔH of fusion

14 / 50

14. Which reaction has ΔH = 0?

a) Physical change

b) Formation of compound

c) Phase transition

d) Element in standard state

15 / 50

15. The specific heat of water is approximately:

a) 1 J/g·K

b) 4.18 J/g·K

c) 2.0 J/g·K

d) 10.0 J/g·K

16 / 50

16. When bond is formed:

a) Energy is released

b) Energy is absorbed

c) No energy change

d) Energy equals zero

17 / 50

17. ΔH of neutralization is always:

a) Negative

b) Positive

c) Zero

d) Undefined

18 / 50

18. If ΔH > 0 and ΔS > 0, the reaction is:

a) Always spontaneous

b) Never spontaneous

c) Spontaneous at high temp

d) Spontaneous at low temp

19 / 50

19. Lattice energy is:

a) Always positive

b) Always negative

c) May be either

d) Zero

20 / 50

20. Which of the following is NOT a thermochemical equation?

a) Includes physical states

b) Includes enthalpy change

c) Balanced chemical equation

d) Includes catalysts

21 / 50

21. ΔH is greater than ΔU when:

a) Gases are produced

b) Gases are consumed

c) No gas involved

d) Pressure is zero

22 / 50

22. In an exothermic reaction:

a) q is positive

b) q is negative

c) ΔH > 0

d) ΔU increases

23 / 50

23. If temperature of water rises, the reaction is:

a) Endothermic

b) Exothermic

c) Neutral

d) Isothermal

24 / 50

24. Which device is used to measure heat flow?

a) Thermometer

b) Manometer

c) Calorimeter

d) Spectrometer

25 / 50

25. If 2 kJ of heat is supplied to 1 mol of gas at constant volume, ΔU is:

a) 2 kJ

b) 0

c) Depends on work

d) Can’t be determined

26 / 50

26. Which of the following conditions always guarantees a spontaneous reaction?

a) ΔH < 0 and ΔS < 0

b) ΔH 0

c) ΔH > 0 and ΔS > 0

d) ΔH > 0 and ΔS < 0

27 / 50

27. A gas expands from 2 L to 6 L at 1 atm. What is the work done by the gas?

a) -404 J

b) +404 J

c) -202 J

d) +202 J

28 / 50

28. The unit of specific heat capacity is:

a) J

b) J/kg

c) J/kg·K

d) J/mol·K

29 / 50

29. A calorimeter is used to measure:

a) Temperature only

b) Mass

c) Heat of reaction

d) Pressure

30 / 50

30. The energy required to break a bond is:

a) Bond enthalpy

b) Heat of formation

c) Activation energy

d) Lattice energy

31 / 50

31. Combustion reactions are typically:

a) Endothermic

b) Isothermal

c) Exothermic

d) Non-spontaneous

32 / 50

32. Which is exothermic?

a) Evaporation

b) Freezing

c) Boiling

d) Melting

33 / 50

33. For a reaction at constant pressure, the heat change is:

a) ΔU

b) ΔH

c) Qv

d) W

34 / 50

34. Heat capacity is defined as:

a) Heat required to raise temp of 1 mol by 1°C

b) Heat required to raise temp of a substance by 1°C

c) Heat released during combustion

d) None

35 / 50

35. Which has the highest enthalpy?

a) Solid

b) Liquid

c) Gas

d) Plasma

36 / 50

36. The heat required to change one mole of solid to liquid at its melting point is:

a) Heat of vaporization

b) Heat of formation

c) Heat of fusion

d) Heat of combustion

37 / 50

37. Standard enthalpy change of formation of an element in its most stable form is:

a) 0

b) 1

c) -1

d) +1

38 / 50

38. Enthalpy change of neutralization of strong acid and strong base is approximately:

a) 13.7 kJ

b) -57kj

c) 100kj

d) 0

39 / 50

39.

Hess’s Law is based on

a) Conservation of energy

b) Law of definite proportions

c) Le Chatelier’s principle

d) Law of multiple proportions

40 / 50

40. Heat transferred at constant volume equals:

a) ΔH

b) ΔG

c) ΔU

d) Qp

41 / 50

41. If a chemical reaction releases 500 kJ of heat, it is:

a) Endothermic

b) Thermoneutral

c) Exothermic

d) Non-spontaneous

42 / 50

42. ΔH = ΔU + PΔV applies under:

a) Constant pressure

b) Constant volume

c) Adiabatic conditions

d) Isothermal conditions

43 / 50

43. Which law is related to the conservation of energy?

a) Hess's law

b) First law of thermodynamics

c) Second law of thermodynamics

d) Boyle’s law

44 / 50

44. Which one is not an extensive property?

a) Enthalpy

b) Internal energy

c) Temperature

d) Heat capacity

45 / 50

45. In an endothermic reaction:

a) Heat is released

b) ΔH is negative

c) Surroundings get hot

d) Heat is absorbed

46 / 50

46. The heat content of a system at constant pressure is known as:

a) Internal energy

b) Work

c) Enthalpy

d) Entropy

47 / 50

47. A reaction is exothermic if:

a) ΔH is positive

b) ΔH is zero

c) ΔH is negative

d) ΔG is positive

48 / 50

48. The SI unit of enthalpy is:

a) cal

b) kcal

c) J

d) kJ/mol

49 / 50

49. Which of the following is a state function?

a) Heat

b) Work

c) Enthalpy

d) Path

50 / 50

50. q = mcΔT is used to calculate:

a) Heat transferred

b) Enthalpy change

c) Entropy

d) Work

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MDCAT XI Chemistry Thermochemistry Online Test-2

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