XI Chemistry Thermochemistry Online Test Mdcat-2024

Instructions for Chapter Thermochemistry Online Test Mdcat-2024:

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Test Details:

Subject: Chemistry
Class: 1st year or 11
Chapter name: Thermochemistry
Test: MDCAT 2024
Book: Sindh Textbook
Total No. Of MCQS: 50
Time Allowed: 50 Minutes
Price : Free

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Created on July 24, 2024 By

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XI Chemistry Thermochemistry Online Test Mdcat-2024

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NameEmailPhone Number

1 / 50

1. Least entropy found in which of the following state of water

a) Liquid water at 4°C

b) Liquid water at 25°C

c) Steam at 100°C

d) Ice at 0°C

2 / 50

2. Calorie is equal to

a) 0.4184J

b) 41.84J

c) 4.184J

d) 418.4J

3 / 50

3. The smallest unit of heat energy is:

a) Calorie

b) Erg

c) Joule

d) Kilo Joule

4 / 50

4. Which one is possible for a chemical reaction:

a) Spontaneous and endothermic

b) Nonspontaneous and exothermic

c) spontaneous and Exothermic

d) All of these

5 / 50

5. ΔHf° represents the enthalpy change at

a) 0°C and 1 atm pressure

b) 0 k and 1 atm pressure

c) 25 k and 1 atm pressure

d) 25°C and 1 atm pressure

6 / 50

6. Which of the following statements is wrong?

a) An endothermic reaction must absorb energy before it can take place

b) during an exothermic reaction heat is evolved

c) if the hat of formation of a compound is negative, the compound is more stable than its elements

d) After an exothermic reaction there is no change in the temperature of the reaction mixture

7 / 50

7. Which of the following set of enthalpies is always positive?

a) Sublimation, Electron Affinity, Ionization

b) Lattice Energy, Electron Affinity, Ionization

c) Sublimation, Enthalpy of atomization, Ionization Enthalpy

d) Only enthalpy of atomization is always positive

8 / 50

8. in Breaking of chlorine molecule into chlorine gas atoms, the enthalpy related to this process is ____ and it's ____

a) Electron Affinity, Always positive

b) Ionization enthalpy, always positive

c) Enthalpy of atomization, always negative

d) Enthalpy of atomization, always positive

9 / 50

9. The Born-Haber cycle is a thermodynamic cycle used to analyze the formation of which type of compounds?

a) Covalent compounds

b) Ionic compounds

c) Metallic compounds

d) Molecular compounds

10 / 50

10. Which of the following represents the correct sequence of steps in a Born-Haber cycle for forming an ionic compound?

a) Sublimation,Ionization, bond dissociation, electron affinity, lattice energy

b) Bond dissociation, sublimation, ionization, lattice energy, electron affinity

c) Ionization, electron affinity, bond dissociation, sublimation, lattice energy

d) Electron affinity, ionization, sublimation, bond dissociation, lattice energy

11 / 50

11. Given the following data, calculate the lattice energy of NaCl using the Born-Haber cycle:

Enthalpy of sublimation of Na: +108 kJ/mol,Ionization energy of Na: +496 kJ/mol,Bond dissociation energy of Cl2: +242 kJ/mol,Electron affinity of Cl: -349 kJ/mol,Standard enthalpy of formation of NaCl: -411 kJ/mol

a) -787 kJ/mol

b) -786 kJ/mol

c) -788 kJ/mol

d) -785 kJ/mol

12 / 50

12. Which of the following best describes the electron affinity in the Born-Haber cycle?

a) The energy required to remove an electron from a gaseous atom

b) The energy change when an electron is added to a gaseous atom

c) The energy required to convert a solid to a gas

d) The energy change when a gas condenses to a liquid

13 / 50

13. Which of the following steps is NOT typically part of the Born-Haber cycle?

a) Sublimation of the metal

b) Dissolution of the ionic compound in water

c) Ionization of the metal

d) Formation of the ionic compound from its gaseous ions

14 / 50

14. The Born-Haber cycle is primarily used to calculate which of the following?

a) Standard enthalpy of formation

b) Lattice energy of ionic compounds

c) Ionization energy of metals

d) Electron affinity of nonmetals

15 / 50

15. Which of the following is the correct formula for calculating the standard enthalpy of reaction (ΔH°rxn) using standard enthalpies of formation (ΔH°f)?

a) ΔH°rxn = ΣΔH°f(products) - ΣΔH°f(reactants)

b) ΔH°rxn = ΣΔH°f(reactants) - ΣΔH°f(products)

c) ΔH°rxn = ΣΔH°f(products) + ΣΔH°f(reactants)

d) ΔH°rxn = ΣΔH°f(reactants) / ΣΔH°f(products)

16 / 50

16. Standard enthalpy of formation is taken zero for Diamond or Graphite?

a) Graphite

b) Diamond

c) Both have zero

d) None

17 / 50

17. Which of the following substances has a standard enthalpy of formation of zero at 25°C and 1 atm?

a) Ozone

b) CO_2(g)

c) O_2(g)

d) CH_4(g)

18 / 50

18. Select the correct statement

a) Standard enthalpy of formation of all elements is taken as zero

b) Standard enthalpy of formation is considered zero only for those elements which exist in allotropic form

c) Standard enthalpy of formation is taken zero for least stable allotropic form of an element.

d) All are incorrect

19 / 50

19. In a certain process, the enthalpy change for converting substance X to substance Y is -200 kJ. The reverse process (Y to X) would have an enthalpy change of:

a) -200 kJ

b) 200 kJ

c) 0 kJ

d) Depends on the conditions

20 / 50

20. If the enthalpy change for reaction A---> B is +50 kJ, and the enthalpy change for the reaction B---> C is -30 kJ, what is the enthalpy change for the reaction A---> C?

a) +20 kJ

b) -20 kJ

c) +80 kJ

d) -80 kJ

21 / 50

21. Which of the following statements is true about Hess's Law?

a) It only applies to reactions occurring at constant pressure

b) It only applies to reactions occurring at constant volume

c) It applies to any state of the system as long as the initial and final states are the same.

d) It only applies to reactions in gaseous states.

22 / 50

22. According to Hess's Law, if a reaction can be expressed as the sum of two or more steps, the enthalpy change of the reaction is:

a) The product of the enthalpy changes of the steps

b) The sum of the enthalpy changes of the steps

c) The difference between the enthalpy changes of the steps

d) None of the above

23 / 50

23. Hess's Law is a consequence of which fundamental principle?

a) The first law of thermodynamics

b) The second law of thermodynamics

c) The law of conservation of mass

d) The ideal gas law

24 / 50

24. Which of the following best describes Hess's Law?

a) The enthalpy change of a reaction depends on the pathway taken.

b) The enthalpy change of a reaction is independent of the pathway taken.

c) The enthalpy change of a reaction is always negative.

d) The enthalpy change of a reaction is always positive.

25 / 50

25. Which of the following is correct relation at constant volume

a) qp =ΔH

b) ΔH=ΔE

c) ΔH =ΔE + PΔV

d) None

26 / 50

26. Which of the following is not true for internal energy?

a) It is the total energy content of a thermodynamic system

b) It is a state function

c) It does not depend upon path.

d) None, as all are correct

27 / 50

27. A gaseous chemical reaction is carried out in a cylinder under a constant external pressure of 1 atm. If during the reaction volume increases from 3dm³ to 5dm³ by moving the piston upward. Calculate the workdone and express in Kj?

a) 0.20265Kj

b) -0.20265Kj

c) -0.20265j

d) -202.65Kj

28 / 50

28. If a gas absorbs 100 J of heat and does 40 J of work, what is the change in internal energy ΔE

a) 60 J

b) 140 J

c) -60 J

d) .-140 J

29 / 50

29. In the equation ΔE = q + w, what does w represent?

a) Heat added to the system

b) Work done by the system

c) Internal energy of the system

d) Work done on the system

30 / 50

30. Which equation represents the first law of thermodynamics?

a) ΔE= q + w

b) ΔS= q/T

c) PV = nRT

d) q = mCΔT

31 / 50

31. The first law of thermodynamics is also known as:

a) The law of conservation of momentum

b) The law of conservation of energy

c) The law of constant composition

d) The law of conservation of mass

32 / 50

32. If the enthalpy change for a process is +150 kJ, what can be inferred about the process?

a) The process is exothermic and releases 150 kJ of heat

b) The process is endothermic and absorbs 150 kJ of heat.

c) The process is exothermic and absorbs 150 kJ of heat.

d) The process is endothermic and releases 150 kJ of heat.

33 / 50

33. Which equation correctly represents the relationship between the change in enthalpy and heat exchanged at constant pressure

a) ΔH=qv

b) ΔH=-qv

c) ΔH=qp

d) ΔH=E + W

34 / 50

34. The change in enthalpy ΔH for a reaction is negative. What does this indicate about the reaction?

a) The reaction is endothermic

b) The reaction absorbs heat from the surroundings

c) The reaction releases heat to the surroundings

d) The reaction does no work

35 / 50

35. Unit of work in thermochemistry is taken as

a) atm/dm³

b) dm³/atm

c) atm.dm³

d) N.m

36 / 50

36. In thermochemistry Work is taken positive for

a) Thermochemical expansion

b) Thermochemical Compression

c) When heat is released

d) None

37 / 50

37. In thermochemistry work done by a system is considered as

a) Positive

b) Negative

c) Neutral

d) None

38 / 50

38.

A + B - 60Kj ------> AB

What does the above equation represent?

a) Endothermic reaction

b) Exothermic reaction

c) Non spontaneous reaction

d) Both A and C

39 / 50

39. Select the correct statement

a) Endothermic reactions are spontaneous

b) In exothermic reactions energy of product is greater than reactant

c) In exothermic reactions enthalpy of backward reaction is greater than enthalpy of forward reaction

d) Photosynthesis is an exothermic reaction

40 / 50

40. Which change take place during exothermic reaction:

a) Surroundings get warmer

b) Surroundings get colder

c) Heat is absorbed

d) Both B and C

41 / 50

41. Gas wielding is an:

a) Endothermic reaction

b) Exothermic reaction

c) Both of them

d) None

42 / 50

42. The sum of internal energy and thermodynamic work is called as

a) Heat

b) Enthalpy

c) Temperature

d) Entrooy

43 / 50

43. Which of the following is not a state function?

a) Enthalpy

b) Temperature

c) Heat

d) Volume

44 / 50

44. Select the odd one out:

a) Pressure

b) Volume

c) Mass

d) Moles

45 / 50

45. Which of the following is not an intensive property

a) Surface Tension

b) Pressure

c) Melting Point

d) Enthalpy

46 / 50

46. Properties which are not dependent on quantity of matter in the given system:

a) Intensive properties

b) Extensive properties

c) Cognitive Properties

d) None

47 / 50

47. Example of a system which allows transfer of both: mass and energy is

a) A boiling tea kettle

b) Pressure Cooker

c) Thermoflask

d) All of these

48 / 50

48. A thermodynamic system which allows transfer of energy but not mass:

a) Open system

b) Closed system

c) Isolated System

d) All of these

49 / 50

49. A branch of science which deals with the study of inter transformation of heat, work and other forms of energies:

a) Electrochemistry

b) Thermochemistry

c) Stochiometry

d) Reaction Kinetics

50 / 50

50. Select the incorrect statement:

a) Temperature describes the random movement of particles of a substance

b) Heat is associated with trabsfer of energy between two bodies with different temperature

c) Thermodynamics is a macroscopic property

d) None

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