Chemical Thermodynamics & Energetic Mcqs for NEET | pdf

Chemical Thermodynamics & Energetics is a very important chapter for NEET Aspirants. NEET exam is important in your life, because your future career depends upon your score in NEET exam Chemical Thermodynamics & Energetics MCQ for NEET test your knowledge, intelligence, memory and quick response. Your speed and accuracy is the essence of this NEET MCQ. For this you have to cultivate a different frame of mind. For this first solve the different Chemical Thermodynamics & Energetics MCQs for NEET given in this page and then try to complete each Chapter of chemistry NEET MCQs given on

With Our Chemical Thermodynamics & Energetics MCQ for NEET Find out where you stand, your strong points and weak points and try to take corrective steps immediately. In this process your subconscious mind will be thinking about the correct answers of Chemical Thermodynamics & Energetics  MCQS for those questions and in the second round, you will be getting most of the answers. Remember before starting to solve our Chemical Thermodynamics and Energetics  MCQs online test all the important notes and the meaning of all definitions should be understood.

Here are the list of MCQs on Chemical Thermodynamics & Energetic for NEET | pdf

1) .......not an example of open systems.
a) Plants
b) Animals
c) Human beings
d) Tea in closed cup
Answer : d) Tea in closed cup

2) isolated system includes.....with surrounding.
a) exchange of energy 
b) exchange of matter
C) both exchange of energy & matter
d) none of these
Answer :d) none of these

3) an example of set of extensive properties.
a) Mass, volume, temperature, heat capacity
b) Heat capacity, volume, pressure, temperature
c) Mass, volume, internal energy, entropy
d) entropy, enthalpy, temperature, pressure
Answer :c) Mass, volume, internal energy, entropy

4) Extensive property is....
a) additive
b) non-additive
d) pressure
Answer : a) additive

5) Statistical thermodynamics is a branch of.......of the system
a) microscopic properties
b) macroscopic properties
c)physical properties
d) chemical properties
Answer : a) microscopic properties

6) Mass is....
a) non-state function
b) intensive property
C) state function
d) not an extensive property
Answer : C) state function

6) if pressure and volume of the system remains constant, this is known as....
a) chemical equilibrium
b) thermal equilibrium
c) mechanical equilibrium
d) all
Answer : c) mechanical equilibrium

7) For isothermal correct.
a) ΔU≠0
b) Δ≠T
c) q=0
d) ΔU=0
Answer :a) ΔU≠0

8) For isobaric process.. is Correct.
a) P =0
b) ΔV=0
c) ΔU=0
Answer : d) ΔP=0

9) For isochoric process.... iS correct.
a) V=0
b) Δ  ≠0
c) ΔV=0
d) all of these
Answer :d) all of these

10) For adiabatic process.
a) Δq ≠0
b) ΔT=0
c) q=0
Answer : c) q=0

11) For adiabatic process..
a) ΔT=0
b) ΔU=0
c) ΔU≠0
d) ≠0
Answer :c) ΔU≠0

12) A reversible process Occurs at ...
a) slow rate
b) very slow rate
c) fast rate
d) very fast rate
Answer :b) very slow rate

13).... not feature of reversible process 
a) Driving and opposing forces are in
b) Process can be reversed at any finite steps
c) Maximum work can be drawn from reversible process
d) process can be reversed at any point
Answer :b) Process can be reversed at any finite steps

14) Thermodynamics does not consider
a) initial and final state
b) time factor
c) bulk of matter
d) energy change
Answer :b) time factor

15) A system which can neither exchange a matter nor energy with the surroundings is called,
a) isolated system 
b) Opern system
c) Closed system
d) Ideal system
Answer :a) isolated system

16) Water at its freezing point,in a closed insulated vessel, represents a an_____
a) open system
b) heterogeneous system
c) closed system 
d) homogeneous System 
Answer :b) heterogeneous system

17) An isolated system is one,
a) Which can transfer neither matter nor energy to and from its surroundings
b) Which can transfer both energy and matter
c) Which can transfer matter only
d) Which can transter energy only
Answer : a) Which can transfer neither matter nor energy to and from its surroundings

18) Thermodynamics is based on study of...... of the system
a) microscopic properties
b) macroscopic properties
c) physical properties
d) chemical properties
Answer :b) macroscopic properties

19) Boiling tea in a tea pot which is not closed is a/ an,
a) closed system
b) Open system
c) isolated system
d) homogeneous system
Answer : b) Open system

20) An example of closed system is,
a) hot water present in an open beaker
b) some amount of water present in equilibrium with its vapour in a closed and insulated beaker
c) some amount of hot water enclosed in a Closed container
d) ice kept in open beaker
Answer :c) some amount of hot water enclosed in a Closed container

21) A System is used to be in thermodynamics equilibrium when....
a) the temperature of the system is non uniform and different  from the temperature of the surrounding 
b) the mechanical properties is non uniform throughout the system
c) the state function of the system do not change with time
d) only pressure of the reaction is at equilibrium 
Answer :c) the state function of the system do not change with time

22)  Which of the following is intensive property?
a) Temperature
b) Density
c) molarity
d) all
Answer :d) all

23)  When compositions of the system does not change with time, then the system is in........ equilibrium.
a) thermal 
b) chemical
c) mechanical
d) physical
Answer :b) chemical

24) Which of the following is extensive property? 
a) Mass
b) Mole
c) Volume
d All are correct
Answer :d All are correct

25) Temperature and heat are,
a) Extensive properties 
b) Intensive properties
c) Intensive and extensive properties respectively
d) Extensive and intensive propertes respectively 
Answer :c) Intensive and extensive properties respectively

26) A system which can exchange energy with the Surroundings but no matter is called
a) a heterogenous system
b) an open system
c) closed system
d) an isolated system
Answer :c) closed system

27) Mark the false statement regard lay 
thermodynamic processes-
a) a reversible change is a change in which the pressure remains constant
b) an adiabatic change is a change in which the System is completely isolated in the thermal sense.
c) in an isochoric process, the volume of the System remains constant
d) all the nautral processes are irreversible
Answer : a) a reversible change is a change in which the pressure remains constant

28) Melting of ice at room temperature is....... process.
a) spontaneous
b) non spontaneous 
c) exotheric
d) both (a) and (b)
Answer : a) spontaneous

29) Which of the following is spontaneous endothermic process?
a) conversion of N2,O4, to NO2,
b) low of heat from cold object to hot object
c) separation of Ar and Kr
d) heat transfer from ice to room temperature at 25 C
Answer : a) conversion of N2,O4, to NO2

30) Entropy is....
a) state function
b) non- state function
c) relates orderly arrangement
d) relates freezing of liquid water
Answer : a) state function

31) The unit of entropy is.....
a) JK-1
b) cal K
c) Jk
d) cal-1 K
Answer : a) JK-1

32) Which of the following is correct
a) qp+qv =ΔnRT
b) qreve= TΔS
c) Δn= nR(g) - nP(g)
d) ΔG= + WRT
Answer : b) qreve= TΔS

33) ΔS> 0 for.....
a) freezing of a liquid
b) sublimation of solid
c) liqification of a gas
d) condensation of a gas
Answer : b) sublimation of solid

34) Which of the following is correct ?
a) Sether(l) = SCH3OH (l)
b) Sether(l)  > SCH3OH(l)
c) SCH3OH(l) > Sether(l)  
d) none of the above 
Answer : b) Sether(l) > SCH3OH(l)

35) N2O4(g) has higher entropy than NO
a) due to more complexity of N2,04,
b) more contribution of vibrational motion of N2,04
c) both (a) and (b)
d) more complexity of NO
Answer : c) both (a) and (b)

36) For which of the following , ΔS is positive 
a) 3O2(g) ---> 2O3(g)
b) I2(s)+aq-----> I2(aq)
c) H2O(g)-----> H2O(l)
d) 2H2(g) + O2(g)----> 2H2O(l)
Answer : b) I2(s)+aq-----> I2(aq)

37) Heat of reactions are generally represented at ..
a) 273 K and 1atm
b) 298 K and 2 atm
c) 1atm and 298 K
d) 300 K and 1 atm
Answer : c)1 atm and 298 K

38) For writing thermodynamics equation which of the following is not correct.
a) Reaction is represented by balanced chemical equation
b) Enthalpy changes are measured at 300 K and atm pressure
c) Enthalpy of elements in their standard physical states is zero
d) The enthalpy of any compound is equal to its heat of formation
Answer :a) Reaction is represented by balanced chemical equation

39) ΔcH° of any element or compound is.....
a) always positive
b) always zero
c)always negative
d) both (a) and (b)
Answer : c)always negative

40) Enthalpy of hydration is always ..
a) Exothermic
b) Endothermic Zero
c) always negative 
d) Both (a) and (c)
Answer : a) Exothermic

41) Which of the following is endothermic...
a) Δc
b) ΔL
c) Δatm
d)  Δf
Answer : c) Δatm

42) Which of the following is correct for enthalpy of formation of compounds ?
a) always exothermic
b) always endothermic
c) may be exothermic or endothermic
d) unpredictable
Answer : c) may be exothermic or endothermic

42) The correct order of increasing energy content is
a) lit-atm <calorie<joule < erg
b) joule<calorie <erg< lit-atmm
c) lit-atm> calorie>  > erg
d) erg >calorie >lit-atm >joule
Answer : c) lit-atm> calorie> joule > erg

43) The general gas constant (R) is equal to.....
a) 4.184 J
b) 1.987j
c) 0.0821 lit -atm
d) 8.314 cal
Answer : a) 4.184 J

44) One calorie is equal to,
a) 4.184 x 10 J
b)  107J
c) 4.184 J
d) 24.2J
Answer : c) 4.184 J

45) In an isothermal expansion of an ideal gas,
a) ΔP=0
b) ΔV=0
c) ΔU=0
d) none of the above 
Answer : c) ΔU= 0

46) The work done during expansion in vacuum is zero because,
a) P=0
b) ΔV=0
c) ΔU=0
d) none of above
Answer : a) P=0

47) A gas expands isothermally and reversibly. The work done by the gas is,
a) Zero
b) Minimum
c) Maximum
d)Equal to internal energy change
Answer : c) Maximum

48) Mass and energy are conserved. It is demonstrated by...
a) first law of thermodynamics
b) law of conservation of energy
c) modified form of first law of thermodynamics
d) law of conservation of mass
Answer : c) modified form of first law of thermodynamics

49) It is a general principal that the less energy a system contains, it is....
a) more unstable
b) unstable
C) less stable
d) more stable
Answer :d) more stable

51) The process in which work is done at the expense of internal energy is....
a) isobaric
b) adiabatic
c) isochoric
d) isothermal
Answer :b) adiabatic

52) Following gases have equal masses at the same temperature, pressure and volume. The maximum work is done by....
a) nitrogen
b) hydrogen sulphide
c) ammonia
d) chlorine
Answer :c) ammonia

53) Theoretical basis of Hess's law is....
a) law of conservation of energy
b) heat of ionization of strong acids and strong bases
C) variation in heat of reaction
d) Kirchoff's law
Answer : a) law of conservation of energy

54) The energy required per mole to separate molecules from each other is called....
a) potential energy
b) binding energy
C) internal energy
d) intramole energy
Answer : 
C) internal energy

55) Entropy change of the system and the surrounding in equilibrium..
a) decrease
b) increase
C) is constant
d) either increase or decrease
Answer : C) is constant

56) In general, an exothermic reaction will become a spontaneous one, if
a) temperature is zero
b) temperature is low
c) temperature is high
d) temperature is constant
Answer : b) temperature is low

57) when H2SO4 is added to water the solution becomes hot, the reaction is...
a) an exothermic
b) an irreversible
C) a reversible
d) an endothermic
Answer : a) an exothermic

58) which law of thermodynamics help in calculating Entropy at different temperature...
a) 1st law
b) 2nd law
C) 3rd law
d) none of the above
Answer : C) 3rd law

59) The standard heat of formation at 101.3 kNm-2 and 298 K is arbitarily taken to be zero for....
a) solid bromine
b) liquid bromine
C) gaseous bromine molecules
d) gaseous bromine atoms
Answer : b) liquid bromine

60) Assuming enthalpy of combustion of hydrogen at 273 K is -286 kJ and Enthalpy of fusion of ice at the same temperature to be + 6.0 kJ, calculate Enthalpy change during formation of 100 g of ice
a) +292 kJ
b) +1622 kJ
C) -292 kJ
d) -1622 kJ
Answer : d) -1622 kJ