IIT JEE MCQ Quiz Hub

1. A negative sign of the free energy change denotes that
the system is in constant equilibrium
the reaction is very much unlikely
the reaction is non-spontaneous
the reaction tends to proceed spontaneously

2. For a reversible process the total entropy change
increases
is constant
decreases
is zero

3. The heat of neutralization of a strong acid by a strong base
is greater than 13.7 Kcal
is less than 13.7 Kcal
is nearly 13.7 Kcal
depends upon the nature of the acid

4. Entropy of the universe is always
increasing
decreasing
constant
five

5. The factor that does not influence the heat of reaction is
method by which reactants change to products
chemical state of the reactants and products
whether it is taking place at constant temperature
All the above

6. The highest temperature at which vapour pressure of a liquid can be measured is
the boiling point of the liquid
critical solution temperature
ionisation temperature
inversion temperature

7. On dissolving sodium chloride in water there is
increase in entropy
increase in the free energy
decrease in entropy
No change in enthalpy

8. n a spontaneous irreversible process the total entropy of the system & its surroundings
is constant
decreases
increases
is zero

9. Heat of reaction
depends on the rate of reaction
depends on pressure
is independent of temperature
may or may not depend on temperature

10. On dissolving magnesium sulphate in water
no change in entropy
entropy decreases
entropy increases
nothing can be said

11. Which out of the following represents a closed system?
Hot water contained in a closed container
Hot water contained in open container
Water in a closed insulated container in equilibrium with its vapours
None of the above

12. A person requires 2870 Kcal of energy for leading a normal life. If heat of combustion of cane sugar is -1349 Kcal then he must consume??kg of cane sugar daily.
728
448
142
224

13. 1 Joule is equal to
2.39 Cal
0.04184 Cal
1.390 Cal
0.239 Cal

14. According to Hess Law the thermal effects of a reaction depend upon
initial and final conditions of reactants and products
final conditions of products
intermediate stage of reaction
None of these

15. The process in which no heat change takes place is
an irreversible process
an isothermal process
a reversible process
an adiabatic process

16. If temperature is kept constant during the reaction the process is said to be?.
Adiabatic
Isobaric
Isothermal
None of the above

17. The heat of formation is the change in enthalpy accompanying the formation of a substance from its elements at 298 K and 1 atmospheric pressure. Since the enthalpies of elements are taken to be zero the heat of formation of the compound may be
always positive
always negative
positive or negative
zero

18. Heat of fusion of a molecular solid is
high
low
average
very high

19. Evaporation of water is a spontaneous process although it is
an endothermic in nature
a photochemical reaction
an exothermic in nature
proceeds without heat loss or heat gain

20. On heating a liquid at its boiling point
temperature of the liquid increases
enthalpy increases
activation energy increases
entropy of the system increases

21. Heat of neutralisation of HCl and NaOH is -57.32 kJ per gram equivalent and that of acetic acid and NaOH is -55.23 kJ per gram equivalent. The heat of dissociation of acetic acid per gram equivalent should be
-2.09
2.09
-2.196
2.196

22. n burning hydrogen in an atmosphere of chlorine 1.65 gm of HCl was obtained and 1 Kcal of heat was liberated. The heat of formation of HCl should be:
-21.12 Kcal/mol
-44.2 Kcal/mol
500 cal/mol
500 cal/gm

23. The apparatus used for measuring the heat changes is known as
Thermometer
Ammeter
Voltmeter
Calorimeter

24. The enthalpy of the elements in their standard states is taken as zero. So the enthalpy of formation of a compound may be
negative
positive
zero
negative or positive

25. Which of the following will have maximum entropy?
Argon
Helium
Silver
Diamond

26. Internal energy of the elements is assigned a value of??.cal per mole at standard states.
5
9
99
0

27. Entropy of a substance is Zero at
the temp. at which a substance is in the liquid state
standard states i.e. 25 degreeCentigrade
absolute zero
0 degreeCentigrade

28. 10 gm of ice at 0 degreeCentigrade is placed into 100 gm of water at 50 degreeCentigrade. The temperature of water after the whole ice has melted will be
32.8 degreeCentigrade
19.5 degreeCentigrade
31.8 degreeCentigrade
38.1 degreeCentigrade

29. What is true about entropy?
Entropy of universe increases and tends towards maximum value
Entropy of universe decreases and tends to be zero
Entropy of universe always remain constant
Increases and decreases with a periodic rate.

30. All naturally occurring processes proceed spontaneously in a direction which leads to
increase in enthalpy of system
decrease in entropy of system
decrease in free energy of system
increase in free energy of system.

31. Which of the following processes proceed with increase of entropy?I. solid changing into liquidII. expansion of gasIII. dissolution of solid in liquidIV. polymerization.
Only I
IIIIII
IIIII
IIIIV

32. The heat of solution depends upon
nature of solute
nature of solvent
concentration of solution
All the above

33. The vaporization process is always
exothermic
endothermic
can be exothermic or endothermic
isoentropic.

34. The free energy change occurring during the irreversible process is
negative
positive
dependent on whether the process is exothermic or endothermic
negative only if the process is exothermic.

35. Calorific values of food and fuel are determined by
Bomb calorimeter
Bunsens ice calorimeter
Backmanns thermometer
None of the above

36. Enthalpy of reaction? is the heat change accompanuing the conversion of
1 mole of reactants into products
1 gm of reactants into products
Number of moles of reactants into products as are indicated by the balanced equation of the process
22.4 L of reactants at N.T.P. into products.

37. Internal energy of a given mass of an ideal gas depends upon
Temperature
Pressure
Volume
On all the above factors.

38. The heat of reaction depends upon
ctemperature of the reaction
physical states of reactants and products
both a and b
path of the reaction and temperature.

39. Which statement is not applicable to thermochemical equations?I. They represent chemical change as well as heat changeII. They give the idea about mechanism of the processIII. They depict the spontaneity of the processIV. Exothermic or endothermic nature of reaction.
II IV
III I
III I
II III

40. All the naturally occurring processes proceed spontaineously in a direction which leads to
increase in enthalpy of system
decrease in entropy of system
increase in entropy of system
increase in entropy of universe

41. The heat change in a reaction does not depend upon the
conditions under which reaction is carried
state of reactants and products
number of intermediate stages involved
state of reactants and products

42. In which of the following process entropy increases?I. Rusting of ironII. Vaporisation of CamphorIII. Crystallisation of sugar from syrupIV. Atomisation of dihydrogen.
I II
II III
I IV
Only IV

43. When a solid melts there is
an increase in entropy
an increase in enthalpy
a decrease in internal energy
Both (A) and (B) are correct.

44. Absorption of heat occurs when
carbon burns in air
sulphur dioxide is oxidised to sulphur trioxide
ammonium chloride dissolves s in water
cooking gas is burnt.

45. A system absorbs 20 kJ of heat and also does 10 kJ of work. The net internal energy of the system
increases by 10 kJ
decreases by 10 kJ
increases by 30 kJ
decreases by 30 kJ

46. Thermodynamic parameter which is a state function and is also used to measure disorder of the system is
Entropy
Fugacity
Viscosity
Periodicity

47. In naturally occurring changes a system tends to alter in such a way that the entropy of the system
increases
decreases
remains constant
is reduced to zero

48. In thermodynamics a quantity whose value simply depends upon the initial and final state of the system is called
thermolynamic quantity
state function
adiabatic quantity
path function.

49. Thermochemistry is the study of relationship between heat energy and
activation energy
friction energy
chemical energy
Gibbs energy

50. The enthalpy of formation of the compound is
always + ve
always - ve
can be + ve or - ve
unpredicatable.

51. In the sublimation of iodine
randomness of particles remains unaffected
randomness of particles tends to decrease
energy of the system tends to increase
randomness of particles tends to increase

52. Variation of heat of reaction with temperature is given by relation known as
vant Hoffs isotherm
Vant Hoffs isochore
Kirchhoffs equation
Born-Lande equation.