Chemistry chapter 8 Entry Test MCQs
26. A sample of matter under examination in laboratory of unit consideration in the classroom is:
a. Substance
b. Surrounding
c. State function
d. System
28. Sublimation, vaporization, melting and photosynthesis all are examples of
a. Biochemical process
b. Chemical processes
c. Endothermic processes
d. Physical processes
29. Ice can be melted at a room temperature. The process is an example of a
a. Non-spontaneous physical change
b. Chemical change
c. Non-spontaneous chemical change
d. Spontaneous physical change
30. Which of the following is not a spontaneous process?
a. Combustion of natural gas
b. Reaction of H2 with O2 to form H2O
c. Synthesis of glucose by plants
d. Neutralization of HCl with NaOH
31. Thermochemistry is the study of chemical reaction accompanying
a. Mass change
b. Heat change
c. Volume change
d. Rate change
32. Melting of ice at room temperature, rusting of iron and combustion of methane are
a. Spontaneous and endothermic processes
b. Spontaneous and exothermic processes
c. Spontaneous processes
d. Spontaneous and reversible processes
33. N2 and O2 are present in air but they do not react chemically at ordinary conditions of temperature and pressure because it is a
a. Reversible reaction
b. Spontaneous reaction
c. Exothermic reaction
d. Non-spontaneous reaction
34. Burning of coal in air is initiated by a spark and it is an example of a spontaneous reaction because
a. Coal and air react giving reversible reaction
b. Burning of coal in air releases large amount of energy
c. Burning of coal is an endothermic process
d. None of the above
35. For an endothermic reaction, where ΔH represents the enthalpy of the reaction in kJ/mole. The minimum value for the energy of activation will be
a. more than ΔH
b. less than ΔH
c. equal to ΔH
d. zero
First law of Thermodynamics
36. Energy equivalent to one erg, one joule and one calorie is in the order
a. 1 erg > 1 calorie > 1 Joule
b. 1 erg > 1 joule > 1 calorie
c. 1 joule > 1 calorie > 1 erg
d. 1 calorie > 1 joule > 1 erg
37. A mixture of two moles of carbon monoxide and one mole of oxygen, in a closed vessel is ignited to convert the carbon monoxide to carbon dioxide. If ΔH is the enthalpy change and ΔE is the change in internal energy, then
a. ΔH < ΔE
b. ΔH > ΔE
c. The relationship depends on the capacity of the vessel
d. ΔH = ΔE
38. The relation between ΔE and ΔH is:
a. ΔE = ΔV + ΔH
b. ΔH = ΔE – ΔV
c. ΔE =ΔH + PΔV
d. ΔH = ΔE + PΔV
39. The law of conservation of energy states that:
a. The heat content of a system is constant
b. The internal energy of a system is constant
c. There is an equivalence between energy and mass
d. Energy is neither created nor destroyed
40. An ideal gas at constant temperature and pressure expands, then its:
a. Internal energy decreases
b. Internal energy remains same
c. Entropy first increases and then decreases
d. Internal energy increases
41. For the reaction, C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(l) at constant temperature ΔH – ΔE is:
a. –3RT
b. – RT
c. +3RT
d. +RT
42. The work done by a system is 8 joule, when 40 joule heat is supplied to it. What is the increase in internal energy of system
a. 32 J
b. 25 J
c. 28 J
d. 30 J
43. A system absorb 600J of heat and work equivalent to 300J on its surroundings. The change in internal energy is
a. 500 J
b. 300 J
c. 600J
d. 400 J
44. Unit of heat in the SI system is
a. Cal
b. J
c. GJ
d. Kcal
45. The total energy of a system is
a. K.E + heat energy
b. P.E + K.E
c. P.E + mechanical
d. P.E + heat energy
46. Mathematical form of first law of thermodynamics is
a. ΔE = q x v
b. ΔH=qp
c. ΔE = q + W
d. All of the above
47. The total of all the possible kind of energies in a system is called
a. Potential Energy
b. Total energy
c. Internal Energy
d. Kinetic Energy
48. If a system loses 250 kJ of heat at the same time that it is doing 500 kJ of work, what is the change in the internal energy of the system
a. +750 kJ
b. +250 kJ
c. -750 kJ
d. -250 kJ
49. Which one of the following triad of molecules has all type of kinetic Energies: -?
a. CH4,Ne, SO2
b. H2, CO2, NH3
c. He, H2, CH4
d. SO2,CO2, CH4
50. Which statement is contrary to the first law of thermodynamics?
a. In an adiabatic process the work done is independent of its path
b. Energy can neither be created nor destroyed
c. Continuous production of energy
d. One form of energy can be converted into other form of energy