JEE Questions for Chemistry Thermodynamics Quiz 1 - MCQExams.com

A Beckmann thermometer is used to measure
  • High temperature
  • Low temperature
  • Normal temperature
  • All temperature
The calorific value of fat is ……….
  • less than carbohydrates and protein
  • less than that of protein but more than carbohydrates
  • less than that of carbohydrates and more than that of protein
  • more than thant of carbohydrates and protein
A piece of ice kept at room temperature melts of its own. This reaction is governed by which law ?
  • Second law of thermodynamics
  • First law of thermodynamics
  • Third law of thermodynamics
  • Zeroth law of thermodynamics
For a chemical reaction, ∆G will always be negative if
  • ∆H and T∆S both are positive
  • ∆H and T∆S both are negative
  • ∆H is negative and T∆S is positive
  • ∆H is positive and T∆S is negative
Which of the following processes is accompanied by an increase in entropy ?
  • Normal rubber band to stretched rubber band
  • Normal egg to hard boiled egg
  • Decomposition of N2O5 to N2O to O2
  • Formation of NH3 for N2H2
Which of the following does not exhibit zero entropy at absolute zero
  • Benzene
  • Glass
  • Pyridine
  • CCl4
The favourable conditions for a spontaneous reaction are
  • T∆S > ∆H, ∆H = +ve, ∆S = +ve
  • T∆S > ∆H, ∆H = +ve, ∆S = –ve
  • T∆S = ∆H, ∆H = –ve, ∆S = –ve
  • T∆S = ∆H, ∆H = +ve, ∆S = +ve

Chemistry-Thermodynamics-8664.png
  • -1371.5 kJ
  • -1369.0 kJ
  • - 1364.0 kJ
  • -1361.5 kJ
The heat of combustion of carbon to CO2 is –393.5 kJ/mol. The heat released upon formation of 35.2 g of CO2 from carbon and oxygen gas is
  • –315 kJ
  • +315kJ
  • –630 kJ
  • –3.15 kJ

Chemistry-Thermodynamics-8616.png
  • 32
  • 38
  • 317
  • 477
A gas undergoes a thermodynamical process but the volume of the gas does not change. What is the nature of this process ?
  • Isothermal
  • Adiabatic
  • Isobaric
  • Isochoric
An adiabatic process occurs in
  • open system
  • closed system
  • isolated system
  • in all the given system
An ideal gas expands in volume from 1 × 10- 3 m3 to 1 × 10-2 m3 at 300 K against a constant pressure of 1 × 105 Nm- 2 . The work done is
  • - 900 J
  • - 900 kJ
  • 270 kJ
  • 900 kJ
Which one of the following is not a state function ?
  • Enthalpy
  • Entropy
  • Work
  • Free energy
Which of the following is correct option for free expansion of an ideal gas under adiabatic condition ?

  • Chemistry-Thermodynamics-8617.png
  • 2)
    Chemistry-Thermodynamics-8618.png

  • Chemistry-Thermodynamics-8619.png

  • Chemistry-Thermodynamics-8620.png
Which of the following is a path function?
  • Internal energy
  • Enthalpy
  • Work
  • Entropy
Which of the following is an intensive property ?
  • Temperature
  • Viscosity
  • Surface tension
  • All of these
Three moles of an ideal gas expanded spontaneously into vacuum. The work done will be :
  • Zero
  • Infinite
  • 3 Joules
  • 9 Joules
Internal energy is sum of
  • kinetic energy and potential energy
  • all types of energy of the system
  • energy of internal system
  • None of the above
Hess's law is based on
  • law of conservation of mass
  • law of conservation of energy
  • first law of thermodynamics
  • None of the above
In an adiabatic process

  • Chemistry-Thermodynamics-8622.png
  • q = +W
  • ∆E = q
  • q = 0
In an isothermal process
  • q = 0 and ∆E = 0
  • q ≠ 0 and ∆E = 0
  • q = 0 and ∆E ≠ 0
  • q ≠ 0 and ∆E ≠ 0
The first law of thermodynamics is expressed as
  • q - W = ∆E
  • ∆E = q - W
  • q = ∆E - W
  • W = q + ∆E
  • None of the above
Hess's law is used to calculate
  • enthalpy of reaction
  • entropy of reaction
  • work done in reaction
  • All of these
The temperature of the system decreases in an
  • adiabatic compression
  • isothermal compression
  • isothermal expansion
  • adiabatic expansion
In order to decompose 9 g water 142.5 kJ heat is required. Hence, the enthalpy of formation of water is
  • -142.5 kJ
  • + 142.5 kJ
  • - 285 kJ
  • + 285 kJ
Calculate the amount of heat evolved when 500 cm3 of 0.1 M HCl is mixed with 200 cm3 of 0.2 M NaOH.
  • 57.3 kJ
  • 2.865 kJ
  • 2.292 kJ
  • 0.573 kJ
The bond energy (in kcal mol-1) of C-C single bond is approximately
  • 1
  • 10
  • 100
  • 1000
The species which by definition has zero standard molar enthalpy of formation at 298 K is
  • Br2 (g)
  • Cl2 (g)
  • H2O (g)
  • CH4 (g)
The enthalpy of formation of NH3 is -46 kJ mol-1. The enthalpy change for the reaction 2NH3 (g) → N2 (g ) + 3H2 (g) is
  • + 184 kJ
  • + 23 kJ
  • + 92 kJ
  • + 46 kJ
How many joules of heat are absorbed when 70.0 g of water is completely vaporised at its boiling point ?
(LV = 2260 kJ / kg)
  • 23352
  • 7000
  • 15813
  • 158200
If one mole of ammonia and one mole of hydrogen chloride are mixed in a closed container to form ammonium chloride gas, then
  • ∆H > ∆U
  • ∆H = ∆U
  • ∆H < ∆U
  • there is no relationship
The bond energy is the energy required to
  • dissociate one mole of the substance
  • dissociate bond in 1 kg of the substance
  • break one mole of similar bonds
  • break bonds in one mole of substance
The relation between ∆H and ∆U is
  • ∆H = ∆U + RT
  • ∆H = ∆U - ∆nRT
  • ∆H = ∆U + ∆nRT
  • ∆U = ∆H + ∆nRT
Heat of combustion of carbon monoxide at constant volume and at 17° C is - 67710 cal. The heat of combustion at constant pressure is
  • - 68000 cal
  • - 67800 cal
  • - 67050 cal
  • + 68500 cal
Identify the reaction for which ∆H ≠ ∆E

  • Chemistry-Thermodynamics-8626.png
  • 2)
    Chemistry-Thermodynamics-8627.png

  • Chemistry-Thermodynamics-8628.png

  • Chemistry-Thermodynamics-8629.png

Chemistry-Thermodynamics-8630.png
  • (I) and (IV)
  • (II), (III) and (IV)
  • (I), (II) and (III)
  • (II) and (III)

Chemistry-Thermodynamics-8631.png
  • 180 kJ
  • 186.4 kJ
  • 166.0 kJ
  • 160 kJ
A process is taking place at constant temperature and pressure. Then,
  • ∆H = ∆E
  • ∆H = T∆S
  • ∆H = 0
  • ∆S = 0
Which is correct for an endothermic reaction ?
  • ∆H is positive
  • ∆H is negative
  • ∆E is negative
  • ∆H = 0
For the gaseous reaction involving the complete combustion of iso-butane
  • ∆H = ∆E
  • ∆H > ∆E
  • ∆H < ∆E
  • None of these
∆E° of combustion of iso-butylene is -X kJ mol -1 . The value of ∆H° is
  • = ∆E°
  • > ∆E°
  • = 0
  • < ∆E°
Heat liberated with 100 mL of 1 N NaOH is neutralised by 300 mL of 1 N HCl
  • 11.56 kJ
  • 5.73 kJ
  • 22.92 kJ
  • 17.19 kJ
The quantity of heat measured for a reaction in a bomb calorimeter is equal to
  • ∆G
  • ∆H
  • p∆V
  • ∆E
The heat of neutralisation of any strong acid and a strong base is nearly equal to
  • - 75.3 kJ
  • + 57.3 kJ
  • - 57.3 kJ
  • + 75.3 kJ
Heat required to raise the temperature of 1 mole of a substance by 1° is called
  • specific heat
  • molar heat capacity
  • water equivalent
  • specific gravity
If ∆G for a reaction is negative, you infer that the change is
  • spontaneous
  • non-spontaneous
  • reversible
  • irrevrsible
  • equilibrium
What will be the value of ∆G for ice at 8°C temperature ?
  • One
  • Negative
  • Positive
  • Zero
One mole of which of the following has the highest entropy?
  • Liquid nitrogen
  • Hydrogen gas
  • Mercury
  • Diamond
Gibb's free energy G, enthalpy H and entropy S are interrelated as in
  • G = H + TS
  • G = H - TS
  • G - TS = H
  • G = S = H
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