Check the below NCERT MCQ Questions for Class 11 Chemistry Chapter 6 Thermodynamics with Answers Pdf free download. MCQ Questions for Class 11 Chemistry with Answers were prepared based on the latest exam pattern. We have provided Thermodynamics Class 11 Chemistry MCQs Questions with Answers to help students understand the concept very well.
Q.1 Which of the following has the highest entropy?
(a) Mercury
(b) Hydrogen
(c) Water
(d) Graphite
(b) Hydrogen
Q.2 Hesss law is an application of
(a) 1st law of Thermodynamics
(b) 2nd law of Thermodynamics
(c) Entropy change
(d) ∆H = ∆U + P∆V
(a) 1st law of Thermodynamics
Q.3 One mole of which of the following has the highest entropy?
(a) Liquid Nitrogen
(b) Hydrogen Gas
(c) Mercury
(d) Diamond
(b) Hydrogen Gas
Q.4 At absolute zero the entropy of a perfect crystal is zero. This statement corresponds to which law of thermodynamics?
(a) Zeroth Law
(b) First Law
(c) Second Law
(d) Third Law
(d) Third Law
Q.5 Third law of thermodynamics provides a method to evaluate which property?
(a) Absolute Energy
(b) Absolute Enthalpy
(c) Absolute Entropy
(d) Absolute Free Energy
(c) Absolute Entropy
Q.6 In a reversible process the system absorbs 600 kJ heat and performs 250 kJ work on the surroundings. What is the increase in the internal energy of the system?
(a) 850 kJ
(b) 600 kJ
(c) 350 kJ
(d) 250 kJ
(c) 350 kJ
Q.7 Which one of the following statement is false?
(a) Work is a state function
(b) Temperature is a state function
(c) Change in the state is completely defined when the initial final states are specified
(d) Work appears at the boundary of the system
(a) Work is a state function
Q.8 A system absorb 10 kJ of heat at constant volume and its temperature rises from 270 C to 370 C. The value of ∆ U is
(a) 100 kJ
(b) 10 kJ
(c) 0 kJ
(d) 1 kJ
(b) 10 kJ
Q.9 In which of the following process, a maximum increase in entropy is observed?
(a) Dissolution of Salt in Water
(b) Condensation of Water
(c) Sublimation of Naphthalene
(d) Melting of Ice
(c) Sublimation of Naphthalene
Q.10 In a chemical reaction the bond energy of reactants is more than the bond energy of the products. Therefore, the reaction is
(a) Exothermic
(b) Athermic
(c) Endothermic
(d) Endergonic
(c) Endothermic
Q.11 Entropy of the universe is
(a) Continuously Increasing
(b) Continuously Decreasing
(c) Zero
(d) Constant
(a) Continuously Increasing
Q.12 In which of the following process, the process is always non-feasible?
(a) ∆H > 0, ∆S > 0
(b) ∆H < 0, ∆S > 0
(c) ∆H > 0, ∆S < 0
(d) ∆H < 0, ∆S < 0
(c) ∆H > 0, ∆S < 0
Q.13 Which thermodynamic function accounts automatically for enthalpy and entropy both?
(a) Helmholtz Free Energy (A)
(b) Internal Energy (E)
(c) Work Function
(d) Gibbs Free Energy
(d) Gibbs Free Energy
Q.14 Internal energy does not include
(a) Nuclear energy
(b) Vibrational energy
(c) Rotational energy
(d) Energy of gravitational pull
(d) Energy of gravitational pull
Q.15 In a reversible process the system absorbs 600 kJ heat and performs 250 kJ work on the surroundings. What is the increase in the internal energy of the system?
(a) 850 kJ
(b) 600 kJ
(c) 350 kJ
(d) 250 kJ
(c) 350 kJ
Q.16 The enthalpies of combustion of carbon and carbon monoxide are -393.5 and -283.0 kJ mol-1 respectively. The enthalpy of formation of carbon monoxide is:
(a) -676 kJ
(b) 110.5 kJ
(c) -110.5 kJ
(d) 676.5 kJ
(c) -110.5 kJ
Q.17 An adiabatic’expansion of an ideal gas always has
(a) Decrease in temperature
(b) q = 0
(c) W = 0
(d) ∆H = 0
(b) q = 0
Q.18 The temperature of the system decreases in an ______________.
(a) Adiabatic Compression
(b) Isothermal Expansion
(c) Isothermal Compression
(d) Adiabatic Expansion
(d) Adiabatic Expansion
Q.19 The heat required to raise the temperature of a body by 1 K is called
(a) Specific heat
(b) Thermal capacity
(c) Water equivalent
(d) Molar heat capacity
(b) Thermal capacity
Q.20 Amount of heat required to change 1 g ice at 0°C to 1 g steam at 100°C is
(a) 616 cal
(b) 12 R cal
(c) 717 cal
(d) None of these
(c) 717 cal
Q.21 In thermodynamics a process is called reversible when
(a) Surroundings and system change into each other
(b) There is no boundary between system and surroundings
(c) The surroundings are always in equilibrium with the system
(d) The system changes into surroundings spontaneously
(c) The surroundings are always in equilibrium with the system
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