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# Single Correct MCQs: Thermodynamics - Notes | Study All Types of Questions for JEE - JEE

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Q.1. A well stoppered thermos flask contains some ice cubes. This is an example of
(a) Closed system
(b) Open system
(c) Isolated system
(d) Non thermodynamics system

It is an isolated system

Q.2. For the reaction C(s) + O2(g) → CO2(g)
(a) △H >△U
(b) △H < △U
(c) △H = △U
(d) None of these

Here △ng RT = 0 , because reactant and product contain same number of gaseous molecules. So that △H = △U + △ng RT ⇒ △H = △U

Q.3. For an ideal gas, CV and CP are related as:
(a) CV – CP = R
(b) CV + CP = R
(c) CP – Cv = RT
(d) CP – Cv = R

For an ideal gas, CV and CP are related as CP – Cv = R

Q.4. The least random state of the water system is:
(a) ice
(b) liquid water
(c) steam
(d) randomness is same

The least random state of the water system is ice.

Q.5. Considering entropy(S) thermodynamic parameters the criteria for the spontaneity of any process is:
(a) △S system + △S surroundings > 0
(b) △S system – △S surroundings < 0
(c) △S system > 0
(d) △S surroundings > 0

The criteria for the spontaneity of any process is △S system + △S surroundings > 0

Q.6. The enthalpy change in a reaction does not depend upon
(a) The state of reactions and products
(b) The nature of the reactants and products
(c) Different intermediate steps in the reaction
(d) Initial and final enthalpy of the reaction

The enthalpy change is a state function so it doesn’t depend on different intermediate steps in the reaction.

Q.7. The correct relationship between free energy change in a reaction and the corresponding equilibrium constant KC is
(a) -△G = RT lnKC
(b) △G0 = RT lnKC
(c) -△G0 = RT lnKC
(d) △G = RT lnKC

The relationship between free energy change in a reaction and the corresponding equilibrium constant KC is △G0 = – RT lnKC or -△G0 = RT lnKC

Q.8. What is the entropy change (in JK-1 mol-1) when 1 mole of ice is converted into water at 0℃? (The enthalpy change for the conversion of ice to liquid water is 6.0 kJ mol-1 at 0℃)
(a) 20.13
(b) 2.013
(c) 2.198
(d) 21.98

The entropy change; ds = dqrev /T ⇒ ds = 6000J mol-1 / 273K
⇒ ds = 21.978JK-1 mol-1

Q.9. If liquids A and B form an ideal solution
(a) The entropy of mixing is zero
(b) The free energy of mixing is zero
(c) The free energy as well as the entropy of mixing are zero
(d) The enthalpy of mixing is zero

If liquids A and B form an ideal solution the enthalpy of mixing is zero

Q.10. When water is added to quick lime the reaction is
(a) Explosive
(b) Endothermic
(c) Exothermic
(d) Photochemical

When water is added to quick lime the reaction is exothermic
CaO + H2O → Ca(OH)2 △H = -ve

Q.11. A solution of 200 ml of 1 M KOH is added to 200 ml of 1 M HCl and the mixture is well shaken. The rise in temperature T1 is noted. The experiment is repeated by using 100 ml of each solution and increase in temperature T2 is again noted. Which of the following is correct?
(a) T1 = T2
(b) T2 is twice as large as T1
(c) T1 is twice as large as T2
(d) T1 is four times as large T2

|ΔH| = msΔT ⇒ T1 = T2

Q.12. ΔH0f of CO2(g), CO(g), N2O(g) and NO2(g) in kJ/mol are respectively –393, –110, 81 and 34. Calculate the ΔH in kJ of the following reaction:
2NO2(g) + 3CO(g) → N2O(g) + 3CO2(g)
(a) 836
(b) 1460
(c) – 836
(d) –1460

ΔH = 81 + 3 (-393) -2 (34) -3 (-110) = 81 - 1179 - 68 + 330 = – 836 kJ.

Q.13. Heat of combustion of CH4, C2H6, C2H4 and C2H2 are – 212.8, –373.0, –337.0 and –310.5 kcal mol-1 respectively at the same temperature. The best fuel among these gases is (Atomic masses: H = 1, C = 12)
(a) CH4
(b) C2H6
(c) C2H4
(d) C2H
2

Heat of combustion per g is called fuel value. The best fuel is that substance which has a maximum heat of combustion per g.

Q.14. Under same conditions how many ml of 1M NaOH and M/2 H2SO4 solutions should be mixed so that the total volume of the solution is 100 ml and rise in temperature is highest
(a) 67, 33
(b) 33, 67
(c) 60, 40
(d) 50, 50

If 50 ml. of 1(M) NaOH and 50 ml. of M/2 H2SO4 is taken, complete neutralization of acid and base occurs, maximum heat will be released.

Q.15. One mole of an ideal gas at 300 K is expanded isothermally from an initial volume of one litre to 10 litres. The ΔE for this process is (E stands for internal energy)
(a) 16.7 cal
(b) 1381.1 cal
(c) 9 lit atm
(d) Zero

If the gas is ideal, its expansion at constant temperature is called isothermal expansion and it will be accompanied by no change in internal energy. Thus, ΔE = 0.

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