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Thermodynamics Class 11 MCQs Questions with Answers
Multiple Choice Type Questions
Question 1.
One gram of sample of NH4NO3 is decomposed in a bomb calorimeter. The temperature of the calorimeter increases by 6.12 K. The heat capacity of the system is 1.23 kj/deg. What is the molar heat of decomposition of NH4NO3?
(a) -7.53 kj/mol
(b) -398.1 kj mol-1
(c) -16.1 kj/mol
(d) -602 kj/mol.
Answer
Answer: (d) -602 kj/mol.
Question 2.
AHr of graphite is 0.23 kj/mol and ∆Hf for diamond is 1.896 kj mol-1, ∆Htransition from graphite to diamond is
(a) 1.66 kj/mol
(b) 2.1 kj/mol
(c) 2.33 kj/mol
(d) 1.5 kj/mol
Answer
Answer: (a) 1.66 kj/mol
Question 3.
The bond energies of C-C, C=C; H-H and C-H linkages are 350, 600, 400 and 410 kj per mole respectively. The heat of hydrogenation of ethylene is
(a) -170 kj mol-1
(b) -260 kj mol-1
(c) 400 kj mol-1
(d) -450 kj mol-1
Answer
Answer: (a) -170 kj mol-1
Question 4.
Which of the following reaction defines ∆H\(_{f}^{0}\)?
(a) C(Diamond) + O2(g) → CO2(g)
(b) \(\frac {1}{2}\) H2(g) + \(\frac {1}{2}\) F2(g) → HF(g)
(c) N2(g) + 3H2(g) → 2NH3(g)
(d) CO(g) + \(\frac {1}{2}\) O2(g) → CO2(g)
Answer
Answer: (b) \(\frac {1}{2}\) H2(g) + \(\frac {1}{2}\) F2(g) → HF(g)
Question 5.
One mole of a hon-ideal gas undergoes a change of state (2.0 atm, 3.0 L, 95 K) → (4.0 atm, 5.0 L, 245 K) with a change in internal energy, ∆U = 30.0 L atm. The change in enthalpy (∆H) of the process in L atm is
(a) 44.0
(b) 42.3
(c) 44.0
(d) not defined because pressure is not constant.
Answer
Answer: (c) 44.0
Question 6.
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
Answer
Answer: (a) Work is a state function
Question 7.
Molar heat capacity of water in equilibrium with ice at constant pressure is
(a) zero
(b) infinity
(c) 40.45 kj K-1 mol-1
(d) 75.48 JK-1 mol-1
Answer
Answer: (b) infinity
Question 8.
For the reaction C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(I) at constant temperature ∆H – ∆E is
(a) + RT
(b) – 3RT
(c) + 3RT
(d) -RT
Answer
Answer: (b) – 3RT
Question 9.
For which one of the following equations AHreaction equals ∆H\(_{f}^{0}\) for the product?
(a) N2(g) + O3(g) → N2O3(g)
(b) CH4(g) + 2Cl2(g) → CH2Cl2(l) + 2HCl(g)
(c) Xe(g) + 2F2(g) → XeF4(g)
(d) 2C(g) + O2(g) → 2CO2(g)
Answer
Answer: (c) Xe(g) + 2F2(g) → XeF4(g)
Question 10.
Enthalpy of CH4 + \(\frac {1}{2}\) O2 → CH3OH is negative.
If enthalpy of combustion of CH4 and CH3OH are x and y respectively then which reaction is correct?
(a) x > y
(b) x < y
(c) x = y
(d) x ≥ y
Answer
Answer: (b) x < y
Question 11.
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
Answer
Answer: (b) Thermal capacity
Question 12.
In a reaction involving only solids and liquids, which of the following is true?
(a) ∆H < ∆E (b) ∆H = ∆E (c) ∆H > ∆E
(d) ∆H = ∆E + RT∆11
Answer
Answer: (b) ∆H = ∆E
Question 13.
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
Answer
Answer: (c) ∆H > 0, ∆S < 0
Question 14.
Internal energy does not include
(a) Nuclear energy
(b) Vibrational energy
(c) Rotational energy
(d) Energy of gravitational pull
Answer
Answer: (d) Energy of gravitational pull
Question 15.
Which of the following reactions is endothermic?
(a) N2 + O2 → 2NO
(b) H2 + Cl2 → 2HCl
(c) H2SO4 + 2NaOH → Na2SO4 + 2H11O
(d) None of these
Answer
Answer: (a) N2 + O2 → 2NO
Question 16.
An adiabatic’expansion of an ideal gas always has
(a) Decrease in temperature
(b) q = 0
(c) W = 0
(d) ∆H = 0.
Answer
Answer: (b) q = 0
Question 17.
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
Answer
Answer: (c) 717 cal
Question 18.
In what proportional 1 M NaOH and 0.5 MH2SO4 are mixed respectively so as to release maximum amount of energy and to form 100 ml of solution?
(a) 33 and 67
(b) 67 and 33
(c) 40 and 60
(d) 50 and 50
Answer
Answer: (d) 50 and 50
Question 19.
In order to decompose 9 g water, 142.5 kj heat is required. Hence the enthalpy of formation of water is
(a) -196 kj mol-1
(b) +196 kj mol-1
(c) +948 kj mol-1
(d) -948 kj mol-1
Answer
Answer: (b) +196 kj mol-1
Question 20.
Change in enthalpy for the reaction 2H2O2(l) → 2H2O(l) + O2(g) if the heat of formation of H2O2(l) and H2O(l) are – 188 kj mol-1 and -283 kj mol-1. Therefore the heat of formation of CO in kj mol-1 is
(a) +172.5
(b) -110.5
(c) -1070
(d) -676.5
(e) +110.5
Answer
Answer: (a) +172.5
Question 21.
The heats of combustion of graphite and CO respectively are -393.5 kj mol-1 and -283 kj mol-1. Therefore the heat of formation of CO in kj moj-1 is.
(a) +172.5
(b) -110.5
(c) -1070
(d) -676.5
(e) +110.5
Answer
Answer: (b) -110.5
Question 22.
Compounds with high heat of formation are less stable because
(a) It is difficult to synthesise them
(b) Energy rich state leads to instability
(c) High temperature is required to synthesise them
(d) Molecules of such compounds are distorted
Answer
Answer: (b) Energy rich state leads to instability
Question 23.
C(diamond) → C(graphite) ∆H = -ve. This shows that
(a) Graphite is more stable than diamond
(b) Diamond is more stable than graphite
(c) Both are equally stable
(d) Stability cannot be predicted.
Answer
Answer: (a) Graphite is more stable than diamond
Question 24.
Enthalpy of neutralisation of HCl with NaOH is x. The heat evolved when 500 ml of 2N HCl are mixed with 250 ml of 4N NaOH will be
(a) 500x
(b) 100x
(c) x
(d) 10x
Answer
Answer: (c) x
Question 25.
In a closed insulated container, a liquid is stirred with a paddle to increase the temperature. Which of the following is true?
(a) ∆E = W ≠ 0, q = 0
(b) ∆E = W = q ≠ 0
(c) ∆E = 0, W = q ≠ 0
(d) W = 0, ∆E = q ≠ 0
Answer
Answer: (a) ∆E = W ≠ 0, q = 0
Question 26.
For an endothermic reaction ∆S is positive, the reaction is
(a) feasible when T∆S > ∆H
(b) feasible when ∆H > T∆S
(c) feasible at all temperature
(d) Not feasible at all
Answer
Answer: (a) feasible when T∆S > ∆H
Question 27.
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
Answer
Answer: (c) The surroundings are always in equilibrium with the system
Question 28.
Entropy change involved in the conversion of 1 mol of liquid water at 373 K to vapour at the same temperature will be (∆Hvap = 2.257 kJg-1)
(a) 0.119 kj
(b) 0.109 kj
(c) 0.129 kj
(d) 0.120 kj
Answer
Answer: (b) 0.109 kj
Question 29.
2 mol of an ideal gas at 27°C is expanded reversibly from 2 L to 20 L. Find entropy change (R = 2 cal/mol K) in cal K-1 mol-1
(a) 92.1
(b) 0
(c) 4
(d) 9.2
Answer
Answer: (d) 9.2
Question 30.
Which of the following is not a state function
(a) ∆G
(b) ∆E
(c) W
(d) H
Answer
Answer: (c) W
Question 31.
For the reaction H2(s) ⇌ H2O(l) at 0°C and normal pressure
(a) ∆H < T∆S
(b) ∆H = ∆G
(c) EH = T∆S
(d) ∆H > T∆S
Answer
Answer: (c) EH = T∆S
Question 32.
Which of the following does not result in an increase in entropy?
(a) Crystallisation of surcose from solution
(b) Rusting of iron
(c) Conversion of ice to water
(d) Vaporisation of camphor
Answer
Answer: (a) Crystallisation of surcose from solution
Question 33.
The unit of entropy is
(a) joule
(b) joule per mole
(c) joule per Kelvin
(d) joule per gram.
Answer
Answer: (c) joule per Kelvin
Question 34.
In the reaction normal egg → Hard boiled egg ∆S is
(a) -ve
(b) 0
(c) +ve
(d) +ve and 0.
Answer
Answer: (a) -ve
Question 35.
PbO2 → PbO, ∆G298 < 0
SnO2 → SnO, ∆G298 > 0.
Most probable oxidation state of Pb and Sn will be
(a) Pb+4, Sn+4
(b) Pb+4, Sn-2
(c) Pb+2, Sn+2
(d) Pb+2, Sn+4
Answer
Answer: (d) Pb+2, Sn+4
Question 36.
The bond dissociation energies for Cl2, I2 and ICl are 242.3, 151.0 and 211.3 kj mol-1 respectively. The enthalpy of sublimation of iodine is 62.8 kj mol-1 What is the standard1 enthalpy of formation of ICl(g) nearly equal to
(a) -211.3 kj mol-1
(b) -14.6 kj mol-1
(c) 16.8 kj mol-1
(d) 33.5 kj mol-1
Answer
Answer: (c) 16.8 kj mol-1
Question 37.
The quantity of heat measured for a reaction in a bomb calorimeter is equal to
(a) ∆G
(b) ∆H
(c) P∆V
(d) ∆E
Answer
Answer: (d) ∆E
Question 38.
Consider the following reactions:
(i) H+(aq) + OH–(aq) → H2O(l); ∆H = – X1kJ mol-1
(ii) H2(g) + \(\frac {1}{2}\) O2(g) → H2O(l); ∆H = – X2 kj mol-1
(iii) CO2(g) + H2(g) → CO(g) + HO(l) – X3kJ mol-1
(iv) C2H2(g) + \(\frac {1}{2}\) O2(g) → 2CO2(g) + H2O(l) + X4 kj mol-1
Enthalpy of formation of H2O(l) is
(a) +X1 kj mol-1
(b) -X2 kj mol-1
(c) +X3 kj mol-1
(d) -X4 kj mol-1
Answer
Answer: (b) -X2 kj mol-1
Question 39.
Given that the bond energies of H-H and Cl-Cl are 430 kj mol-1 and 240 kj mol-1 respectively and ∆fH for HCl is – 90 kj mol-1 Bond enthalpy of HCl is
(a) 245 kj mol-1
(b) 290 kj mol-1
(c) 380 kj mol-1
(d) 425 kj mol-1.
Answer
Answer: (d) 425 kj mol-1.
Question 40.
If K < 1.0, what will be the value of ∆G° of the following?
(a) 1.0
(b) zero
(c) Negative
(d) Positive
Answer
Answer: (d) Positive
Fill in the Blanks
Question 1.
In a closed system, there is no exchange of ……………… but exchange of ……………… is possible between the system and the surroundings.
Answer
Answer: matter, energy
Question 2.
When there is no exchange of heat taking place between the system and surroundings, it is said to undergo ……………… process.
Answer
Answer: Adiabatic
Question 3.
The state function is one whose value depends on ……………… state and ……………… state of the system and not on the ……………… followed.
Answer
Answer: initial, final, path
Question 4.
The positive sign of w indicates work done …………….. the system and negative sign of w indicates work done ……………… the system.
Answer
Answer: on, by
Question 5.
I law of thermodynamics states that energy of an isolated system is ………………
Answer
Answer: constant
Question 6.
Mathematically 1 law of thermodynamics is q + w = ………………
Answer
Answer: AU
Question 7.
∆H is ……………… for exothermic reactions and ∆H is ……………… for endothermic reactions.
Answer
Answer: negative, positive
Question 8.
Internal energy is an ……………… property and pressure is ……………… property.
Answer
Answer: extensive intensive
Question 9.
The experimental techniques to measure energy changes associated with chemical and physical processes is called ………………
Answer
Answer: calorimetry
Question 10.
Lattice energy of an ionic compound like Na+Cl– can be calculated using ………………
Answer
Answer: Born-Haber Cycle.
True/False Statements
Question 1.
q is positive when heat is transferred from the surroundings to the system.
Answer
Answer: True
Question 2.
∆H indicates change in energy at constant volume.
Answer
Answer: False
Question 3.
Work is a state function.
Answer
Answer: False
Question 4.
Enthalpy is the total heat content of a system at constant pressure.
Answer
Answer: True
Question 5.
The standard state of a substance at a specified temperature is the pure form at 1 bar.
Answer
Answer: True
Question 6.
If ∆G > 0, the process is spontaneous.
Answer
Answer: False
Question 7.
A spontaneous process is an irreversible process.
Answer
Answer: True
Question 8.
Entropy is the measure of orderliness of a system.
Answer
Answer: False
Question 9.
A process in which ∆H is positive and ∆S is negative is spontaneous.
Answer
Answer: False
Question 10.
Many reactions which are non-spontaneous at low temperature, are made spontaneous at high temperatures having positive entropy.
Answer
Answer: True
Match Type Questions
| Column I | Column II |
| 1. Internal energy | (i) U + PV |
| 2. Enthalpy H | (ii) ∫PdV |
| 3. Work of an expansion contractions | (iii) \(\frac {q_{rev}}{T}\) |
| 4. ∆S | (iv) State function |
Answer
Answer:
| Column I | Column II |
| 1. Internal energy | (iv) State function |
| 2. Enthalpy H | (i) U + PV |
| 3. Work of an expansion contractions | (ii) ∫PdV |
| 4. ∆S | (iii) \(\frac {q_{rev}}{T}\) |
| Column I | Column II |
| 1. ∆G | (i) Rln (\(\frac {V_2}{V_1}\)) |
| 2. ∆ST | (ii) RTln (\(\frac {V_1}{V_2}\)) |
| 3. ∆U | (iii) CvdT |
| 4. wadiabatic | (iv) (∆H)v – V∆P |
Answer
Answer:
| Column I | Column II |
| 1. ∆G | (ii) RTln (\(\frac {V_1}{V_2}\)) |
| 2. ∆ST | (i) Rln (\(\frac {V_2}{V_1}\)) |
| 3. ∆U | (iii) CvdT |
| 4. wadiabatic | (iv) (∆H)v – V∆P |
| Column I | Column II |
| 1. Isothermal process | (i) q = ∆U |
| 2. Adiabatic process | (ii) w = – P∆V |
| 3. Isobaric process | (iii) w = ∆U |
| 4. Isochoric process | (iv) w = nRTln (\(\frac {V_2}{V_1}\)) |
Answer
Answer:
| Column I | Column II |
| 1. Isothermal process | (iv) w = nRTln (\(\frac {V_2}{V_1}\)) |
| 2. Adiabatic process | (iii) w = ∆U |
| 3. Isobaric process | (ii) w = – P∆V |
| 4. Isochoric process | (i) q = ∆U |
| Column I | Column II |
| 1. Pressure | (i) Intensive property |
| 2. Entropy | (ii) Extensive property |
| 3. Work | (iii) State function |
| 4. Enthalpy | (iv) Path function |
Answer
Answer:
| Column I | Column II |
| 1. Pressure | (i) Intensive property |
| 2. Entropy | (ii) Extensive property |
| 3. Work | (iv) Path function |
| 4. Enthalpy | (iii) State function |
| Column I | Column II |
| 1. Law of Thermodynamics | (i) R |
| 2. Mass, Volume | (ii) ∆G = ∆H – T∆S |
| 3. CP, CV = | (iii) Extensive property |
| 4. Gibbs-Helmholtz equation | (iv) ∆U = q + w |
Answer
Answer:
| Column I | Column II |
| 1. Law of Thermodynamics | (iv) ∆U = q + w |
| 2. Mass, Volume | (iii) Extensive property |
| 3. CP, CV = | (i) R |
| 4. Gibbs-Helmholtz equation | (ii) ∆G = ∆H – T∆S |
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