JEE Advanced (Single Correct MCQs): Thermodynamics

Question 1

The difference between heats of reaction at constant pressure and constant volume for the reaction : 2 C₆H₆(l) + 15O_2(g)→ 12CO₂(g) + 6H₂O(l) at 25ºC in kJ is (1991)

Accepted Answer

&ndash;7.43

Answer

+3.72

Answer

&ndash;3.72

Answer

+7.43

Question 2

For which change ΔH ≠ ΔE : (1995S)

Accepted Answer

N₂(g)+ 3H₂(g) → 2NH₃(g)

Answer

H₂(g) + I₂(g) → 2HI(g)

Answer

HCl + NaOH → NaCl

Answer

C(s) + O₂(g) → CO₂(g)

Question 3

The ΔH⁰_f for CO₂(g), CO(g) and H₂O(g) are –393.5, –110.5 and –241.8 kJ mol^–1 respectively. The standard enthalpy change (in kJ) for the reaction CO₂(g) + H₂(g) → CO(g) + H₂O(g) is (2000S)

Accepted Answer

41.2

Answer

524.1

Answer

&ndash;262.5

Answer

&ndash;41.2

Question 4

In thermodynamics, a process is called reversible when (2001S)

Accepted Answer

the surroundings are always in equilibrium with the system.

Answer

surroundings and system change into each other.

Answer

there is no boundary between system and surroundings.

Answer

the system ch an ges in to the sur r oun dings spontaneously.

Question 5

Which one of the following statements is false? (2001S)

Accepted Answer

Work is a state function.

Answer

Temperature is a state function.

Answer

Change in the state is completely defined when the initial and final states are specified.

Answer

Work appears at the boundary of the system.

Question 6

One mole of a non-ideal gas undergoes a change of state (2.0 atm, 3.0L, 95(K) → (4.0 atm, 5.0 L, 245K) with a change in internal energy, ΔU= 30.0L atm . The change in enthalpy (ΔH) of the process in L atm is (2002S)

Accepted Answer

44.0

Answer

40.0

Answer

42.3

Answer

not defined, because pressure is not constant

Question 7

Which of the reaction defines ΔH^°_f ? (2003S)

Accepted Answer

Answer

Answer

Answer

Question 8

Two moles of an ideal gas is expanded isothermally and reversibly from 1 litre to 10 litre at 300 K. The enthalpy change (in kJ) for the process is (2004S)

Accepted Answer

0 kJ

Answer

11.4 kJ

Answer

– 11.4 kJ

Answer

4.8 kJ

Question 9

The enthalpy of vapourization of liquid is 30 kJ mol^–1 and entropy of vapourization is 75 J mol^–1 K. The boiling point of the liquid at 1 atm is (2004S)

Accepted Answer

400 K

Answer

250 K

Answer

450 K

Answer

600 K

Question 10

The direct conversion of A to B is difficult, hence it is carried out by the following shown path :

Given

where e.u. is the entropy unit, then ΔS_(A→B) is (2006 - 3M, –1)

Accepted Answer

+60 e.u.

Answer

+100 e.u.

Answer

&ndash;60 e.u.

Answer

–100 e.u.

Question 11

The value of log₁₀ K for a reaction A B is (Given : 1 Δ_rH^°_298K=-54.07 kJ mol^-1, Δ_rS^°_298K = 10 JK^–1 mol^–1 and R = 8.314 JK^–1 mol^–1; 2.303 × 8.314 × 298 = 5705) (2007)

Accepted Answer

10

Answer

5

Answer

95

Answer

100

Question 12

For the process H₂O(l) (1 bar, 373 K) → H₂O(g) (1 bar, 373 K), the correct set of thermodynamic parameters is (2007)

Accepted Answer

ΔG = 0, ΔS = +ve

Answer

ΔG = 0, ΔS = –ve

Answer

ΔG = +ve, ΔS = 0

Answer

ΔG = –ve, ΔS = +ve

Question 13

The species which by definition has ZERO standard molar enthalpy of formation at 298 K is (2010)

Accepted Answer

Cl2(g)

Answer

Br2(g)

Answer

H2O(g)

Answer

CH4(g)

Question 14

The standard enthalpies of formation of CO₂(g), H₂O(l) and glucose(s) at 25°C are –400 kJ/mol, –300 kJ/mol and –1300 kJ/mol, respectively. The standard enthalpy of combustion per gram of glucose at 25°C is (JEE Advanced 2013-I)

Accepted Answer

–16.11 kJ

Answer

+2900 kJ

Answer

&ndash;2900 kJ

Answer

+16.11 kJ

Question 15

For the process (JEE Adv. 2014) H₂O(l) → H₂O(g) at T = 100°C and 1 atmosphere pressure, the correct choice is

Accepted Answer

ΔS_system > 0 and ΔS_surroundings < 0

Answer

ΔS_system > 0 and ΔS_surroundings > 0

Answer

ΔS_system< 0 and ΔS_surroundings > 0

Answer

ΔS_system < 0 and ΔS_surroundings < 0

Question 16

One mole of an ideal gas at 300 K in thermal contact with surroundings expands isothermally from 1.0 L to 2.0 L against a constant pressure of 3.0 atm. In this process, the change in entropy of surroundings (ΔS_surr) in JK^–1 is (1 L atm = 101.3 J) (JEE Adv. 2016)

Accepted Answer

&ndash;1.013

Answer

5.763

Answer

1.013

Answer

&ndash;5.763

JEE Advanced (Single Correct MCQs): Thermodynamics Chapter MCQs & solutions

MCQ Practice Test & Solutions: JEE Advanced (Single Correct MCQs): Thermodynamics (16 Questions)

The difference between heats of reaction at constant pressure and constant volume for the reaction : 2 C₆H₆(l) + 15O_2(g)→ 12CO₂(g) + 6H₂O(l) at 25ºC in kJ is (1991)

For which change ΔH ≠ ΔE : (1995S)

The ΔH⁰_f for CO₂(g), CO(g) and H₂O(g) are –393.5, –110.5 and –241.8 kJ mol^–1 respectively. The standard enthalpy change (in kJ) for the reaction CO₂(g) + H₂(g) → CO(g) + H₂O(g) is (2000S)

In thermodynamics, a process is called reversible when (2001S)

Which one of the following statements is false? (2001S)

One mole of a non-ideal gas undergoes a change of state (2.0 atm, 3.0L, 95(K) → (4.0 atm, 5.0 L, 245K) with a change in internal energy, ΔU= 30.0L atm . The change in enthalpy (ΔH) of the process in L atm is (2002S)

Which of the reaction defines ΔH^°_f ? (2003S)

Two moles of an ideal gas is expanded isothermally and reversibly from 1 litre to 10 litre at 300 K. The enthalpy change (in kJ) for the process is (2004S)

The enthalpy of vapourization of liquid is 30 kJ mol^–1 and entropy of vapourization is 75 J mol^–1 K. The boiling point of the liquid at 1 atm is (2004S)

The direct conversion of A to B is difficult, hence it is carried out by the following shown path :
Given

where e.u. is the entropy unit, then ΔS_(A→B) is (2006 - 3M, –1)

The value of log₁₀ K for a reaction A B is (Given : 1 Δ_rH^°_298K=-54.07 kJ mol^-1, Δ_rS^°_298K = 10 JK^–1 mol^–1 and R = 8.314 JK^–1 mol^–1; 2.303 × 8.314 × 298 = 5705) (2007)

For the process H₂O(l) (1 bar, 373 K) → H₂O(g) (1 bar, 373 K), the correct set of thermodynamic parameters is (2007)

The species which by definition has ZERO standard molar enthalpy of formation at 298 K is (2010)

The standard enthalpies of formation of CO₂(g), H₂O(l) and glucose(s) at 25°C are –400 kJ/mol, –300 kJ/mol and –1300 kJ/mol, respectively. The standard enthalpy of combustion per gram of glucose at 25°C is (JEE Advanced 2013-I)

For the process (JEE Adv. 2014) H₂O(l) → H₂O(g) at T = 100°C and 1 atmosphere pressure, the correct choice is

One mole of an ideal gas at 300 K in thermal contact with surroundings expands isothermally from 1.0 L to 2.0 L against a constant pressure of 3.0 atm. In this process, the change in entropy of surroundings (ΔS_surr) in JK^–1 is (1 L atm = 101.3 J) (JEE Adv. 2016)

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JEE Advanced (Single Correct MCQs): Thermodynamics Chapter MCQs & solutions

MCQ Practice Test & Solutions: JEE Advanced (Single Correct MCQs): Thermodynamics (16 Questions)

The difference between heats of reaction at constant pressure and constant volume for the reaction : 2 C6H6(l) + 15O2(g) → 12CO2(g) + 6H2O(l) at 25ºC in kJ is (1991)

For which change ΔH ≠ ΔE : (1995S)

The ΔH0f for CO2(g), CO(g) and H2O(g) are –393.5, –110.5 and –241.8 kJ mol–1 respectively. The standard enthalpy change (in kJ) for the reaction CO2(g) + H2(g) → CO(g) + H2O(g) is (2000S)

In thermodynamics, a process is called reversible when (2001S)

Which one of the following statements is false? (2001S)

One mole of a non-ideal gas undergoes a change of state (2.0 atm, 3.0L, 95(K) → (4.0 atm, 5.0 L, 245K) with a change in internal energy, ΔU= 30.0L atm . The change in enthalpy (ΔH) of the process in L atm is (2002S)

Which of the reaction defines ΔH°f ? (2003S)

Two moles of an ideal gas is expanded isothermally and reversibly from 1 litre to 10 litre at 300 K. The enthalpy change (in kJ) for the process is (2004S)

The enthalpy of vapourization of liquid is 30 kJ mol–1 and entropy of vapourization is 75 J mol–1 K. The boiling point of the liquid at 1 atm is (2004S)

The direct conversion of A to B is difficult, hence it is carried out by the following shown path :Given where e.u. is the entropy unit, then ΔS(A→B) is (2006 - 3M, –1)

The value of log10 K for a reaction A B is (Given : 1 ΔrH°298K =-54.07 kJ mol-1, ΔrS°298K = 10 JK–1 mol–1 and R = 8.314 JK–1 mol–1; 2.303 × 8.314 × 298 = 5705) (2007)

For the process H2O(l) (1 bar, 373 K) → H2O(g) (1 bar, 373 K), the correct set of thermodynamic parameters is (2007)

The species which by definition has ZERO standard molar enthalpy of formation at 298 K is (2010)

The standard enthalpies of formation of CO2(g), H2O(l) and glucose(s) at 25°C are –400 kJ/mol, –300 kJ/mol and –1300 kJ/mol, respectively. The standard enthalpy of combustion per gram of glucose at 25°C is (JEE Advanced 2013-I)

For the process (JEE Adv. 2014) H2O(l) → H2O(g) at T = 100°C and 1 atmosphere pressure, the correct choice is

One mole of an ideal gas at 300 K in thermal contact with surroundings expands isothermally from 1.0 L to 2.0 L against a constant pressure of 3.0 atm. In this process, the change in entropy of surroundings (ΔSsurr) in JK–1 is (1 L atm = 101.3 J) (JEE Adv. 2016)

Chapter-wise Tests for JEE Main & Advanced

Chapter-wise Tests for JEE Main & Advanced

Top Courses for JEE

About this JEE Practice Test

Explore more JEE Study Resources

The difference between heats of reaction at constant pressure and constant volume for the reaction : 2 C₆H₆(l) + 15O_2(g)→ 12CO₂(g) + 6H₂O(l) at 25ºC in kJ is (1991)

The ΔH⁰_f for CO₂(g), CO(g) and H₂O(g) are –393.5, –110.5 and –241.8 kJ mol^–1 respectively. The standard enthalpy change (in kJ) for the reaction CO₂(g) + H₂(g) → CO(g) + H₂O(g) is (2000S)

Which of the reaction defines ΔH^°_f ? (2003S)

The enthalpy of vapourization of liquid is 30 kJ mol^–1 and entropy of vapourization is 75 J mol^–1 K. The boiling point of the liquid at 1 atm is (2004S)

The direct conversion of A to B is difficult, hence it is carried out by the following shown path :
Given

where e.u. is the entropy unit, then ΔS_(A→B) is (2006 - 3M, –1)

The value of log₁₀ K for a reaction A B is (Given : 1 Δ_rH^°_298K=-54.07 kJ mol^-1, Δ_rS^°_298K = 10 JK^–1 mol^–1 and R = 8.314 JK^–1 mol^–1; 2.303 × 8.314 × 298 = 5705) (2007)

For the process H₂O(l) (1 bar, 373 K) → H₂O(g) (1 bar, 373 K), the correct set of thermodynamic parameters is (2007)

The standard enthalpies of formation of CO₂(g), H₂O(l) and glucose(s) at 25°C are –400 kJ/mol, –300 kJ/mol and –1300 kJ/mol, respectively. The standard enthalpy of combustion per gram of glucose at 25°C is (JEE Advanced 2013-I)

For the process (JEE Adv. 2014) H₂O(l) → H₂O(g) at T = 100°C and 1 atmosphere pressure, the correct choice is

One mole of an ideal gas at 300 K in thermal contact with surroundings expands isothermally from 1.0 L to 2.0 L against a constant pressure of 3.0 atm. In this process, the change in entropy of surroundings (ΔS_surr) in JK^–1 is (1 L atm = 101.3 J) (JEE Adv. 2016)