Question 1: Palette 1/32

JEE Advanced 2026 MCQ

An ideal gas (0.5 mol), initially at 2 bar pressure, is compressed at a constant temperature of 600 K in two steps: first, against a constant external pressure of P bar (2 < P < 8), and then against constant external pressure of 8 bar. At each step, the compression is stopped only when the pressure of the gas becomes equal to the external pressure. The total work done on the gas in these steps is W. Considering all possible values of P (2 < P < 8) and taking the gas constant as R (in J K⁻¹ mol⁻¹), the minimum value of |W| (in J) is

A

207R

B

600R

C

630R

D

900R

Question 2: Palette 2/32

JEE Advanced 2026 MCQ

List-I contains various physical/chemical processes, and List-II contains combinations of changes in enthalpy ($\Delta H$) and entropy ($\Delta S$). Match each entry in List-I to the appropriate entry in List-II, and choose the correct option.

List-I	List-II
(P) Physisorption	(1) $\Delta H > 0 \text{ and } \Delta S > 0$
(Q) Diamond $\rightarrow$ Graphite	(2) $\Delta H < 0 \text{ and } \Delta S < 0$
(R) Denaturation of protein	(3) $\Delta H < 0 \text{ and } \Delta S = 0$
(S) Propene $\rightarrow$ Cyclopropane	(4) $\Delta H > 0 \text{ and } \Delta S < 0$
	(5) $\Delta H < 0 \text{ and } \Delta S > 0$

A

P → 2; Q → 3; R → 5; S → 4

B

P → 4; Q → 3; R → 5; S → 1

C

P → 2; Q → 5; R → 1; S → 4

D

P → 2; Q → 5; R → 1; S → 3

Question 3: Palette 3/32

JEE Advanced 2022 MSQ

The correct option(s) about entropy (S) is(are)

$[\mathrm{R}=$ gas constant, $\mathrm{F}=$ Faraday constant, $\mathrm{T}=$ Temperature $]$

A

For the reaction, $\mathrm{M}(s)+2 \mathrm{H}^{+}(a q) \rightarrow \mathrm{H}_{2}(g)+\mathrm{M}^{2+}(a q)$, if $\frac{d E_\text{cell}}{d T}=\frac{R}{F}$, then the entropy change of the reaction is $\mathrm{R}$ (assume that entropy and internal energy changes are temperature independent).

B

The cell reaction, $\operatorname{Pt}(s) \mid \mathrm{H}_{2}(g, 1$ bar $)\left|\mathrm{H}^{+}(a q, 0.01 \mathrm{M}) \| \mathrm{H}^{+}(a q, 0.1 \mathrm{M})\right| \mathrm{H}_{2}(g, 1 \mathrm{bar}) \mid \operatorname{Pt}(s)$, is an entropy driven process.

C

For racemization of an optically active compound, $\Delta \mathrm{S}>0$.

D

$\Delta \mathrm{S}>0$, for $\left[\mathrm{Ni}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}+3$ en $\rightarrow\left[\mathrm{Ni}(\mathrm{en})_{3}\right]^{2+}+6 \mathrm{H}_{2} \mathrm{O}$ (where en $=$ ethylenediamine).

Question 4: Palette 4/32

JEE Advanced 2021 MSQ

An ideal gas undergoes a reversible isothermal expansion from state I to state II followed by a reversible adiabatic expansion from state II to state III. The correct plot(s) representing the changes from state I to state III is (are)

(p : pressure, V : volume, T : temperature, H : enthalpy, S : entropy)

A

B

C

D

Question 5: Palette 5/32

JEE Advanced 2020 MSQ

In thermodynamics, the p-V work done is given by

$w = - \int {dV{p_{ext}}} $

For a system undergoing a particular process, the work done is

$w = - \int {dV\left( {{{RT} \over {V - b}} - {a \over {{V^2}}}} \right)} $

This equation is applicable to a

A

system that satisfies the van der Walls' equation of state

B

process that is reversible and isothermal

C

process that is reversible and adiabatic

D

process that is irreversible and at constant pressure

Question 6: Palette 6/32

JEE Advanced 2019 MSQ

Choose the reaction(s) from the following options, for which the standard enthalpy of reaction of equal to the standard enthalpy of formation.

A

2C(g) + 3H₂(g) $ \to $ C₂H₆(g)

B

2H₂(g) + O₂(g) $ \to $ 2H₂O(l)

C

${3 \over 2}$O₂(g) $ \to $ O₃(g)

D

${1 \over 8}$S₈(s) + O₂(g) $ \to $ SO₂(g)

Question 7: Palette 7/32

JEE Advanced 2019 MSQ

Which of the following statement(s) is(are) correct regarding the root mean square speed (U_rms) and average translational kinetic energy (E_av) of a molecule in a gas at equilibrium?

A

U_rms is inversely proportional to the square root of its molecular mass.

B

U_rms is doubled when its temperature is increased four times.

C

E_avg is doubled when its temperature is increased four times.

D

E_avg at a given temperature does not depend on its molecular mass.

Question 8: Palette 8/32

JEE Advanced 2018 MSQ

For a reaction, $A\,\,\rightleftharpoons\,\,P,$ the plots of $\left[ A \right]$ and $\left[ P \right]$ with time at temperature ${T_1}$ and ${T_2}$ are given below.


If ${T_2} > {T_1},$ the correct statement(s) is (are) (Assume $\Delta {H^ \circ }$ and $\Delta {S^ \circ }$ are independent of temperature and ratio of $lnK$ at ${T_1}$ to $lnK$ at ${T_2}$ is greater than ${{{T_2}} \over {{T_1}}}.$ Here $H,$ $S,G$ and $K$ are enthalpy, entropy, Gibbs energy and equilibrium constant, respectively.)

A

$\Delta {H^ \circ } < 0,\Delta {S^ \circ } < O$

B

$\Delta {G^ \circ } < 0,\Delta {H^ \circ } > 0$

C

$\Delta {G^ \circ } < 0,\Delta {S^ \circ } < 0$

D

$\Delta {G^ \circ } < 0,\Delta {S^ \circ } > 0$

Question 9: Palette 9/32

JEE Advanced 2018 MSQ

A reversible cyclic process for an ideal gas is shown below. Here, $P, V,$ and $T$ are pressure, volume and temperature, respectively. The thermodynamic parameters $q,w, H$ and $U$ are heat, work, enthalpy and internal energy, respectively.



The correct option(s) is (are)

A

${q_{Ac}} = \Delta {U_{BC}}\,\,$ and ${w_{AB}} = {P_2}\left( {{V_2} - {V_1}} \right)$

B

${w_{BC}} = {P_2}\left( {{V_2} - {V_1}} \right)\,\,$ and ${q_{BC}} = \Delta {H_{AC}}$

C

$\Delta {H_{CA}} < \Delta {U_{CA}}\,\,$ and $\,\,{q_{AC}} = \Delta {U_{BC}}$

D

$\,\,{q_{BC}} = \Delta {H_{AC}}\,\,$ and $\Delta {H_{CA}} > \Delta {U_{CA}}$

Question 10: Palette 10/32

JEE Advanced 2017 MSQ

For a reaction taking place in a container in equilibrium with its surroundings, the effect of temperature on its equilibrium constant $K$ in terms of change in entropy is described by

A

With increase in temperature, the value of $K$ for exothermic reaction decreases because the entropy change of the system is positive

B

With increase in temperature, the value of $K.$ for endothermic reaction increases because unfavorable change in entropy of the surroundings decreases

C

With increase in temperature, the value of $K$ for endothermic reaction increases because the entropy change of the system is negative

D

with increase in temperature, the value of $K$ for exothermic reaction decreases because favorable change in entropy of the surroundings decreases

Question 11: Palette 11/32

JEE Advanced 2017 MSQ

An ideal gas is expanded from $\left( {{p_1},{V_1},{T_1}} \right)$ to $\left( {{p_2},{V_2},{T_2}} \right)$ under different conditions. The correct statement(s) among the following is (are)

A

The work done on the gas is maximum when it is compressed irreversibly from $\left( {{p_2},{V_2}} \right)$ to $\left( {{p_1},{V_1}} \right)$ against constant pressure ${p_1}$

B

If the expansion is carried out freely, it is simultaneously both isothermal as well as adiabatic

C

The work done by the gas is less when it is expanded reversibly from ${V_1}$ to ${V_2}$ under adiabatic conditions as compared to that when expanded reverseibly from ${V_1}$ to ${V_2}$ under isothermal conditions

D

The change in internal energy of the gas is (i) zero, if it is expanded reversibly with ${T_1} = {T_2}$ , and (ii) positive, if it is expanded reversibly under adiabatic conditions with ${T_1}\, \ne \,{T_2}$

Question 12: Palette 12/32

JEE Advanced 2017 MCQ

The standard state Gibbs free energies of formation of $C$(graphite) and $C$(diamond) at $T=298$ $K$ are

${\Delta _f}{G^0}$ [$C$(graphite)] $ = 0kJmo{l^{ - 1}}$

${\Delta _f}{G^0}$ [$C$(diamond)] $ = 2.9kJmo{l^{ - 1}}$

The standard state means that the pressure should be $1$ bar, and substance should be pure at a given temperature. The conversion of graphite [$C$(graphite)] to diamond [$C$(diamond)] reduces its volume by $2 \times {10^{ - 6}}\,{m^3}\,mo{l^{ - 1}}$ If $C$(graphite) is converted to $C$(diamond) isothermally at $T=298$ $K,$ the pressure at which $C$(graphite) is in equilibrium with $C$(diamond), is

[Useful information : $1$ $J=1$ $kg\,{m^2}{s^{ - 2}};1\,Pa = 1\,kg\,{m^{ - 1}}{s^{ - 2}};$ $1$ bar $ = {10^5}$ $Pa$]

A

$14501$ bar

B

$58001$ $bar$

C

$1450$ bar

D

$29001$ bar

Question 13: Palette 13/32

JEE Advanced 2016 MCQ

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 surrounding ($\Delta$S_surr)in JK^–1 is (1L atm = 101.3 J)

A

5.763

B

1.013

C

– 1.013

D

– 5.763

Question 14: Palette 14/32

JEE Advanced 2015 MCQ

Match the thermodynamics processes given under column I with expression given under column II

Column I
(A) Freezing water at 273 K and 1 atm
(B) Expansion of 1 mol of an ideal gas into a vacuum under isolated conditions.
(C) Mixing of equal volumes of two ideal gases at constant temperature and pressure in an isolated container.
(D) Reversible heating of H₂(g) at 1 atm from 300K to 600K, followed by reversible cooling to 300K at 1 atm

Column II
(p) q = 0
(q) w = 0
(r) $\Delta S_{sys}$ < 0
(s) $\Delta U$ = 0
(t) $\Delta G$ = 0

A

A $\to$ r,t; B $\to$ q,s; C $\to$ p,s; D $\to$ p,q,s;

B

A $\to$ r,t; B $\to$ p,s; C $\to$ s; D $\to$ q,s,t;

C

A $\to$ r,t; B $\to$ p,q,s; C $\to$ p,q,s; D $\to$ p,q,s,t;

D

A $\to$ r,t; B $\to$ p,s; C $\to$ p,q,s; D $\to$ p,s,t;

Question 15: Palette 15/32

JEE Advanced 2014 MCQ

For the process
H₂O(l) $\to$ H₂O(g)
at T = 100^oC and 1 atmosphere pressure, the correct choice is

A

$\Delta S$_system > 0 and $\Delta S$_surroundings > 0

B

$\Delta S$_system > 0 and $\Delta S$_surroundings < 0

C

$\Delta S$_system < 0 and $\Delta S$_surroundings > 0

D

$\Delta S$_system < 0 and $\Delta S$_surroundings < 0

Question 16: Palette 16/32

JEE Advanced 2013 MSQ

Benzene and naphthalene form an ideal solution at room temperature. For this process, the true statement(s) is(are)

A

$\Delta G$ is positive

B

$\Delta S_{system}$ is positive

C

$\Delta S_{surroundings}$ = 0

D

$\Delta H$ = 0

Question 17: Palette 17/32

JEE Advanced 2013 MCQ

The succeeding operations that enable this transformation of states are

A

Heating, cooling, heating, cooling.

B

Cooling, heating, cooling, heating.

C

Heating, cooling, cooling, heating.

D

Cooling, heating, heating, cooling.

Question 18: Palette 18/32

JEE Advanced 2013 MCQ

The pair of isochoric processes among the transformation of states is

A

K to L and L to M

B

L to M and N to K

C

L to M and M to N

D

M to N and N to K

Question 19: Palette 19/32

JEE Advanced 2013 MCQ

The standard enthalpies of formation of CO₂(g), H₂O(l) and glucose(s) at 25^oC are –400 kJ/mol, –300 kJ/mol and –1300 kJ/mol, respectively. The standard enthalpy of combustion per gram of glucose at 25^oC is

A

+2900 kJ

B

– 2900 kJ

C

–16.11 kJ

D

+16.11 kJ

Question 20: Palette 20/32

JEE Advanced 2012 MSQ

The reversible expansion of an ideal gas under adiabatic and isothermal conditions is shown in the figure. Which of the following statement(s) is(are) correct?

A

T₁ = T₂

B

T₃ > T₁

C

w_isothermal > w_adiabatic

D

$\Delta$U_isothermal > $\Delta$U_adiabatic

Question 21: Palette 21/32

JEE Advanced 2012 MSQ

For an ideal gas, consider only P-V work in going from an initial state X to the final state Z. The final state Z can be reached by either of the two paths shown in the figure. Which of the following choice(s) is(are) correct? (Take $\Delta$S as change in entropy and W as work done)

A

$\Delta {S_{X \to Z}} = \Delta {S_{X \to Y}} + \Delta {S_{Y \to Z}}$

B

$\Delta {W_{X \to Z}} = \Delta {W_{X \to Y}} + \Delta {W_{Y \to Z}}$

C

${W_{X \to Y \to Z}} = {W_{X \to Y}}$

D

$\Delta {S_{X \to Y \to Z}} = \Delta {S_{X \to Y}}$

Question 22: Palette 22/32

JEE Advanced 2012 MCQ

Using the data provided, calculate the multiple bond energy (kJ mol^$-$1) of a C=C bond in C₂H₂. That energy is (take the bond energy of C-H bond as 350 kJ mol^$-$1).

$\matrix{ \hfill {2C(s) + {H_2}(g) \to {C_2}{H_2}} & \hfill {\Delta H = 225\,kJ\,mo{l^{ - 1}}} \cr \hfill {2C(s) \to 2C(g)} & \hfill {\Delta H = 1410\,kJ\,mo{l^{ - 1}}} \cr \hfill {{H_2}(g) \to 2H(g)} & \hfill {\Delta H = 330\,kJ\,mo{l^{ - 1}}} \cr } $

A

1165 kJ mol^$-$1

B

837 kJ mol^$-$1

C

865 kJ mol^$-$1

D

815 kJ mol^$-$1

Question 23: Palette 23/32

JEE Advanced 2011 MCQ

Match the transformations in column I with appropriate options in column II

Column I
(A) CO₂(s) $\to$ CO₂(g)
(B) CaCO₃(s) $\to$ CaO(s) + CO₂(g)
(C) 2H $\to$ H₂(g)
(D) P_{(white, solid)} $\to$ P_{(red, solid)}

Column II
(p) phase transition
(q) allotropic change
(r) $\Delta H$ is positive
(s) $\Delta S$ is positive
(t) $\Delta S$ is negative

A

A $\to$ p,r,s; B $\to$ r,s; C $\to$ t; D $\to$ p,q,t

B

A $\to$ r,s; B $\to$ p,s; C $\to$ t; D $\to$ p,q,t

C

A $\to$ p,r,s; B $\to$ r,s; C $\to$ r; D $\to$ p,t

D

A $\to$ p,r,s; B $\to$ r,s; C $\to$ t; D $\to$ q,t

Question 24: Palette 24/32

JEE Advanced 2010 MSQ

Among the following, the intensive property is (properties are)

A

molar conductivity

B

electromotive force

C

resistance

D

heat capacity

Question 25: Palette 25/32

JEE Advanced 2010 MCQ

The bond energy (in kcal mol^-1) of a C-C single bond is approximately

A

1

B

10

C

100

D

1000

Question 26: Palette 26/32

JEE Advanced 2010 MCQ

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

A

Br₂ (g)

B

Cl₂ (g)

C

H₂O (g)

D

CH₄ (g)

Question 27: Palette 27/32

JEE Advanced 2009 MSQ

Among the following, the state function(s) is(are)

A

Internal energy.

B

Irreversible expansion work.

C

Reversible expansion work.

D

Molar enthalpy.

Question 28: Palette 28/32

JEE Advanced 2008 MCQ

Statement 1 : There is a natural asymmetry between converting work to heat and converting heat to work.

Statement 2 : No process is possible in which the sole result is the absorption of heat from a reservoir and its complete conversion into work.

A

Statement 1 is True, Statement 2 is True; Statement 2 is a CORRECT explanation for Statement 1.

B

Statement 1 is True, Statement 2 is True; Statement 2 is a NOT CORRECT explanation for Statement 1.

C

Statement 1 is True, Statement 2 is False.

D

Statement 1 is False, Statement 2 is True.

Question 29: Palette 29/32

JEE Advanced 2007 MCQ

For the process $\mathrm{H_2O}(l)$ (1 bar, 373 K) $\to$ $\mathrm{H_2O}(g)$ (1 bar, 373 K), the correct set of thermodynamic parameters is:

A

$\mathrm{\Delta G=0,\Delta S=+ve}$

B

$\mathrm{\Delta G=0,\Delta S=-ve}$

C

$\mathrm{\Delta G=-ve,\Delta S=0}$

D

$\mathrm{\Delta G=-ve,\Delta S=+ve}$

Question 30: Palette 30/32

JEE Advanced 2007 MCQ

The value of log$_{10}$ K for a reaction $A \rightleftharpoons B$ is

(Given : ${\Delta _r}H{^\circ _{298\,K}} = - 54.07$ kJ mol$^{-1}$, ${\Delta _r}S{^\circ _{298\,K}} = 10$ J K$^{-1}$ mol$^{-1}$ and R = 8.314 J K$^{-1}$ mol$^{-1}$; 2.303 $\times$ 8.314 $\times$ 298 = 5705)

A

5

B

10

C

95

D

100

Question 31: Palette 31/32

JEE Advanced 2006 MCQ

A monatomic ideal gas undergoes a process in which the ratio of P to V at any instant is constant and equals to 1 . What is the molar heat capacity of the gas?

A

$\frac{4 R}{2}$

B

$\frac{3 R}{2}$

C

$\frac{5 R}{2}$

D

0

Question 32: Palette 32/32

JEE Advanced 2006 MCQ

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

$ \begin{aligned} & \Delta \mathrm{S}_{(\mathrm{A} \rightarrow \mathrm{C})}=50 \text { e.u. } \\ & \Delta \mathrm{S}_{(\mathrm{C} \rightarrow \mathrm{D})}=30 \text { e.u. } \\ & \Delta \mathrm{S}_{(\mathrm{B} \rightarrow \mathrm{D})}=20 \text { e.u. } \end{aligned} $

Where e.u. is entropy unit. Then $\Delta \mathrm{S}_{(\mathrm{A} \rightarrow \mathrm{B})}$ is :

A

+100 e.u.

B

+60 e.u.

C

-100 e.u.

D

-60 e.u.