Thermodynamics

Arrange the following in order of magnitude of work done by the system / on the system at constant temperature :
(a) \(\left|{\mathrm{w}}_{\text{reversible }}\right|\) for expansion in infinite stage.
(b) \(\left|{\mathrm{w}}_{\text{irreversible }}\right|\) for expansion in single stage.
(c) \(\left|{\mathrm{w}}_{\text{reversible }}\right|\) for compression in infinite stage.
(d) \(\left|{\mathrm{W}}_{\text{irreversible }}\right|\) for compression in single stage.
Choose the correct answer from the options given below

[JEE Main 2025, 2 Apr (Shift 2)]

The combustion of benzene (L) gives\(C{O}_{2}\) (g) and \({H}_{2}O\) (L). Given that heat of combustion of benzene at constant volume is -3263.9 kJ/mol at 25°C, heat of combustion (in kJ/mol) of benzene at constant pressure will be: (R = 8.314J\({K}^{-1}mo{l}^{-1}\))

Given :
\({\mathrm{ΔH}}_{\text{sub }}^{⊖}[\mathrm{C}\text{ (graphite) }]=710\mathrm{kJ}{\mathrm{mol}}^{-1}\\ {\Delta }_{\mathrm{C}-\mathrm{H}}{\mathrm{H}}^{⊖}=414\mathrm{kJ}{\mathrm{mol}}^{-1}\\ {\Delta }_{\mathrm{H}-\mathrm{H}}{\mathrm{H}}^{⊖}=436\mathrm{kJ}{\mathrm{mol}}^{-1}\\ {\Delta }_{\mathrm{C}=\mathrm{C}}{\mathrm{H}}^{⊖}=611\mathrm{kJ}{\mathrm{mol}}^{-1}\)
The \(\Delta {\mathrm{H}}_{\mathrm{f}}^{⊖}\) for \({\mathrm{CH}}_{2}={\mathrm{CH}}_{2}\) is ________ \({\mathrm{kJmol}}^{-1}\) (nearest integer value)

[JEE Main 2025, 3 Apr (Shift 1)]

Which of the following is not correct?

Let us consider an endothermic reaction which is non-spontaneous at the freezing point of water. However, the reaction is spontaneous at boiling point of water. Choose the correct option

Consider the given data:
(a) \(\mathrm{HCl}(\mathrm{g})+10{\mathrm{H}}_{2}\mathrm{O}(\mathrm{l})\to \mathrm{HCl}.10{\mathrm{H}}_{2}\mathrm{O}\\ \mathrm{ΔH}=-69.01\mathrm{kJ}{\mathrm{mol}}^{-1}\)
(b) \(\mathrm{HCl}(\mathrm{g})+40{\mathrm{H}}_{2}\mathrm{O}(\mathrm{l})\to \mathrm{HCl}.40{\mathrm{H}}_{2}\mathrm{O}\\ \mathrm{ΔH}=-72.79\mathrm{kJ}{\mathrm{mol}}^{-1}\)
Choose the correct statement :

[JEE Main 2025, 4 Apr (Shift 2)]

If \(C\) (diamond) \(\to C\) (graphite)+X \(kJmo{l}^{-1}\)
\(C(\text{ diamond })+{O}_{2}(g)\to C{O}_{2}(g)+YkJmo{l}^{-1}\)
C (graphite) \(+{O}_{2}(g)\to C{O}_{2}(g)+ZkJmo{l}^{-1}\)

at constant temperature. Then

[JEE Main 2025, 29 Jan (Shift 2)]

By using relation
\(∆\mathrm{G}=∆\mathrm{H}-\mathrm{T}∆\mathrm{S}\)

Which of the following is incorrect for spontaneous reaction at a given temperature?

(Memory Based JEE Mains 23/01/2025 ,Shift -2)

Energy supplied to 1 mole of monoatomic gas is \(48\mathrm{J}\) and changes its temperature by \(2^\circ \mathrm{C}\). Find the work done by gas.

Adiabatic constant of gas is 3/2. If volume of gas initially at \({0}^{\mathrm{o}}\mathrm{C}\) is reduced to one-fourth of the original volume then new temperature is (memory based jee mains shift-1 23/01/2025)

Energy supplied to 1 mole of monoatomic gas is \(48\mathrm{J}\) and changes its temperature by \(2^\circ \mathrm{C}\). Find the work done by gas.

Consider the following thermochemical reaction and choose the correct option

\(\mathrm{C}(\mathrm{diamond})\to \mathrm{C}(\mathrm{graphite})+\mathrm{x}\mathrm{KJ}\\ \mathrm{C}(\mathrm{diamond})+{\mathrm{O}}_{2}\to {\mathrm{CO}}_{2}+\mathrm{y}\mathrm{KJ}\\ \mathrm{C}(\mathrm{graphite})+{\mathrm{O}}_{2}\to {\mathrm{CO}}_{2}+\mathrm{z}\mathrm{KJ}\)

29/Jan/25 Evening shift

A liquid when kept inside a thermally insulated closed vessel at 25 degree celsius was mechanically stirred from outside. What will be the correct option for the following thermodynamic parameters?

[JEE Main 2025, 22 Jan (Shift 1)]

The correct statement amongst the following is

[JEE Main 2025, 7 Apr (Shift 2)]

Consider the following thermochemical reaction and choose the correct option

\(\mathrm{C}(\mathrm{diamond})\to \mathrm{C}(\mathrm{graphite})+\mathrm{x}\mathrm{KJ}\\ \mathrm{C}(\mathrm{diamond})+{\mathrm{O}}_{2}\to {\mathrm{CO}}_{2}+\mathrm{y}\mathrm{KJ}\\ \mathrm{C}(\mathrm{graphite})+{\mathrm{O}}_{2}\to {\mathrm{CO}}_{2}+\mathrm{z}\mathrm{KJ}\)

29/Jan/25 Evening shift

If \(C\) (diamond) \(\to C\) (graphite)+X \(kJmo{l}^{-1}\)
\(C(\text{ diamond })+{O}_{2}(g)\to C{O}_{2}(g)+YkJmo{l}^{-1}\)
C (graphite) \(+{O}_{2}(g)\to C{O}_{2}(g)+ZkJmo{l}^{-1}\)

at constant temperature. Then

By using relation
\(∆\mathrm{G}=∆\mathrm{H}-\mathrm{T}∆\mathrm{S}\)

Which of the following is incorrect for spontaneous reaction at a given temperature?

(Memory Based JEE Mains 23/01/2025 ,Shift -2)

Given ionisation enthalpy of element \({\mathrm{E}}_{(\mathrm{g})}\) is 300 kJ / mol and electron gain enthalpy of A,B,C and D gases atoms are -320 kJ / mol,-340 kJ / mol ,-200 kJ / mol and -250 kJ / mol, then what will be the correct order of ionic nature of compounds?

Let us consider an endothermic reaction which is non-spontaneous at the freezing point of water. However, the reaction is spontaneous at boiling point of water. Choose the correct option.

[JEE Main 2025, 24 Jan (Shift 1)]

The correct statement amongst the following is

\(S(g)+\frac{3}{2}{O}_{2}(g)\to S{O}_{3}(g)+2xkcal\\ S{O}_{2}(g)+\frac{1}{2}{O}_{2}(g)\to S{O}_{3}(g)+ykcal\)

The heat of formation of \(S{O}_{2}(g)\) is given by

Let us consider a reversible reaction at temperature, T .
In this reaction, both \(\Delta \mathrm{H}\) and \(\Delta \mathrm{S}\) were observed to have positive values. If the equilibrium temperature is Te , then the reaction becomes spontaneous at

[JEE Main 2025, 4 Apr (Shift 1)]

The standard Gibbs energy \(\left(∆{G}^{^\circ }\right)\) for the following reaction is \(A(s)+{B}^{+2}(aq)⇌{A}^{+2}(aq)+B(s),Kc={10}^{12}at\) (Kc = equilibrium constant)

Given ionisation enthalpy of element \({\mathrm{E}}_{(\mathrm{g})}\) is 300 kJ / mol and electron gain enthalpy of A,B,C and D gases atoms are -320 kJ / mol,-340 kJ / mol ,-200 kJ / mol and -250 kJ / mol, then what will be the correct order of ionic nature of compounds?

A sample of n-octane \((1.14\mathrm{g})\) was completely burnt in excess of oxygen in a bomb calorimeter, whose heat capacity is \(5\mathrm{kJ}{\mathrm{K}}^{-1}\). As a result of combustion reaction, the temperature of the calorimeter is increased by \(5\mathrm{K}\) . The magnitude of the heat of combustion of octane at constant volume is _____ \({\mathrm{kJmol}}^{-1}\) (nearest integer).

The standard Gibbs energy \(\left(∆{G}^{^\circ }\right)\) for the following reaction is \(A(s)+{B}^{+2}(aq)⇌{A}^{+2}(aq)+B(s),Kc={10}^{12}at\) (Kc = equilibrium constant)

Let us consider a reversible reaction at temperature, T .
In this reaction, both \(\Delta \mathrm{H}\) and \(\Delta \mathrm{S}\) were observed to have positive values. If the equilibrium temperature is Te , then the reaction becomes spontaneous at

[JEE Main 2025, 4 Apr (Shift 1)]

The formation enthalpies, \(\Delta {{H}_{f}}^{⊖}\) for \({H}_{(g)}\) and \({O}_{(g)}\) are 220.0 and \(250.0kJmo{l}^{-1}\), respectively, at 298.15 K , and \(\Delta {{H}_{f}}^{⊖}\) for \({H}_{2}{O}_{(g)}\)is \(-242.0kJmo{l}^{-1}\) at the same temperature. The average bond enthalpy of the \(O-H\) bond in water at 298.15 K is _______ \(kJmo{l}^{-1}\) (nearest integer)

[JEE Main 2025, 28 Jan (Shift 1)]

In a closed insulated container, a liquid is stirred with a paddle to increase the temperature, which of the following is true?

A liquid when kept inside a thermally insulated closed vessel at 25 degree celsius was mechanically stirred from outside. What will be the correct option for the following thermodynamic parameters?

[JEE Main 2025, 22 Jan (Shift 1)]

If \(C\) (diamond) \(\to C\) (graphite)+X \(kJmo{l}^{-1}\)
\(C(\text{ diamond })+{O}_{2}(g)\to C{O}_{2}(g)+YkJmo{l}^{-1}\)
C (graphite) \(+{O}_{2}(g)\to C{O}_{2}(g)+ZkJmo{l}^{-1}\)

at constant temperature. Then

500 J of energy is transferred as heat to 0.5 mol of Argon gas at 298 K and 1.00 atm . The final temperature and the change in internal energy respectively are
(Given : \(\mathrm{R}=8.3{\mathrm{JK}}^{-1}{\mathrm{mol}}^{-1}\))

[JEE Main 2025, 29 Jan (Shift 1)]

By using relation
\(∆\mathrm{G}=∆\mathrm{H}-\mathrm{T}∆\mathrm{S}\)

Which of the following is incorrect for spontaneous reaction at a given temperature?

(Memory Based JEE Mains 23/01/2025 ,Shift -2)

Consider the given data:
(a) \(\mathrm{HCl}(\mathrm{g})+10{\mathrm{H}}_{2}\mathrm{O}(\mathrm{l})\to \mathrm{HCl}.10{\mathrm{H}}_{2}\mathrm{O}\mathrm{ΔH}=-69.01\mathrm{kJ}{\mathrm{mol}}^{-1}\)
(b) \(\mathrm{HCl}(\mathrm{g})+40{\mathrm{H}}_{2}\mathrm{O}(\mathrm{l})\to \mathrm{HCl}.40{\mathrm{H}}_{2}\mathrm{O}\mathrm{ΔH}=-72.79\mathrm{kJ}{\mathrm{mol}}^{-1}\)
Choose the correct statement :

[JEE Main 2025, 4 Apr (Shift 2)]

One mole of an ideal gas expands isothermally and reversibly from \(10{\mathrm{dm}}^{3}\) to \(20{\mathrm{dm}}^{3}\) at \(300\mathrm{K}.\mathrm{ΔU}\), q and work done in the process respectively are :
Given : \(\mathrm{R}=8.3{\mathrm{JK}}^{-1}{\mathrm{mol}}^{-1}\)
In \(10=2.3\)
\(\log 2=0.30\)
\(\log 3=0.48\)

[JEE Main 2025, 4 Apr (Shift 1)]

The combustion of benzene (L) gives\(C{O}_{2}\) (g) and \({H}_{2}O\) (L). Given that heat of combustion of benzene at constant volume is -3263.9 kJ/mol at 25°C, heat of combustion (in kJ/mol) of benzene at constant pressure will be: (R = 8.314J\({K}^{-1}mo{l}^{-1}\))

One mole of an ideal gas expands isothermally and reversibly from \(10{\mathrm{dm}}^{3}\) to \(20{\mathrm{dm}}^{3}\) at \(300\mathrm{K}.\mathrm{ΔU}\), q and work done in the process respectively are :
Given : \(\mathrm{R}=8.3{\mathrm{JK}}^{-1}{\mathrm{mol}}^{-1}\)
In \(10=2.3\)
\(\log 2=0.30\)
\(\log 3=0.48\)

[JEE Main 2025, 4 Apr (Shift 1)]

For an ideal monoatomic gas undergoing an isobaric process, the ratio of \(\frac{∆\mathrm{Q}}{∆\mathrm{U}}\) is (memory based jee mains shift-1 24/01/2025)

Arrange the following in order of magnitude of work done by the system / on the system at constant temperature :
(a) \(\left|{\mathrm{w}}_{\text{reversible }}\right|\) for expansion in infinite stage.
(b) \(\left|{\mathrm{w}}_{\text{irreversible }}\right|\) for expansion in single stage.
(c) \(\left|{\mathrm{w}}_{\text{reversible }}\right|\) for compression in infinite stage.
(d) \(\left|{\mathrm{W}}_{\text{irreversible }}\right|\) for compression in single stage.
Choose the correct answer from the options given below

[JEE Main 2025, 2 Apr (Shift 2)]

Combustion of 1 mole of benzene is expressed at
\({C}_{6}{H}_{6}(l)+\frac{15}{2}{O}_{2}(g)\to 6C{O}_{2}(g)+3{H}_{2}O(l)\text{. }\)

The standard enthalpy of combustion of 2 mol of benzene is \({{}^{'}x}^{'}kJ\).
\(x=\)__________

Given :
1. Standard Enthalpy of formation of 1 mol of \({C}_{6}{H}_{6}(l)\) , for the reaction \(6\mathrm{C}\)(graphite) \(+3{H}_{2}(g)\to {C}_{6}{H}_{6}(l)\) is 48.5 kJ/mol
2. Standard Enthalpy of formation of 1 mol of \(C{O}_{2}(g)\), for the reaction \(\mathrm{C}\)(graphite)\(+{O}_{2}(g)\to C{O}_{2}(g)\) is -393.5 kJ/mol
3. Standard and Enthalpy of formation of 1 mol of \({H}_{2}O(l)\) , for the reaction \({H}_{2}(g)+\frac{1}{2}{O}_{2}(g)\to {H}_{2}O(l)\) -286 kJ/mol

[JEE Main 2024, 5 Apr (Shift 2)]

\(S(g)+\frac{3}{2}{O}_{2}(g)\to S{O}_{3}(g)+2xkcal\\ S{O}_{2}(g)+\frac{1}{2}{O}_{2}(g)\to S{O}_{3}(g)+ykcal\)

The heat of formation of \(S{O}_{2}(g)\) is given by

Consider the following data :
Heat of formation of \(C{O}_{2}(g)=-393.5kJmo{l}^{-1}\)
Heat of formation of \({H}_{2}O(l)=-286.0kJmo{l}^{-1}\)
Heat of combustion of benzene \(=-3267.0kJmo{l}^{-1}\)
The heat of formation of benzene is ______ \(kJmo{l}^{-1}\).
(Nearest integer)

[JEE MAINS 2025, 20 Feb, Shift-1]

Identify the correct option regarding extensive and intensive property (memory based jee mains shift-2 22/01/2025)

In the process, pressure of gas is directly proportional to temperature then choose correct option (MEMORY based jee mains shift-1 24/01/2025)

A: Process is isochoric

B: Work done in process is zero

C: Internal energy increases with increase in temperature

Given below are two statements: One is labelled as Assertion (A) and the other is labelled as Reason (R)

Assertion (A) : Enthalpy of neutralisation of strong monobasic acid with strong monoacidic base is always -57 kJ/mol.

Reason (R) : Enthalpy of neutralisation is the amount of heat liberated when one mole of \({H}^{+}\) ions furnished by acid combine with one mole of \({\mathrm{OH}}^{-}\) ions furnished by base to form one mole of water.

In the light of the above statements, choose the correct answer from the options given below

[JEE Main 2024, 05 Apr (Shift 1)]

Given below are two statements: One is labelled as Assertion (A) and the other is labelled as Reason (R)

Assertion (A) : Enthalpy of neutralisation of strong monobasic acid with strong monoacidic base is always -57 kJ/mol.

Reason (R) : Enthalpy of neutralisation is the amount of heat liberated when one mole of \({H}^{+}\) ions furnished by acid combine with one mole of \({\mathrm{OH}}^{-}\) ions furnished by base to form one mole of water.

In the light of the above statements, choose the correct answer from the options given below

[JEE Main 2024, 05 Apr (Shift 1)]

Consider the following data :
Heat of formation of \(C{O}_{2}(g)=-393.5kJmo{l}^{-1}\)
Heat of formation of \({H}_{2}O(l)=-286.0kJmo{l}^{-1}\)
Heat of combustion of benzene \(=-3267.0kJmo{l}^{-1}\)
The heat of formation of benzene is ______ \(kJmo{l}^{-1}\).
(Nearest integer)

[JEE Main 2025, 28 Jan (Shift 2)]

Given below are assertion and reason statements. Select the correct option (memory based jee mains shift-2 29/01/2025)

Assertion: On increasing the pressure, the volume decrease is more in an isothermal process than adiabatic process

Reason: Adiabatic process is given by \({\mathrm{PV}}^{\gamma }\)

Lattice enthalpy and enthalpy of solution of \( \mathrm{NaCl} \) are \( 788 \mathrm{~kJ} \mathrm{~mol}^{-1} \) and \( 4 \mathrm{~kJ} \mathrm{~mol}^{-1} \), respectively. The hydration enthalpy of \( \mathrm{NaCl} \) is

[JEE Main 2020, 5 Sep (Shift 2)]

If the standard molar enthalpy change for combustion of graphite powder is \( -2.48 \times 10^{2} \mathrm{~kJ} \mathrm{~mol}^{-1} \), the amount of heat generated on combustion of \( 1 \mathrm{~g} \) of graphite powder is..... \( \mathrm{kJ} \). (Nearest integer)

For which one of the processes represented by the following equations is the enthalpy (heat) change is likely to be negative

Match List I with List II:

Choose the correct answer from the options given below:

[NEET 2024]

The correct option for free expansion of an ideal gas under adiabatic condition is :

[NEET 2020]

Choose the correct statement from the following:

[JEE Main 2021, 27 Aug (Shift 2)]

If enthalpies of formation of \({C}_{2}{H}_{4}(g),C{O}_{2}(g)and{H}_{2}O(l)at25{C}^{^\circ }and\)1 atm pressure are 52 , -394 , -286 KJ/mol respectively, the change in enthalpy for combustion of \({C}_{2}{H}_{4}\) is equal to

Given
(A) \(2 CO ( g )+ O _2( g ) \rightarrow 2 CO _2( g ) \quad \Delta H _1^\circ =-x \mathrm{~kJ mol} ^{-1}\)
(B) \(C\) (graphite) \(+ O _2( g ) \rightarrow CO _2( g ) \quad \Delta H _2^\circ =-y \mathrm{~kJ mol} ^{-1}\)

The \(\Delta H ^\circ \) for the reaction
\(C\) (graphite) \(+\frac{1}{2} O _2( g ) \rightarrow CO ( g )\) is

[JEE Main 2023, 10 Apr (Shift 1)]

The variation of equilibrium constant with temperature is given below :

The values of \(\Delta \mathrm{H}^{\circ}, \Delta \mathrm{G}^{\circ}\) at \(\mathrm{T}_{1}\) and \(\Delta \mathrm{G}^{\circ}\) at \(\mathrm{T}_{2}\) (in \(\mathrm{kJ} \mathrm{mol}^{-1}\) ) respectively, are close to [Use \(\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\) ]

The true statement amongst the following is :

[JEE Main 2020, 9 Jan (Shift 2)]

Given below are two statements: One is labelled as Assertion (A) and the other is labelled as Reason (R)

Assertion (A): Enthalpy of neutralisation of strong monobasic acid with strong monoacidic base is always \(−57\text{ }{\text{kJ mol}}^{−1}\)

Reason (R): Enthalpy of neutralisation is the amount of heat liberated when one mole of \({\mathrm{H}}^{+}\) ions furnished by acid combine with one mole of ^–OH ions furnished by base to form one mole of water. In the light of the above statements, choose the correct answer from the options given below.

Five moles of an ideal gas at 1 bar and \( 298 \mathrm{~K} \) is expanded into vacuum to double the volume. The work done is

[JEE Main 2020, 4 Sep (Shift 2)]

For the combustion reaction at 298 K

\(2\mathrm{Ag}(\mathrm{s})+1/2{\mathrm{O}}_{2}(\mathrm{g})\to 2{\mathrm{Ag}}_{2}\mathrm{O}(\mathrm{s})\)

Which of the following alternatives is correct?

In thermodymanics , heat and work are :

[JEE Main 2021, 16 Mar (Shift 1)]

The value of \(\log K\) for the reaction \(A \rightleftharpoons B\) at \(\mathrm{298 ~K}\) is ______ (Nearest integer)

Given: \(\Delta H ^0=-54.07 \mathrm{~kJ mol ^{-1}}\)
\(\Delta S ^{\circ}=-10 \mathrm{~JK ^{-1} mol ^{-1}}\)
\((\) Take \(2.303 \times 8.314 \times 298=5705\))

Match the columns and select the correct option (memory based jee mains shift-2 22/01/2025)

Work out the heat change (cal) when 40 g of He gas at \(27^\circ \mathrm{C}\)undergoes isothermal and reversible compression from initial pressure of 1 atm to 10 atm \(\left(\mathrm{R}=2\mathrm{cal}{\mathrm{K}}^{-1}{\mathrm{mol}}^{-1}\right).\)

Given below are two statements:

One is labelled as Assertion A and the other is labelled as Reason R

Assertion (A): The reduction of a metal oxide is easier if the metal formed is in liquid state than solid state.
Reason (R): The value of \(\Delta G ^{\ominus}\) becomes more on negative side as entropy is higher in liquid state than solid state.
In the light of the above statements, choose the most appropriate answer from the options given below

[JEE Main 2022, 28 Jul (Shift 2)]

For water at \(100^{\circ} C\) and 1 bar
\[\Delta_{\text {vap }} H -\Delta_{\text {vap }} U = \square \times 10^2 J mol ^{-1}\]
(Round off to the Nearest integer)
[Use: \(R =8.31 J mol ^{-1} K ^{-1}\) ]
[Assume volume of \(H _2 O (l)\) is much smaller than volume of \(H _2 O ( g )\). Assume \(H _2 O ( g )\) can be treated as an ideal gas]

\(0.3 g\) of ethane undergoes combustion at \(27^{\circ} C\) in a bomb calorimeter. The temperature of calorimeter system (including the water) is found to rise by \(0.5^{\circ} C\). The heat evolved during combustion of ethane at constant pressure is -____\(kJ mol ^{-1}\). (Nearest integer)
[Given: The heat capacity of the calorimeter system is \(20 kJ K ^{-1}, R =8.3 JK ^{-1} mol ^{-1}\).
Assume ideal gas behaviour.
Atomic mass of \(C\) and \(H\) are 12 and \(1 g mol ^{-1}\) respectively]

[JEE Main 2023, 1 Feb (Shift 2)]

\(\mathrm{30.4 ~kJ}\) of heat is required to melt one mole of sodium chloride and the entropy change at the melting point is \(28.4 \mathrm{~JK ^{-1} mol ^{-1}}\) at \(\mathrm{1 ~atm}\). The melting point of sodium chloride is.............................. K (Nearest integer)

[JEE Main 2023, 15 Apr (Shift 1)]

For the reaction, \( 2 \mathrm{NO}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{~g}) \), when \( \Delta S=-176.0 \mathrm{~JK}^{-1} \) and \( \Delta \mathrm{H}=-57.8 \mathrm{~kJ} \mathrm{~mol}^{-1} \), the magnitude of \( \Delta \mathrm{G} \) at \( 298 \mathrm{~K} \) for the reaction is -____ \( \mathrm{kJmol}^{-1} \). (Nearest integer)

The variation of equilibrium constant with temperature is given below :

The values of \(\Delta \mathrm{H}^{\circ}, \Delta \mathrm{G}^{\circ}\) at \(\mathrm{T}_{1}\) and \(\Delta \mathrm{G}^{\circ}\) at \(\mathrm{T}_{2}\) (in \(\mathrm{kJ} \mathrm{mol}^{-1}\) ) respectively, are close to [Use \(\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\) ]

[JEE Main 2020, 6 Sep (Shift 1)]

The total number of intensive properties from the following is------------------------

Volume, Molar heat capacity, Molarity, \({E}_{cell}^{^\circ }\), Gibbs free energy change, Molar mass, Mole

[JEE Main 2023, 11 Apr (Shift 2)]

One mole of an ideal gas at \(\mathrm{350 ~K}\) is in a \(\mathrm{~2.0 ~L}\) vessel of thermally conducting walls, which are in contact with the surroundings. It undergoes isothermal reversible expansion from \(\mathrm{~2.0 ~L}\) to \(\mathrm{~3.0 ~L}\) against a constant pressure of \(\mathrm{4 ~atm}\). The change in entropy of the surroundings \((\Delta S )\) is ______ \(J K ^{-1}\) (Nearest integer)

Given: \(\mathrm{R =8.314 ~J K ^{-1} Mol ^{-1}}\).

[JEE Main 2023, 12 Apr (Shift 1)]

An average person needs about \( 10000 \mathrm{~kJ} \) energy per day. The amount of glucose (molar mass \( =180.0 \mathrm{~g} \mathrm{~mol}^{-1} \) ) needed to meet this energy requirement is ____g. (Use : \( \Delta_{\mathrm{C}} \mathrm{H}( \) glucose \( \left.)=-2700 \mathrm{~kJ} \mathrm{~mol}^{-1}\right) \)