JEE Main 2025 (Online) 22nd January Morning Shift | Thermodynamics Question 17 | Chemistry

JEE Main 2025 (Online) 22nd January Morning Shift

MCQ (Single Correct Answer)

-1

A liquid when kept inside a thermally insulated closed vessel at $25^{\circ} \mathrm{C}$ was mechanically stirred from outside. What will be the correct option for the following thermodynamic parameters ?

$\Delta \mathrm{U}=0, \mathrm{q}<0, \mathrm{w}>0$

$\Delta \mathrm{U}>0, \mathrm{q}=0, \mathrm{w}>0$

$\Delta \mathrm{U}=0, \mathrm{q}=0, \mathrm{w}=0$

$\Delta \mathrm{U}<0, \mathrm{q}=0, \mathrm{w}>0$

JEE Main 2024 (Online) 5th April Morning Shift

MCQ (Single Correct Answer)

-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 $$-57 \mathrm{~kJ} \mathrm{~mol}^{-1}$$

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 $${ }^{-} \mathrm{OH}$$ 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.

(A) is true but (R) is false

Both (A) and (R) are true and (R) is the correct explanation of (A)

Both (A) and (R) are true but (R) is not the correct explanation of (A)

(A) is false but (R) is true

JEE Main 2024 (Online) 1st February Morning Shift

MCQ (Single Correct Answer)

-1

Choose the correct option for free expansion of an ideal gas under adiabatic condition from the following :

$\mathrm{q}=0, \Delta \mathrm{T}=0, \mathrm{w}=0$

$\mathrm{q}=0, \Delta \mathrm{T} \neq 0, \mathrm{w}=0$

$\mathrm{q} \neq 0, \Delta \mathrm{T}=0, \mathrm{w}=0$

$\mathrm{q}=0, \Delta \mathrm{T}<0, \mathrm{w} \neq 0$

JEE Main 2024 (Online) 29th January Morning Shift

MCQ (Single Correct Answer)

-1

Which of the following is not correct?

$$\Delta \mathrm{G}$$ is positive for a spontaneous reaction

$$\Delta \mathrm{G}$$ is positive for a non-spontaneous reaction

$$\Delta \mathrm{G}$$ is zero for a reversible reaction

$$\Delta \mathrm{G}$$ is negative for a spontaneous reaction

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