Q1. Zeroth Law
Assertion (A): If two systems are separately in thermal equilibrium with a third system, they are in thermal equilibrium with each other.
Reason (R): All systems in thermal equilibrium have the same temperature.
(1) A & R both true and R is correct explanation
(2) A & R both true but R is not correct explanation
(3) A true, R false
(4) A false, R true


Q2. First Law
Assertion (A): Internal energy of an isolated system remains constant.
Reason (R): Energy can neither be created nor destroyed, only converted from one form to another.
(1) A & R both true and R is correct explanation
(2) A & R both true but R is not correct explanation
(3) A true, R false
(4) A false, R true



Q3. Second Law
Assertion (A): Heat cannot spontaneously flow from a colder body to a hotter body.
Reason (R): Total entropy of an isolated system always increases for a spontaneous process.
(1) A & R both true and R is correct explanation
(2) A & R both true but R is not correct explanation
(3) A true, R false
(4) A false, R true


Q4. Third Law
Assertion (A): Entropy of a perfectly crystalline substance is zero at absolute zero temperature.
Reason (R): At absolute zero, only one microstate is possible.
(1) A & R both true and R is correct explanation
(2) A & R both true but R is not correct explanation
(3) A true, R false
(4) A false, R true

Q1.
Assertion (A): For a spontaneous process at constant temperature and pressure, ΔG is negative.
Reason (R): Spontaneous processes occur with decrease in Gibbs free energy.
Options:
(1) A & R true, R correct explanation
(2) A & R true, R not explanation
(3) A true, R false
(4) A false, R true


Q2.
Assertion (A): When ΔG = 0, the system is at equilibrium.
Reason (R): At equilibrium, forward and backward reaction rates are equal


Q3.
Assertion (A): A reaction with ΔH < 0 and ΔS < 0 is spontaneous at all temperatures.
Reason (R): Decrease in enthalpy always favours spontaneity.



Q5. (Numerical concept)
Assertion (A): If ΔH = −40 kJ and ΔS = −100 J K⁻¹, reaction is spontaneous at low temperature.
Reason (R): Negative ΔS disfavors spontaneity at high temperature

Q1
Assertion (A): Solubility of AgCl decreases on addition of NaCl.
Reason (R): Addition of NaCl increases concentration of Cl⁻ ions.


Q2
Assertion (A): Larger the value of Ksp, higher is the solubility of a salt.
Reason (R): Ksp is directly proportional to solubility for all salts


Q3
Assertion (A): Precipitation occurs when ionic product exceeds Ksp.
Reason (R): Solution becomes supersaturated under this condition.


Q4
Assertion (A): Solubility of BaSO₄ increases in presence of dilute HCl.
Reason (R): H⁺ ions react with SO₄²⁻ ions to form HSO₄⁻.


Q5
Assertion (A): Two salts having same Ksp may have different solubilities.
Reason (R): Solubility depends on number of ions produced on dissociation