Assertion : Water in liquid state is more stable than ice at room temperature.

Reason : Water in liquid form has higher entropy than ice.

• If both assertion and reason are true and reason is the correct explanation of the assertion.

• If both assertion and reason are true but reason is not the correct explanation of the assertion.

• If assertion is true, but reason is false.

• Both assertion and reason are false statements.

Assertion : First ionization energy for nitrogen is lower than oxygen.

Reason : Across a period effective nuclear charge decreases.

• If both assertion and reason are true and reason is the correct explanation of assertion.

• If both assertion and reason are true but reason is not the correct explanation of assertion.

• If assertion is true but reason is false.

• If both assertion and reason are false.

The heat of neutralization of a strong base and a strong acid is 57 kJ. The heat released when 0.5 mole of HNO₃ solution is added to 0.20 moles of NaOH solution, is :

• 11.4 kJ

• 34.7 kJ

• 23.5 kJ

• 58.8 kJ

How much energy is released when 6 moles of octane is burnt in air? Given $∆{\mathrm{H}}_{\mathrm{f}}^{°}$ for CO_2(g) , H₂O_(g) and C₈H_18(l)  respectively are - 490, -240 and +160 kJ/mol.

• -6.2 kJ

• -37.4 kJ

• -35.5 kJ

• -20.0 kJ

For the equilibrium ${\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{l}\right)} \rightleftharpoons {\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{g}\right)}$ at 1 atm and 298K.

• standard free energy change is equal to zero ($∆{\mathrm{G}}^{°}$= 0)

• free energy change is less than zero ($∆{\mathrm{G}}^{°}$ < 0)

• standard free energy change is less than zero ($∆{\mathrm{G}}^{°}$< 0)

• standard free energy change is greater than zero ($∆$G° > 0).

Of the following which change will shift the reaction towards the product?

${\mathrm{I}}_{2\left(\mathrm{g}\right)} \rightleftharpoons 2{\mathrm{I}}_{\left(\mathrm{g}\right),} ∆{\mathrm{H}}_{\mathrm{f}}^{°} \left(298\mathrm{K}\right) = +150\mathrm{kJ}$

• Increase in concentration of I

• Decrease in concentration of I₂

• Increase in temperature

• Increase in total pressure

One gram sample of NH₄NO₃ is decomposed in a bomb calorimeter. The temperature of the calorimeter increases by 6.12 K. The heat capacity of the system is 1.23 kJ/g/deg. What is the molar heat of decomposition for NH₄NO₃ ?

• -7.53 kJ/mol

• -398.1 kJ/mol

• -16.1 kJ/mol

• -602 kJ/mol

378.

Which one of the following has $∆$S° greater than zero?

• CaO_(s) + CO_2(g) $\rightleftharpoons$ CaCO_3(s)

• NaCl_(aq) $\rightleftharpoons$NaCl_(s)

• NaNO_3(s) $\rightleftharpoons$ Na⁺_(aq) + NO₃^-_(aq)

• N_2(g) + 3H_2(g) $\rightleftharpoons$ 2NH_3(g)

The potential energy diagram for a reaction R → P is given in the figure. $∆$H ° of the reaction corresponds to the energy

• a

• b

• c

• a + b

Assertion : The increase in internal energy ($∆$E) for the vapourization of one mole of water at 1 atm and 373 K is zero.

Reason : For all isothermal processes, $∆$E = 0.

• If both assertion and reason are true and the reason is the correct explanation of the assertion.

• If both assertion and reason are true and the reason is not the correct explanation of the assertion.

• If assertion is true but reason is false.

• If both assertion and reason are false.