200 mL of 0.2 M HCl is mixed with 300 mL of 0.1 M NaOH. The molar heat of neutralization of this reaction is $$-$$57.1 kJ. The increase in temperature in $$^\circ$$C of the system on mixing is x $$\times$$ 10^$$-$$2. The value of x is ___________. (Nearest integer)

[Given : Specific heat of water = 4.18 J g^$$-$$1 K^$$-$$1, Density of water = 1.00 g cm^$$-$$3]

[Assume no volume change on mixing)

For water $$\Delta$$_vap H = 41 kJ mol^$$-$$1 at 373 K and 1 bar pressure. Assuming that water vapour is an ideal gas that occupies a much larger volume than liquid water, the internal energy change during evaporation of water is ___________ kJ mol^$$-$$1

[Use : R = 8.3 J mol^$$-$$1 K^$$-$$1]

The Born-Haber cycle for KCl is evaluated with the following data :

$${\Delta _f}{H^\Theta }$$ for KCl = $$-$$436.7 kJ mol^$$-$$1 ;

$${\Delta _{sub}}{H^\Theta }$$ for K = 89.2 kJ mol^$$-$$1 ;

$${\Delta _{ionization}}{H^\Theta }$$ for K = 419.0 kJ mol^$$-$$1 ;

$${\Delta _{electron\,gain}}{H^\Theta }$$ for Cl_(g) = $$-$$348.6 kJ mol^$$-$$1 ;

$${\Delta _{bond}}{H^\Theta }$$ for Cl₂ = 243.0 kJ mol^$$-$$1

The magnitude of lattice enthalpy of KCl in kJ mol^$$-$$1 is _____________ (Nearest integer)

When 400 mL of 0.2 M H₂SO₄ solution is mixed with 600 mL of 0.1 M NaOH solution, the increase in temperature of the final solution is __________ $$\times$$ 10^$$-$$2 K. (Round off to the nearest integer).

[Use : H⁺ (aq) + OH^$$-$$ (aq) $$\to$$ H₂O : $$\Delta$$_$$\gamma$$H = $$-$$57.1 kJ mol^$$-$$1]

Specific heat of H₂O = 4.18 J K^$$-$$1 g^$$-$$1

density of H₂O = 1.0 g cm^$$-$$3

Assume no change in volume of solution on mixing.