1.

An example of a salt that will not hydrolyse is

• CH₃COONH₄

• CH₃COOK

• NH₄Cl

• KCl

van der Waal's equation for n moles of a gas is

• $\left(\mathrm{P} + \frac{{\mathrm{n}}^2\mathrm{a}}{{\mathrm{V}}^2}\right)(\mathrm{V} - \mathrm{nb}) = \mathrm{RT}$

• $\left(\mathrm{P} + \frac{\mathrm{na}}{{\mathrm{V}}^2}\right)(\mathrm{V}\hspace{0.17em}- \mathrm{nb}) = \mathrm{RT}$

• $\left(\mathrm{P} + \frac{\mathrm{a}}{{\mathrm{V}}^2}\right)(\hspace{0.17em}\mathrm{V}\hspace{0.17em}- \mathrm{b}) = \mathrm{RT}$

• $\left(\mathrm{P}\hspace{0.17em}+ \frac{{\mathrm{n}}^2\mathrm{a}}{{\mathrm{V}}^2}\right) (\mathrm{V}\hspace{0.17em}- \mathrm{b})\hspace{0.17em}= \mathrm{RT}$

Smallest among these species is

• lithium

• lithium ion

• hydrogen

• helium

Covalent compounds have low melting point because

• covalent molecules are held by weak van der Waal's force of attraction

• covalent bond is less exothermic

• covalent bond is weaker than ionic bond

• covalent molecules have definite shape

Which one of the following statements is true?

• $∆$E ia always greater than $∆$H

• $∆$E is always less than $∆$H

• $∆$E may be lesser or greater or equal to $∆$H

• $∆$E is always proportional to $∆$H

For a f-orbital, the values of m are

• -1, 0, +1

• 0, +1, +2, +3

• -2, -1, 0, +1, +2

• -3, -2, -1, 0, +1, +2, +3

Chloride ion and potassium ion are isoelectronic. Then

• potassium ion is relatively bigger

• depends on the other cation and anion

• their size are same

• chloride ion is bigger than potassium ion

Aqueous solutions of hydrogen sulphide and sulphur dioxide when mixed together, yield

• sulphur trioxide and water

• hydrogen and sulphurous acid

• sulphur and water

• hydrogen peroxide and sulphur

The intensive property among these quantities is

• enthalpy

• mass/ volume

• mass

• volume

30g of Mg and 30g of oxygen are reacted and the residual mixture contains

• 45 g of MgO and 15 g of O₂

• 50 g of MgO and 10 g of O₂

• 60 g of MgO only

• 40 g of MgO and 20 g of O₂