Ice melts at a temperature lower than its usual melting point when the pressure is increased. This is because-

1. Ice has less density than water

2. Pressure generates heat

3. The chemical bonds break under pressure

4. Ice is not a true solid

An ionic compound is dissolved simultaneously in heavy water and ordinary water, its solubility is –

1. Larger in heavy water

2. Smaller in heavy water

3. Solubility is same in both waters

4. Smaller in simple water

The oxide that gives hydrogen peroxide $\left({\mathrm{H}}_2{\mathrm{O}}_2\right)$ on the treatment with a dilute acid $\left({\mathrm{H}}_2{\mathrm{SO}}_4\right)$ is –

(A) ${\mathrm{MnO}}_2$                                  

(B) ${\mathrm{PbO}}_2$

(C) ${\mathrm{Na}}_2{\mathrm{O}}_2$                                 

(D) ${\mathrm{TiO}}_2$ 

The oxidising property of ${\mathrm{H}}_2{\mathrm{O}}_2$ is best explained by assuming that two oxygen atoms in its molecule are.

(1) Bonded differently

(2) Bonded similarly

(3) Bonded covalently

(4) Bonded by hydrogen bonds

${\mathrm{H}}_2\mathrm{O}$ has higher boiling point than ${\mathrm{H}}_2\mathrm{S}$ because.

(1) ${\mathrm{H}}_2\mathrm{O}$ is a smaller molecule and hence more closely packed

(2) The bond angle in ${\mathrm{H}}_2\mathrm{O}$ is more than in ${\mathrm{H}}_2\mathrm{S}$ and hence the former molecules are more tightly packed

(3) Of intermolecular hydrogen bonding in liquid ${\mathrm{H}}_2\mathrm{O}$

(4) The latent heat of vaporisation is higher for ${\mathrm{H}}_2\mathrm{O}$ than for ${\mathrm{H}}_2\mathrm{S}$

On partial hydrolysis of one mole of peroxodisulphuric acid produces

1. two moles of sulphuric acid

2. two moles of peroxomonosulphuric acid

3. one mole of sulphuric acid and one mole of peroxomonosulphuric acid

4. one mole of sulphuric acid, one mole of peroxomonosulphuric acid and one mole of hydrogen peroxide.

The maximum possible number of hydrogen bonds a water molecule can form is –

(1) 2                                         

(2) 4

(3) 3                                         

(4) 1

${\mathrm{H}}_2{\mathrm{O}}_2$ acts as antiseptic due to its –

(1) Reducing property                           

(2) Oxidising property

(3) Bleaching property                           

(4) Acidic property

A compound that has both polar and non-polar bonds is  –

1. ${\mathrm{NH}}_4\mathrm{Cl}$                                    

2. $\mathrm{HCN}$

3. ${\mathrm{H}}_2{\mathrm{O}}_2$                                     

4. ${\mathrm{CH}}_4$

In which of the following reactions is ${\mathrm{H}}_2{\mathrm{O}}_2$ acting as an acid.

(A) $2{\mathrm{KMnO}}_4+3{\mathrm{H}}_2{\mathrm{SO}}_4+5{\mathrm{H}}_2{\mathrm{O}}_2\to {\mathrm{K}}_2{\mathrm{SO}}_4+{\mathrm{MnO}}_4+2{\mathrm{MnSO}}_4+8{\mathrm{H}}_2\mathrm{O}+5{\mathrm{O}}_2$

(B) $2{\mathrm{K}}_3\mathrm{Fe}{\left(\mathrm{CN}\right)}_6+2\mathrm{KOH}+{\mathrm{H}}_2{\mathrm{O}}_2\to 2{\mathrm{K}}_4\mathrm{Fe}{\left(\mathrm{CN}\right)}_6+2{\mathrm{H}}_2\mathrm{O}+{\mathrm{O}}_2$

(C) ${\mathrm{O}}_3+{\mathrm{H}}_2{\mathrm{O}}_2\to {\mathrm{H}}_2\mathrm{O}+2{\mathrm{O}}_2$

(D) $\mathrm{Ba} {\left(\mathrm{OH}\right)}_2+{\mathrm{H}}_2{\mathrm{O}}_2\to {\mathrm{BaO}}_2+{\mathrm{H}}_2\mathrm{O}$