D2O cannot be used for drinking purposes, because - 

1.  it increases the rate of catabolic reactions 

2. it slows the rate of anabolic and catabolic reactions

3. it slows the rate of anabolic reactions.

4. it increases the rate of a reaction.

Saline hydrides can remove traces of water from organic compounds because :

H2O2 behave as a bleaching agent because :

The catalyst used to increase the production of H₂ , by ‘coal gasification' process is -

1. Copper 

2. FeCr₂O₄ (iron chromate) 

3. Pd/C 

4. None of the above.

Hydrogen is placed separately in the periodic table because : 

1. It resembles alkali metals.

2. It shows the same reactions as halogens.

3. Both (1) and (2)

4. None of the above.

NH₃ is an example of :

1. Electron rich hydride

2. Electron-precise hydride

3. Electron deficient hydride

4. None of the above

Incorrect statement regarding structure of H₂O and H₂O₂ is:

1. In gaseous phase, water molecule has a bent form.

2. Bond angle of water is $109.0°$

3. Hydrogen peroxide has a non-planar structure.

4. The dihedral angle of H₂O₂ in gas phase is 111.5° 

The reaction that is not an example of a hydrolysis reaction is-

1. $\mathrm{PbS}\left(\mathrm{s}\right)<mspace\; width="1em"></mspace>+{\mathrm{H}}_2{\mathrm{O}}_2\left(\mathrm{aq}\right)<mspace\; width="1em"></mspace>\to {\mathrm{PbSO}}_4\left(\mathrm{s}\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

2. $\mathrm{CaO}\left(\mathrm{s}\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>\to <mspace\; width="1em"></mspace>\mathrm{Ca}{\left(\mathrm{OH}\right)}_2<mspace\; width="1em"></mspace>\left(\mathrm{aq}\right)$

3. ${\mathrm{AlCl}}_3\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>3{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)<mspace\; width="1em"></mspace>\to {\mathrm{Al}}_2{\mathrm{O}}_3\left(\mathrm{s}\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>6\mathrm{HCl}\left(\mathrm{aq}\right)$

4. ${\mathrm{Ca}}_3{\mathrm{N}}_2\left(\mathrm{s}\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>6{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)<mspace\; width="1em"></mspace>\to 3\mathrm{Ca}{\left(\mathrm{OH}\right)}_2\left(\mathrm{aq}\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>2{\mathrm{NH}}_3\left(\mathrm{g}\right)$

The following reaction is an example of :

\(2 \mathrm{MnO}_4^{-}+6 \mathrm{H}^{+}+5 \mathrm{H}_2 \mathrm{O}_2 \rightarrow 2 \mathrm{Mn}^{2+}+8 \mathrm{H}_2 \mathrm{O}+5 \mathrm{O}_2\)

1. Hydrolysis reaction

2. Redox reaction

3. Disproportionation reaction

4. None of the above

The reaction in which hydrogen peroxide acts as a reducing agent is/are-

1. ${\mathrm{Mn}}^{+2}<mspace\; width="1em"></mspace>\hspace{0.17em}+{\mathrm{H}}_2{\mathrm{O}}_2<mspace\; width="1em"></mspace>\to <mspace\; width="1em"></mspace>{\mathrm{Mn}}^{+4}<mspace\; width="1em"></mspace>+\hspace{0.17em}2{\mathrm{OH}}^{-}$

2. $\mathrm{PbS}<mspace\; width="1em"></mspace>+4{\mathrm{H}}_2{\mathrm{O}}_2<mspace\; width="1em"></mspace>\to <mspace\; width="1em"></mspace>{\mathrm{PbSO}}_4<mspace\; width="1em"></mspace>+\hspace{0.17em}4{\mathrm{H}}_2\mathrm{O}$

3. ${\mathrm{I}}_2<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>{\mathrm{H}}_2{\mathrm{O}}_2<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>2{\mathrm{OH}}^{-}<mspace\; width="1em"></mspace>\to <mspace\; width="1em"></mspace>2{\mathrm{I}}^{-}<mspace\; width="1em"></mspace>+\hspace{0.17em}2{\mathrm{H}}_2\mathrm{O}\hspace{0.17em}+<mspace\; width="1em"></mspace>{\mathrm{O}}_2$

4. All of the above