H2O2 behave as a bleaching agent because :

1.	It acts as a strong oxidizing agent both in acidic and basic media.
2.	It acts as a strong reducing agent both in acidic and basic media.
3.	It acts as a strong oxidizing agent only in neutral media.
4.	It acts as a strong reducing agent only in neutral media.

A colourless liquid 'A' contains H and O elements only. It decomposes slowly on exposure to light. It is stabilised by mixing urea to store in the presence of light. The chemical equation for its decomposition reaction in light is-

1.  ${\mathrm{H}}_2{\mathrm{O}}_2\underset{\mathrm{sunlight}}{\overset{\mathrm{hv}}{\to }}{\mathrm{H}}_2\mathrm{O}+{\mathrm{O}}_3$

2. $2{\mathrm{H}}_2{\mathrm{O}}_2\underset{\mathrm{sunlight}}{\overset{\mathrm{hv}}{\to }}2{\mathrm{H}}_2\mathrm{O}+{\mathrm{O}}_2$

3. $2{\mathrm{H}}_2{\mathrm{O}}_2\underset{\mathrm{sunlight}}{\overset{\mathrm{hv}}{\to }}2{\mathrm{H}}_2\mathrm{O}+{\mathrm{H}}_2$

4.  $2{\mathrm{H}}_2{\mathrm{O}}_2\underset{\mathrm{sunlight}}{\overset{\mathrm{hv}}{\to }}\mathrm{NO}<mspace\; width="1em"></mspace>\mathrm{Rxn}$

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

Hydrolysis and hydration are:

1. Different chemical process

2. Same chemical process

3. Can be used simultaneously

4. All of these