Question

how do we prepare oxygen gas in lab by an experiment​

Answer 1

Answer:

To Make Oxygen in Lab

hydrogen peroxide is poured into a conical flask containing some manganese(IV) oxide. The gas produced is collected in an upside-down gas jar filled with water. As the oxygen collects in the top of the gas jar, it pushes the water out.

Explanation:

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Answer 2

Answer:

Oxygen is the most abundant element on earth. It is found almost in everything in nature and also in free state.

Laboratory Preparation of Oxygen

Oxygen can be prepared in a number of ways in the laboratory. These include:

(a). Heating a mixture of potassium trioxochlorate(V), KClO3 and maganese(IV) oxide, MnO2.

The MnO2 acts as a catalyst. The reaction is actually the decomposition of KClO3.

2KClO3(s) → 2KCl(s) + 3O2(g)

(b). The decomposition of hydrogen peroxide, H2O2 using manganese(IV) oxide - this does not require heating.

Hydrogen peroxide is added drop wisely unto MnO2.

2H2O2(aq) → 2H2O(l) + O2(g)

Or by the drop wise addition of hydrogen peroxide on acidified KMnO4

5H2O2(aq) + 2KMnO4(aq) + 3H2SO4(aq) → K2SO4(aq) + 2MnSO4(aq) + 8H2O(l) + 5O2(g)

(c). The reaction between water and sodium peroxide.

Hydrogen peroxide is formed, and it immediately decomposes by the catalytic effect of the OH- ions in solution.

Na2O2(s) + 2H2O → H2O2 + 2Na+ + 2OH-

Then, 2H2O2 → 2H2O + O2

(d). Application of heat on trioxonitrate(V) salts of metals.

Trioxonitrate(V) salts of metals, e.g, sodium trioxonitrate(V), NaNO3 give off a part of their oxygen upon being heated. NaNO3 loses one third of its oxygen.

2NaNO3(s) → 2NaNO2(s) + O2(g)

(e). Application of heat on certain oxides of the least active metals, e.g., mercury oxide, HgO and silver oxide, Ag2O. These oxides undergo complete dissociation when heated.

2HgO(s) → 2Hg(s) + O2(g)

2Ag2O(s) → 4Ag(s) + O2(g)

(f). Application of heat on oxides of certain metals with more than one oxidation state, e.g., lead(IV) oxide, PbO2 and mangan- ese(IV) oxide, MnO2.

These oxides give off only a part of their oxygen when they are heated. Such reactions usually require very high temperatures.

2PbO2(s) → 2PbO(s) + O2(g)

3MnO2(s) → Mn3O4(s) + O2(g)

(g). The electrolysis of water.

Oxygen is produced at the anode - see the electrolysis of water for details.