Question

draw a labelled diagram showing electrolysis of water and
(1) identify the gases evolved at cathode and anode
(2)write the ratio of the gases evolved and
(3)give a test to identify the gases​

Answer 1

Answer:

Water does not carry a charge well, so an electrolyte is added to the water. Vinegar, a weak acid (acetic acid) may be used. To collect the hydrogen and oxygen gases produced, inverted test tubes are often added, as shown in our diagram below.

Again, take special care to trace the path of the electrons. Unless electrons make a complete circuit, a reaction will not occur.

Electrons are "produced" in the battery at the anode, the site of oxidation.

The electrons leave the electrochemical cell through the external circuit.

These negative electrons create a negative electrode in the electrolytic cell which causes the reduction of water.

Note that the area around this electrode will become basic as OH- ions are produced.

2H2O(l)+2e−⟶H2(g)+2OH−(g)

Meanwhile the the positive electrode water will undergo oxidation:

2H2O(l)⟶O2(g)+4H+(aq)+4e−

Electrons produced during this oxidation process will return to the electrochemical cells.

The ratio will equal to the ratio formed in molecules of water 1:2

Oxygen in 1: hydrogen in 2

You can identify the test by bringing a candle near test tube . Hydrogen produce pop sound when it come in contact with heat so, from which test tube an pop sound produce it will be hydrogen and the other one will be Oxygen

Answer 2

Answer:

open pg 9 of your tb and see by yourself

Explanation:

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