Chemistry

Two methods are used to balance chemical equations for redox processes. One of these methods is based on the change in the oxidation number of reducing agent and the oxidising agent (i.e. oxidation number method) and the other method is based on splitting the redox reaction into two half reactions — one involving oxidation and the other involving reduction (half reaction method). Both these methods are in use and the choice of their use rests with the individual using them.

(a) Combination reactions (b) Decomposition reactions (c) displacement reactions (d) Disproportionation reactions.

Electrochemical series is the series of elements in which elements are arranged in decreasing order of their reduction potential.
Reducing power goes on increasing whereas oxidising power goes on decreasing down the series.

Electrochemical cell is a device in which the redox reaction is carried indirectly and the decrease in free energy appears as electrical energy.

At cathode there is gain of electrons.
At anode there is loss of electrons.
In electrochemical cell anode is written on L.H.S while cathode is written on R.H.S.

(b) Oxidation involves gain of one or more electrons by a species during a reaction.

(d) None of the above

(c) In ClO₄^–, chlorine is in maximum oxidation state of +7. So, it does not show the disproportionation reaction.

5.41. Ideal Gas: A gas that follows Boyle's law, Charles' law and Avogadro law strictly, is called an ideal gas. It is assumed that intermolecular forces are not present between the molecules of an ideal gas.

Real Gases: Gases which deviate from ideal gas behaviour are known as real gases. NH₃ is expected to show more deviation. Since NH₃ is polar in nature and it can be liquified easily.