Let the oxidation number of P be x. As we already know oxidation number of other atoms so we can calculate that of P too.
Na = +1
H= +1 (+2 for hydrogen molecule)
O = -2
Now calculating oxidation number of P:-
1 +2 + x +(-8) = 0
On solving we get x= +5.
If an excess of is treated with , then_____will be produced wherein the oxidation number of P is +3. The compound is
Whenever a reaction between an oxidising agent and a reducing agent is carried out, a compound of lower oxidation state is formed if the reducing agent is in excess and a compound of higher oxidation state is formed if the oxidising agent is in excess. This can be illustrated as follows:
P4 and F2 are reducing and oxidising agents respectively. If an excess of P4 is treated with F2, then PF3 will be produced, wherein the oxidation number (O.N.) of P is +3.
The reaction is not redox because there is no oxidation or reduction of any element (i.e. no change in oxidation state/number).
Ba in BaCl2 is at a +2 charge because it is in group 2. On the other side of the equation Ba in BaSO4 is still +2. Cl2 on the first side of the equation is -2 (as 2 chlorines) and Cl is -2 on the other side as there are 2 of them.
H on both sides are both +1 (but technically +2 as there are two of them).
SO4 does not change oxidation number and always remains -2.
So, the reaction is not a redox reaction.