Question

Complete the reaction $Xe{F_4} + {O_2}{F_2} \to A + {O_2}$ identify A.

Answer 1

Firstly in the question we need to get the reaction we have to balance and then get the elements sorted. Then we have to apply the process in which we will balance all the elements except the oxygen and hydrogen. Then firstly we will find the change in oxidation state of carbon and manganese and then multiply the number in order to gain the balanced state. Then we will use water and protons in the end to balance the oxygen and hydrogen.

Complete step by step answer:
When we observe the given reaction firstly we will see that there are 3 elements in the given reaction:
First is xenon and it has $1$ atoms participating in the reaction.
Second is the oxygen and it has $2$ atoms participating in the reaction.
Third is the fluorine and it has $3$ atoms participating in the reaction.
In the reaction when we observe from the left to the right we will see that all the other atoms except the fluorine are balanced. So we can see that there is a difference of the $2F$ atoms on both sides. By this we get that the $2F$ should be balanced.
Now we know that the Xe can have at max $6$ bonds, therefore we can say that it have the capacity of making two more bonds so it will form and make the product $Xe{F_6}$
And the reaction would be : $Xe{F_4} + {O_2}{F_2} \to Xe{F_6} + {O_2}$
So the A would be $Xe{F_6}$ .

Note: This is just the one process we simply get the product straightforward by addition, when this method fails we can use the other ones too. Then we opt for substitution or other kinds of reactions. But this is mostly used and is most common.