What did i do wrong in this Chemistry question

What is the theoretical yield of Sodium oxide if 5.00grams of sodium are reacted

I got 10gNA2O and it was wrong, how should I have it setup?

4Na + O2 --> 2Na2O ( Balanced reaction )
Mw(Na) = 22.98grams/mol
n=m/MW
n(Na)=5/22.98=0.217mol
moles of Na2O --> 0.217/2=0.108mole
Mw(Na2O)=61.96g/mol
m=n*MW=0.108*61.96=6.69grams

It is so simple dear.
In balanced chemical equation 2moles of sodium combines with oxygen to give 1mole of sodium oxide.
Now look
Mol.wt of sodium oxide is 62g
At.wt of sodium is 23g
2moles of sodium produces sodium oxide = 62g
i.e 46g of sodium produces sodium oxide = 62g
1g of sodium . . . . . . . . = 62/46 g
5g of sodium . . . . . . . . .= 5(62/46)
= 6.74g

You have five grams of sodium. How many moles is that?

Now, write a balanced equation, and how many moles of product can you get from each mole of starting material? And thus, how many grams does that number of moles equal?

4Na + O2--> 2Na2O
molar ratio of Na2O to Na is 1 : 2
5.00 g Na / 22.99 g/mole = 0.2175 mole Na
moles of Na2O = 0.2175 x (1/2) = 0.1087 mole Na2O
0.1087 mole x 61.98 g/mole = 6.74 g Na2O

by doing your own homework.