Question

Given the reaction: 4Na + O2 → 2Na2O How many moles of oxygen are completely consumed in the production of 1.00 mole of Na2O?

Answer 1

Answer : 0.5 moles of oxygen are completely consumed in the production of 1.00 mole of $Na_2O$

Solution : Given,

Moles of $Na_2O$ = 1 mole

The given balanced reaction is,

$4Na+O_2\rightarrow 2Na_2O$

From this balanced reaction, we conclude that

As, 2 moles of $Na_2O$ produces from 1 moles of $O_2$

So, 1 mole of $Na_2O$ produces from $\frac{1}{2}=0.5$ moles of $O_2$

Therefore, 0.5 moles of oxygen are completely consumed in the production of 1.00 mole of $Na_2O$

Answer 2

The answer is 0.5 moles because if 1 moles of o2 is consumed to produce 2 moles of Na2O, then 0.5 moles of o2 will be consumed to produce 1 mole of Na2O.<span />