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

Verified Answer :

sdmatera

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.

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 \(Na_2O\)

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