Verified Answer :

Carbon = 12.010
Oxygen = 15.999 x 2
15.999 x 2 = 31.998 + 12.010 = 44.008
\(\frac{37.15 grams * 1 mole CO2}{44.008 grams}\)
Cancel out the grams
\(\frac{37.15 mol CO2}{44.008} = 0.844 mol CO2\)
2 moles of Oxygen atoms in 1 mol CO2 so
\(0.844 * 2 =\)
1.688 moles of Oxygen

Answer : The number of moles of oxygen required are, 0.844 moles

Solution : Given,

Mass of carbon dioxide = 37.1 g

Molar mass of carbon dioxide = 44 g/mole

First we have to calculate the moles of carbon dioxide.

\(\text{Moles of }CO_2=\frac{\text{Mass of }CO_2}{\text{Molar mass of }CO_2}=\frac{37.15g}{44g/mole}=0.844moles\)

Now we have to calculate the moles of oxygen.

The balanced chemical reaction will be,

\(C+O_2\rightarrow CO_2\)

From the balanced reaction we conclude that

As, 1 mole of carbon dioxide produces 1 mole of oxygen

So, 0.844 mole of carbon dioxide produces 0.844 mole of oxygen

Therefore, the number of moles of oxygen required are, 0.844 moles

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