Question

C6H12 + 9 O2 –> 6 CO2 + 6 H2O
How many grams of O2 are consumed when C6H12 is burned to yield 5.3 grams of CO2?

Answer 1

5.76 g of $O_2$ are consumed when $C_6H_1_2$ is burned to yield 5.3 grams of $CO_2$.

What is a mole?

A mole is defined as 6.02214076 × $10^{23}$ of some chemical unit, be it atoms, molecules, ions, or others.

Calculating moles of $CO_2$

Number of mole of $CO_2$ = $\frac{\;Given \;mass}{\;Molar \;mass}$

$\frac{\;Given \;mass}{\;Molar \;mass}$ = $\frac{5.3g}{44 g/mol}$ = 0.12 mol

As is clear from the reaction stoichiometry, 9 moles of $O_2$6 moles of $CO_2$.

Calculating the number of moles of $CO_2$

$\frac{0.12 X 9}{6}$ = 0.18 mol

Mass of $O_2$ =5.76 g

Hence, 5.76 g of $O_2$ are consumed when $C_6H_1_2$ yield 5.3 grams of $CO_2$.

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