Question

When carbon is burned in air, it reacts with oxygen to form carbon dioxide. When 15.6 g of carbon were burned in the presence of 59.1 g of oxygen, 17.5 g of oxygen remained unreacted. What mass of carbon dioxide was produced?

Answer 1

Answer: 5.72 g mass of carbon dioxide was produced

Explanation:

$C+O_2\rightarrow CO_2$

Moles of C =$\frac{\text{mass of carbon}}{\text{molar mass of carbon}}=\frac{15.6 g}{12 g/mol}=1.3 moles$

Mass of $O_2$ reacted = 59.1 g - 17.5 g = 41.6 g

Moles of $O_2\text{ reacted}=\frac{\text{mass of}O_2}{\text{molar mass of}O_2}=\frac{41.6 g}{32 g/mol}=1.3 moles$

According to reaction 1 mole $O_2$ produces 1 mole of $CO_2$ then 1.3 mole of $O_2$ will produce $\frac{1}{1}\times 1.3$ moles of $CO_2$

Mass of $CO_2$:

=Moles of $CO_2$ × molar mass of$CO_2$ = 1.3 ×44 g/mol =

=57.2 grams

5.72 g mass of carbon dioxide was produced