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

Step-by-step explanation:

`C+O_2\rightarrow CO_2`

Moles of C =
`\frac{\text{mass of carbon}}{\text{molar mass of carbon}}=(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}=(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
`(1)/(1)* 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