Question

Given the balanced equation 2C4H10 + 13O2 → 8CO2 + 10H2O, how many moles of CO2 are produced when 14.9g of O2 are used?

Answer 1

Answer: The number of moles of
`CO_2` produced are, 0.287 moles.

Explanation : Given,

Mass of
`O_2` = 14.9 g

Molar mass of
`O_2` = 32 g/mol

First we have to calculate the moles of
`O_2`

`\text{Moles of }O_2=\frac{\text{Given mass }O_2}{\text{Molar mass }O_2}`

`\text{Moles of }O_2=(14.9g)/(32g/mol)=0.466mol`

Now we have to calculate the moles of
`CO_2`

The balanced chemical equation is:

`2C_4H_(10)+13O_2\rightarrow 10H_2O+8CO_2`

From the reaction, we conclude that

As, 13 mole of
`O_2` react to give 8 moles of
`CO_2`

So, 0.466 mole of
`O_2` react to give
`(8)/(13)* 0.466=0.287` mole of
`CO_2`

Therefore, the number of moles of
`CO_2` produced are, 0.287 moles.