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 $O_2$

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

$\text{Moles of }O_2=\frac{14.9g}{32g/mol}=0.466mol$

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 $\frac{8}{13}\times 0.466=0.287$ mole of $CO_2$

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