Question

What mass of carbon dioxide would be produced if 100g of butane (C4H10) are completely oxidized to carbon dioxide and water?

Answer 1

Answer : The mass of carbon dioxide produced will be, 303.424 grams.

Explanation : Given,

Mass of butane = 100 g

Molar mass of butane = 58 g/mole

Molar mass of carbon dioxide = 44 g/mole

The balanced chemical reaction will be,

$2C_4H_{10}+13O_2\rightarrow 8CO_2+10H_2O$

First we have to calculate the moles of $C_4H_{10}$

$\text{Moles of }C_4H_{10}=\frac{\text{Mass of }C_4H_{10}}{\text{Molar mass of }C_4H_{10}}=\frac{100g}{58g/mole}=1.724moles$

Now we have to calculate the moles of $CO_2$

From the balanced reaction, we conclude that

As, 2 moles of butane react to give 8 moles of carbon dioxide

So, 1.724 moles of butane react to give $\frac{8}{2}\times 1.724=6.896$ moles of carbon dioxide

Now we have to calculate the mass of $CO_2$

$\text{Mass of }CO_2=\text{Moles of }CO_2\times \text{Molar mass of }CO_2$

$\text{Mass of }CO_2=(6.896mole)\times (44g/mole)=303.424g$

Therefore, the mass of carbon dioxide produced will be, 303.424 grams.