Question

If 32.3 grams of CH4 is burned in excess oxygen, how many grams of carbon dioxide is produced?

Answer 1

Let's start by writing the balanced reaction equation:

CH₄ +2O₂ $\rightarrow$ CO₂ + 2H₂O.

As one can see from the equation, one mole of methane (CH₄) results in one mole of carbon dioxide (CO₂): $n(\text{CH}_4) = n(\text{CO}_2)$ .

The amount of substance of CH₄ is its mass divided by its molar mass (16.04 g/mol):

$n(\text{CH}_4) = \frac{32.3 \text{ g}}{16.04 \text{ g/mol}} = 2.01 \text{ mol}$

The mass of carbon dioxide CO₂ produced is:

$m(\text{CO}_2) = n(\text{CO}_2)\cdot M(\text{CO}_2) = 2.01(\text{mol})\cdot44.01 (\text{g/mol})$

$m(\text{CO}_2) = 88.6 (\text{g})$

Answer: If 32.3 g of CH₄ is burned in excess oxygen, 88.6 g of carbon dioxide is produced.