Question

The balanced equation below shows the burning of methane in air.
CH4(g) + 2O2(g)  CO2(g) + H2O(l)
How many grams of carbon dioxide will be produced when 1 mole of methane burns completely?
Given the atomic masses:
C = 12, H = 1, and O = 16

Answer 1

Question # 80564, answer

The balanced equation below shows the burning of methane in air.

$$\mathrm{CH_4(g)} + 2\mathrm{O_2(g)} \rightarrow \mathrm{CO_2(g)} + \mathrm{H_2O(l)}$$

How many grams of carbon dioxide will be produced when 1 mole of methane burns completely?

Given the atomic masses:

$$C = 12, H = 1, \text{ and } O = 16$$

Answer:

1) Balance the reaction equation:

$$\mathrm{CH_4(g)} + 2\mathrm{O_2(g)} \rightarrow \mathrm{CO_2(g)} + 2\mathrm{H_2O(l)}$$

2) Based on reaction stoichiometry 1 mole of carbon dioxide CO2 will be produced as 1 mole of methane CH4 was burned

3) MW of CO2 = 12 + 2*16 = 44 g/mole

4) Mass of CO2 = MW (CO2) * number of moles CO2 = 44 g/mole * 1 mole = 44 g