Question

Which conversion factor do you use first to calculate the number of grams of CO 2 produced by the reaction of 50.6 g of CH 4 with O 2?

Answer 1

Thus, first conversion of mass of methane into moles by dividing it with 16.04 g/mol

Mass = 138.63 g

Step-by-step explanation:

The balanced chemical reaction is shown below:-

`CH_4+2O_2\rightarrow CO_2+2H_2O`

Firstly the moles of methane gas reacted must be calculate as:-

Given, mass of methane = 50.6 g

Molar mass of methane gas = 16.04 g/mol

The formula for the calculation of moles is:-

`Moles=(Mass\ taken)/(Molar\ mass)=(50.6)/(16.04)\ mol=3.15\ mol`

Thus, from the reaction stoichiometry,

1 mole of methane produces 1 mole of carbon dioxide

Also,

3.15 mole of methane produces 3.15 mole of carbon dioxide

Moles of
`CO_2` = 3.15 mole

Molar mass of
`CO_2` = 44.01 g/mol

Mass = Moles*Molar mass =
`3.15* 44.01` g = 138.63 g