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pogonyaev
3 years ago
9

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 wit

h O 2?
Chemistry
1 answer:
Brilliant_brown [7]3 years ago
3 0

Answer:

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

Mass =  138.63 g

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=\frac{Mass\ taken}{Molar\ mass}=\frac{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\times 44.01 g = 138.63 g

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