Question

How many grams of CO2 are produced from 125 g of O2 and excess CH4 in the equation CH4+2O2→CO2+2H2O?

Answer 1

Answer:

85.8 grams of carbon-dioxide is produced.

Explanation:

Since methane is in excess then calculation ill be done with respect to oxygen gas .

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

Moles of oxygen gas = $\frac{125 g]{32 g/mol}=3.90 mol$

According to reaction, 2 mol of oxygen produces 1 mol of carbon-dioxide.

Then 3.90 mol of oxygen will produce :$\frac{1}{2}\times 3.90 =1.95 mol$ of carbon-dioxide.

Mass of carbon-dioxide produced = 44 g/mol × 1.95 mol =85.8 g

85.8 grams of carbon-dioxide is produced.

Answer 2

Answer:

Explanation:

since CH₄ is given in excess, the calculation are to carried on the basis of mass of oxygen.

The given reaction is

CH4+2O2→CO2+2H2O

From the reaction, we can see that

1 mole of CO₂ is produced from 2 moles of oxygen

44 g or CO₂ is produced from 64 g of oxygen

or

64 g of oxygen gives 44 g of CO₂

125 g of oxygen gives (44/64) x 125 g of CO₂

                                   = 85.9375