Question

Calculate the amount of carbon dioxide formed by the complete combustion of 80g of methane as per the
reaction:
CH4 (g) + 2O2 (g) CO2 (g) + 2 H2O (g)
(Atomic mass of C = 12.01u, H = 1.008u, O = 16u)

Answer 1

We can use the masses as follows also:-
C= 12g
H= 1g
O= 16g
Hope it helps..

Answer 2

Answer : The amount of carbon dioxide formed is, 76.93 g

Solution : Given,

Mass of methane = 80 g

Molar mass of methane = 16.042 g/mole

Molar mass of carbon dioxide = 14.026 g/mole

First we have to calculate the moles of $CH_4$.

$\text{Moles of }CH_4=\frac{\text{Mass of }CH_4}{\text{Molar mass of }CH_4}=\frac{80g}{16.042g/mole}=5.485moles$

Now we have of calculate the moles of carbon dioxide.

The balanced chemical reaction is,

$CH_4(g)+2O_2(g)\rightarrow CO_2(g)+2H_2O(g)$

Form the reaction, we conclude that

1 mole of methane react to give 1 mole of carbon dioxide

5.485 moles of methane react to give 5.485 moles of carbon dioxide

Now we have to calculate the mass of carbon dioxide.

Mass of carbon dioxide = Moles of carbon dioxide × Molar mass of carbon dioxide

Mass of carbon dioxide = 5.485 moles × 14.026 g/mole = 76.93 g

Therefore, the amount of carbon dioxide formed is, 76.93 g