Question

Calculate the mass of Co2 and H2O formed on complete combustion of 24 gram of Methane Gas. (atomic masses C=12u , H=1u ,O=16u )​

Answer 1

Answer:-

66 gram carbon dioxide and 54 gram water.

Solution:-

The balanced equation for the combustion of methane is:

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

From balanced equation, 1 mol of methane gives 1 mol of carbon dioxide and 2 moles of water.

Let's convert the given grams of methane to moles and using mol ratio, the moles of each of the products are calculated that could easily be converted to grams on multiplying the moles by their respective molar masses.

Molar mass of methane is 16, molar mass of carbon dioxide is 44 and molar mass of water is 18.

The calculations are as follows:

(a) calculations for grams of carbon dioxide:

$\rm 24gCH_4(\frac{1molCH_4}{16gCH_4})(\frac{1molCO_2}{1molCH_4})(\frac{44gCO_2}{1molCO_2})$

= $\rm66gCO_2$

(b) calculations for grams of water:

$\rm 24gCH_4(\frac{1molCH_4}{16gCH_4})(\frac{2molH_2O}{1molCH_4})(\frac{18gH_2O}{1molH_2O})$

= $\rm 54gH_2O$

So, 24 grams of methane gives 66 grams of carbon dioxide and 54 grams of water on combustion.