calculate mass of co2 and water formed on complete combustion of 20 gm of methane and 8gm of methane
Answers
Answer:
Answer:- 66 gram carbon dioxide and 54 gram water.
Solution:- First of all one correction to the question, The atomic mass of H is 1 not 14 since 14 is the atomic mass for nitrogen.
The balanced equation for the combustion of methane is:
CH_4+2O_2\rightarrow CO_2+2H_2OCH
4
+2O
2
→CO
2
+2H
2
O
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:
24gCH_4(\frac{1molCH_4}{16gCH_4})(\frac{1molCO_2}{1molCH_4})(\frac{44gCO_2}{1molCO_2})24gCH
4
(
16gCH
4
1molCH
4
)(
1molCH
4
1molCO
2
)(
1molCO
2
44gCO
2
)
= 66gCO_266gCO
2
(b) calculations for grams of water:
24gCH_4(\frac{1molCH_4}{16gCH_4})(\frac{2molH_2O}{1molCH_4})(\frac{18gH_2O}{1molH_2O})24gCH
4
(
16gCH
4
1molCH
4
)(
1molCH
4
2molH
2
O
)(
1molH
2
O
18gH
2
O
)
= 54gH_2O54gH
2
O
So, 24 grams of methane gives 66 grams of carbon dioxide and 54 grams of water on combustion.