What mass of carbon dioxide is produced from the complete combustion of $8.50*10^-3$ $g$ of methane?

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Answer 1 · 2016-04-11T15:22:38

3.145 X $10^-3$ g

The equation for the combustion of Methane is as follows.

C $H_4$ + $O_2$ ------> C $O_2$ + 2 $H_2$ O

One mole of Methane on burning produces one mole of Carbon Dioxide or using molar masses , I can write,

16 g of Methane produces 44 g of Carbon dioxide
using ratio and proportions , we can get the answer;

mass of C $O_2$ = [ 16g C $H_4$ / 44 g C $O_2$ ] x 8.50 x $10^-3$ of C $H_4$

                          = 0.37 x 8.50 x  #10^-3# g

                          = 3.145 X # 10^-3# g

What mass of carbon dioxide is produced from the complete combustion of 8.50*10^-38.50*10^-3 gg of methane?