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

Apr 11, 2016

3.145 X ${10}^{-} 3$ g

#### Explanation:

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