Question

If 40 gms of methane is burnt ; then how much amount of Co2 is released ?

Answer 1

Your reaction will produce 100 g of carbon dioxide.

Explanation:

Start by writing the balanced chemical equation for the combusiont of methane

#CH_(4(g)) + 2O_(2(g)) -> CO_(2(g)) + 2H_2O_((l))#

Notice that you have a #1:1# mole ratio between methane and carbon dioxide. This means that the number of moles of carbon dioxide produced will be equal to the number of moles of methane that reacted.

To determine how many moles of methane react, use the compound's molar mass

#40cancel("g") * ("1 mole "CH_4)/(16.04cancel("g")) = "2.49 moles"# #CH_4#

The reaction will thus produce

#2.49cancel("moles"CH_4) * ("1 mole "CO_2)/(1cancel("mole"CH_4)) = "2.49 moles"##CO_2#

To get the mass of carbon dioxide that would contain this many moles, use the compound's molar mass

#2.49cancel("moles") * "44.01 g"/(1cancel("mole")) = "109.6 g"# #CO_2#

Rounded to one sig fig, the number of sig figs you gave for the mass of methane, the naswer will be

#m_(CO_2) = color(green)("100 g "CO_2)