Question

If 16g of
`CH_(4)` reacts with 64g of
`O_(2)` to produce 36g of
`H_(2)O`, how many grams of
`CO_(2)` are produced?

Answer 1

43.56 grams of are produced if 16g of CH4 reacts with 64g of O2.

Step-by-step explanation:

Balance equation for the reaction:

CH4 + 2O2⇒ CO2 +2H2O

Data given : mass of CH4 =16 grams atomic mass = 16.04 grams/mole

mass of water 36 gram atomic mass = 18 grams/moles

mass of CO2=? atomic mass = 44.01 grams/mole

number of moles =
`(mass)/(atomic mass of one mole)` equation 1

number of moles in CH4

n =
`(16)/(16.04)`

= 0.99 moles

Since combustion is done in presence of oxygen hence it is an excess reagent and methane is limiting reagent so production of CO2 depends on it.

From the equation

1 mole of CH4 gave 1 mole of CO2

O.99 moles of CH4 will give x moles of CO2

`(1)/(1)` =
`(x)/(0.99)`

x = 0.99 moles of carbon dioxide

grams of CO2 = number of moles x atomic mass

= 0.99 x 44.01

= 43.56 grams of CO2 is produced.