Question

What mass, in grams, of CO2 and H20 N
is formed from 2.55 mol of propane?

Answer 1

Answer: The mass of
`CO_2` and
`H_2O` produced are 336.6 g and 183.6 g respectively.

Step-by-step explanation:

The combustion reaction between propane and oxygen leads to formation of carbon dioxide and water.

Law of Conservation of mass states that the mass will remain constant for a balanced equation. This is carried out when the total number of atoms on reactant side is same as the total number of atoms on the product side. Thus the equation must be balanced.

`C_3H_8+5O_2\rightarrow 3CO_2+4H_2O`

a) 1 mol of propane produces = 3 moles of
`CO_2`

Thus 2.55 mol of propane produces =
`(3)/(1)* 2.55=7.65 moles of [tex]CO_2`

mass of
`CO_2=moles* {\text {molar mass}}=7.65mol* 44g/mol=336.6g`

b) 1 mol of propane produces = 4 moles of
`H_2O`

Thus 2.55 mol of propane produces =
`(4)/(1)* 2.55=10.2 moles of [tex]H_2O`

mass of
`H_2O=moles* {\text {molar mass}}=10.2mol* 18g/mol=183.6g`

The mass of
`CO_2` and
`H_2O` produced are 336.6 g and 183.6 g respectively.