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Natali [406]
3 years ago
9

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

Chemistry
1 answer:
Black_prince [1.1K]3 years ago
8 0

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

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 = \frac{3}{1}\times 2.55=7.65 moles of [tex]CO_2

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

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

Thus 2.55 mol of propane produces = \frac{4}{1}\times 2.55=10.2 moles of [tex]H_2O

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

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

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