Answer:
The mass of carbon dioxide formed in the reaction is 23.47 grams.
Explanation:
The balanced reaction is:
2 C₂H₆ +7 O₂ ⇒ 4 CO₂ + 6 H₂O
By stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of each compound participate in the reaction:
- C₂H₆: 2 moles
- O₂: 7 moles
- CO₂: 4 moles
- H₂O: 6 moles
Being the molar mass of the compounds:
- C₂H₆: 30 g/mole
- O₂: 16 g/mole
- CO₂: 44 g/mole
- H₂O: 18 g/mole
By reaction stoichiometry, the following mass amounts of each compound participate in the reaction:
- C₂H₆: 2 moles* 30 g/mole= 60 g
- O₂: 7 moles* 16 g/mole= 112 g
- CO₂: 4 moles* 44 g/mole= 176 g
- H₂O: 6 moles* 18 g/mole= 108 g
The limiting reagent is one that is consumed first in its entirety, determining the amount of product in the reaction. When the limiting reagent is finished, the chemical reaction will stop.
To determine the limiting reagent, you can use a simple rule of three as follows: if by stoichiometry of the reaction 7 moles of O₂ react with 60 g of C₂H₆, 2 moles of O₂ will react with how much mass of C₂H₆?
[tex]mass of C_{2}H_{6} =\frac{2 moles of O_{2}* 60 grams of C_{2}H_{6} }{7 moles of O_{2}}[/tex]
mass of C₂H₆= 17.14 grams
But 17.14 grams of C₂H₆ are not available, 8 grams are available. Since you have less moles than you need to react with 2 moles of O₂, ethane C₂H₆ will be the limiting reagent.
Then, it is possible to determine the amount of mass of CO₂ produced by another rule of three: if by stoichiometry 60 grams of C₂H₆ produce 176 grams of CO₂, how many mass of CO₂ will be formed if 8 grams of C₂H₆ react?
[tex]mass of CO_{2} =\frac{8 grams of C_{2}H_{6}* 176 grams of CO_{2} }{60 grams of C_{2}H_{6}}[/tex]
mass of CO₂= 23.47 grams
The mass of carbon dioxide formed in the reaction is 23.47 grams.
