Chemistry, 07.01.2021 14:00 evanmc627

In a reaction, 2mol of oxygen reacts with 8g of ethane to produce carbon dioxide and water, calculate the mass of carbon dioxide formed in this reaction. 2C2H6 +7O2 > 4CO2 +6H2O

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Answer from: kasey1292

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 molesH₂O: 6 moles

Being the molar mass of the compounds:

C₂H₆: 30 g/moleO₂: 16 g/mole CO₂: 44 g/moleH₂O: 18 g/mole

By reaction stoichiometry, the following mass amounts of each compound participate in the reaction:

C₂H₆: 2 moles* 30 g/mole= 60 gO₂: 7 moles* 16 g/mole= 112 gCO₂: 4 moles* 44 g/mole= 176 gH₂O: 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?

$mass of C_{2}H_{6} =\frac{2 moles of O_{2}* 60 grams of C_{2}H_{6} }{7 moles of O_{2}}$

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?

$mass of CO_{2} =\frac{8 grams of C_{2}H_{6}* 176 grams of CO_{2} }{60 grams of C_{2}H_{6}}$

mass of CO₂= 23.47 grams

The mass of carbon dioxide formed in the reaction is 23.47 grams.

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