Question

a student carried out a combustion reaction with methane (ch4) as the limiting reagent. a 12.0g quantity of methane was used, and the student collected 22.0g of carbon dioxide. what was the percent yield

Answer 1

The total percent yield:

After the combustion reaction with methane, the percent yield was 66.7%.  

Combustion of Methane:

• Methane produces a blue flame as it burns in the atmosphere.
• Methane burns in the presence of enough oxygen to produce carbon dioxide (CO₂) and water (H₂O).
• It creates a significant quantity of heat during combustion, making it an excellent fuel source.

The other reactant, air's excess oxygen, is always present, making methane the limiting reactant. As a result, the amount of CH₄ burned will determine how much CO₂ and H₂O are produced.

The following chemical process produces carbon dioxide from methane:

CH₄ + 2O₂ ⇒ CO₂ + 2H₂O

Calculations:

1. Theoretical quantity of carbon dioxide:

All calculations will be based on the amount of methane because the problem specifies that it is the limiting reagent:

12.0g of CH₄ × (1 mol of CH₄/16g CH₄) × (1 mole of CO₂/1 mole of CH₄) × (44g CO₂/1 mole of CO₂)

= 33g of CO₂

2. Percent yield:

= Actual yield/Theoretical yield × 100

= 22.0g/33g × 100

= 66.7%

Learn more about the percent yield here,

brainly.com/question/15535037

#SPJ4