contestada

Gaseous methane (CH4) reacts with gaseous oxygen gas (O2) to produce gaseous carbon dioxide (CO2) and gaseous water (H2O). If 28.2 g of carbon dioxide is produced from the reaction of 15.1 g of methane and 81.2 g of oxygen gas, Calculate the percent yield of carbon dioxide. Be sure your answer has the correct number of significant digits in it.

Respuesta :

jufsanabriasa

Answer:

68.1% is percent yield of the reaction

Explanation:

The reaction of methane with oxygen is:

CH₄ + 2O₂ → CO₂ + 2H₂O

Where 2 moles of oxygen react per mole of CHâ‚„

Percent yield is:

Actual yield (28.2g COâ‚‚) / Theoretical yield * 100

To solve this question we need to find theoretical yield finding limiting reactant :

Moles CHâ‚„:

15.1g CHâ‚„ * (1mol / 16.04g) = 0.9414 moles

Moles Oâ‚‚:

81.2g * (1mol / 32g) = 2.54 moles

For a complete reaction of 0.9414 moles of CHâ‚„ are needed:

0.9414 moles CHâ‚„ * (2 mol Oâ‚‚ / 1mol CHâ‚„) = 1.88 moles of Oâ‚‚. As there are 2.54 moles, Oâ‚‚ is in excess and CHâ‚„ is limiting reactant

In theoretical yield, the moles of methane added = Moles of COâ‚‚ produced. That is 0.9414 moles COâ‚‚. In grams = Theoretical yield:

0.9414 moles COâ‚‚ * (44.01g / mol) = 41.43g COâ‚‚

Percent yield: 28.2g COâ‚‚ / 41.43g COâ‚‚ * 100=

68.1% is percent yield of the reaction

Otras preguntas