Taking into account definition of percent yield, the percent yield for the reaction is 57.08%.
In first place, the balanced reaction is:
CH₄ + Cl₂ → CH₃Cl + HCl
By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:
The molar mass of the compounds is:
Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:
Mass of CH₃Cl formed
The following rule of three can be applied: if by reaction stoichiometry 16 grams of CH₄ form 50.45 grams of CH₃Cl, 25 grams of CH₄ form how much mass of CH₃Cl?
[tex]mass of CH_{3} Cl=\frac{25 grams of CH_{4}x 50.45grams of CH₃Cl }{16 grams of CH_{4}}[/tex]
mass of CH₃Cl= 78.83 grams
Then, 78.83 grams of CH₃Cl can be produced from 25 grams of CH₄.
The percent yield is the ratio of the actual return to the theoretical return expressed as a percentage.
The percent yield is calculated as the experimental yield divided by the theoretical yield multiplied by 100%:
[tex]percent yield=\frac{actual yield}{theorical yield}x100[/tex]
where the theoretical yield is the amount of product acquired through the complete conversion of all reagents in the final product, that is, it is the maximum amount of product that could be formed from the given amounts of reagents.
Percent yield for the reaction in this case
In this case, you know:
Replacing in the definition of percent yields:
[tex]percent yield=\frac{45 grams}{78.83 grams}x100[/tex]
Solving:
percent yield= 57.08%
Finally, the percent yield for the reaction is 57.08%.
Learn more about
the reaction stoichiometry:
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percent yield:
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