A student uses the periodic table to construct a model that uses a simple diagonal arrow to depict decreasing electronegativity.
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Taking into account definition of percent yield, the percent yield for the reaction is 57.08%.
<h3>Reaction stoichiometry</h3>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:
- CH₄: 1 mole
- Cl₂: 1 mole
- CH₃Cl: 1 mole
- HCl: 1 mole
The molar mass of the compounds is:
- CH₄: 16 g/mole
- Cl₂: 70.9 g/mole
- CH₃Cl: 50.45 g/mole
- HCl: 36.45 g/mole
Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:
- CH₄: 1 mole ×16 g/mole= 16 grams
- Cl₂: 1 mole ×70.9 g/mole= 70.9 grams
- CH₃Cl: 1 mole ×50.45 g/mole= 50.45 grams
- HCl: 1 mole ×36.45 g/mole= 36.45 grams
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?
<u><em>mass of CH₃Cl= 78.83 grams</em></u>
Then, 78.83 grams of CH₃Cl can be produced from 25 grams of CH₄.
<h3>Percent yield</h3>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%:
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:
- actual yield= 45 grams
- theorical yield= 78.83 grams
Replacing in the definition of percent yields:
Solving:
<u><em>percent yield= 57.08%</em></u>
Finally, the percent yield for the reaction is 57.08%.
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the reaction stoichiometry:
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