Answer:
[tex]Y=81.5\%[/tex]
Explanation:
Hello.
In this case, for the undergoing chemical reaction:
[tex]5 C(s) + 2 SO_2 (g)\rightarrow CS_2 (g) + 4CO (g)[/tex]
In such a way, since 44.7 g of carbon disulfide (76 g/mol) are actually yielded, we need to compute the theoretical yield via the 42.3 g of carbon (12 g/mol) and the 1:5 mole ratio between them as shown below:
[tex]m_{CS_2}^{theoretical}=42.3 gC*\frac{1molC}{12gC}*\frac{1molCS_2}{5molC}*\frac{76gCS_2}{1molCS_2} \\\\m_{CS_2}^{theoretical}=54.8g[/tex]
Thus, the percent yield, which is computed by dividing the actual yield over the theoretical one, we obtain:
[tex]Y=\frac{44.7g}{54.8g} *100\%\\\\Y=81.5\%[/tex]
Best regards.
Taking into account definition of percent yield, the percent yield for the reaction is 83.43%.
In first place, the balanced reaction is:
5 C + 2 SO₂ → CS₂ + 4 CO
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:
The following rule of three can be applied: if by reaction stoichiometry 60 grams of C form 76 grams of CS₂, 42.3 grams of C form how much mass of CS₂?
[tex]mass of CS_{2} =\frac{42.3 grams of Cx76 grams of CS_{2} }{60 grams of C}[/tex]
mass of CS₂= 53.58 grams
Then, 53.58 grams of CS₂ can be produced from 42.3 grams of C.
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.
In this case, you know:
Replacing in the definition of percent yields:
[tex]percent yield=\frac{44.7 grams}{53.58 grams}x100[/tex]
Solving:
percent yield= 83.43%
Finally, the percent yield for the reaction is 83.43%.
Learn more about
the reaction stoichiometry:
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percent yield:
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