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Answer :
Answer:
For these problems, we need to compare the theoretical yield that we'd get from performing stoichiometry to the actual yield stated in the problem. % yield is the actual yield/theoretical yield x 100%
Cu + 2 AgNO₠→ Cu(NOâ‚)â‚‚ + 2 Ag ==> each mole of copper yields two moles of silver
12.7-g Cu x ( 1 mol Cu /63.5-g Cu) x ( 2 mol Ag / 1 mol Cu) x (108-g Ag / 1 mol Ag) = 43.2-g Ag. This is the theoretical yield. Now, since we got 38.1-g Ag our % yield is:
38.1-g/43.2-g x 100% = 88.2%
For these problems, we need to compare the theoretical yield that we'd get from performing stoichiometry to the actual yield stated in the problem. % yield is the actual yield/theoretical yield x 100%
Cu + 2 AgNO₠→ Cu(NOâ‚)â‚‚ + 2 Ag ==> each mole of copper yields two moles of silver
12.7-g Cu x ( 1 mol Cu /63.5-g Cu) x ( 2 mol Ag / 1 mol Cu) x (108-g Ag / 1 mol Ag) = 43.2-g Ag. This is the theoretical yield. Now, since we got 38.1-g Ag our % yield is:
38.1-g/43.2-g x 100% = 88.2%
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Rewritten by : Barada
Considering the definition of percent yield, the percent yield of silver is 88.36 %.
The balanced reaction is:
Cu + 2 AgNO₃ → Cu(NO₃)₂ + 2 Ag
Theorical yield
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:
- Cu: 1 mole
- AgNO₃: 2 moles
- Cu(NO₃)₂: 1 mole
- Ag: 2 moles
The molar mass of the compounds is:
- Cu: 63.54 g/mole
- AgNO₃: 169.87 g/mole
- Cu(NO₃)₂: 187.54 g/mole
- Ag: 107.87 g/mole
Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:
- Cu: 1 mole× 63.54 g/mole= 63.54 grams
- AgNO₃: 2 moles× 169.87 g/mole= 339.74 grams
- Cu(NO₃)₂: 1 mole× 187.54 g/mole= 187.54 grams
- Ag: 2 moles× 107.87 g/mole= 215.74 grams
Then the following rule of three can be applied: if by reaction stoichiometry 63.54 grams of Cu form 215.74 grams of Ag, 12.7 grams of Cu form how much mass of Ag?
[tex]amount of mass of Ag= \frac{12.7 grams of Cux215.74 grams of Ag}{63.54 grams of Cu}[/tex]
amount of mass of Ag= 43.12grams
Percent yield
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:
- actual yield= 38.1 grams
- theorical yield= 43.12 grams
Replacing in the definition of percent yields:
[tex]percent yield=\frac{38.1 grams}{43.12 grams} x100[/tex]
Solving:
percent yield= 88.36 %
The percent yield of silver is 88.36 %.
Learn more about percent yield:
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