Calculte the Percent Yield if 104grams of CH3CO2CH2CH3 is produced by reaction of 111grams of CH3CO2H according to :
CH3CO2H + CH3CH2OH = CH3CO2CH2CH3 + H20
Just follow the steps in this example.
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To calculate the percent yield, you need to know the actual yield and the theoretical yield of the reaction.
1. Determine the theoretical yield:
The theoretical yield is the maximum amount of product that can be obtained from the given reactants. It is based on the stoichiometry of the reaction.
First, write and balance the chemical equation:
CH3CO2H + CH3CH2OH → CH3CO2CH2CH3 + H2O
According to the balanced equation, the molar ratio between CH3CO2H and CH3CO2CH2CH3 is 1:1. This means that 1 mol of CH3CO2H reacts to produce 1 mol of CH3CO2CH2CH3.
Next, calculate the number of moles of CH3CO2H:
Molar mass of CH3CO2H = (12.01 g/mol) + (3 * 1.01 g/mol) + (2 * 16.00 g/mol) = 60.05 g/mol
Number of moles of CH3CO2H = Mass / Molar mass = 111 g / 60.05 g/mol = 1.849 mol
Since the molar ratio is 1:1, the theoretical yield of CH3CO2CH2CH3 is also 1.849 mol.
2. Determine the actual yield:
The actual yield is the amount of product obtained in the real experiment.
In this case, the actual yield is given as 104 grams of CH3CO2CH2CH3.
3. Calculate the percent yield:
Percent Yield = (Actual Yield / Theoretical Yield) x 100
Percent Yield = (104 g / 1.849 mol) x 100 = 56.28%
Therefore, the percent yield of the reaction is 56.28%.