Want this question answered?
This reaction would yield a fatty acid glyceryl monoester, more commonly called a monoglyceride or monoacylglycerol.
In this case the yield is 77,27 %.
A reaction which goes to completion without the product of any by products, in effect a reaction which has a 100% yield. Although that would be impossible
98.2 % 98.2 %
No, a reaction can never have an actual yield of 110. If an actual yield of 110% if obtained, then the product must contain impurities which increase the experimental mass.
This reaction would yield a fatty acid glyceryl monoester, more commonly called a monoglyceride or monoacylglycerol.
The percent yield of a reaction measures the efficiency of a reaction. The relationship of the actual yield to the theoretical yield is used to determine this.
In this case the yield is 77,27 %.
percentage yield
A reaction which goes to completion without the product of any by products, in effect a reaction which has a 100% yield. Although that would be impossible
No, competing side reaction is a reson why the actual yield is more than the theoretical yield.
(Actual yield / Theoretical yield) x 100%
percentage yield
The actual yield of a reaction product is always less than the yield from the chemical equation. This is because of error.
The amount of product that is possible in a reaction.
98.2 % 98.2 %
Theoretical= calculated