Want this question answered?
No, competing side reaction is a reson why the actual yield is more than the theoretical yield.
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.
Percent Yield
in the haber process its yield is increased by increasing presure
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.
No, competing side reaction is a reson why the actual yield is more than the theoretical yield.
If you raise the temperature, the endothermic reaction will increase to use up the extra heat, therefore producing less percentage yield of ethanol and more of ethene and steam.
You get an increased yield of H2CO3, as the equilibrium shifts to the side with fewer moles.
(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
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.