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All reactants have impurities and those impurities become the limiting factor for the reaction. This means that the actual yield will be lower because there will not be the total measured amount of reactants. Fewer reactants equals lower output.
Wiki User
∙ 9y ago
Wiki User
∙ 9y agoThe theoretical yield does not take into account impurities in the reactants. When one reactant has an impurity, there is less of it which makes it a limiting reactant, thus reducing the actual yield.
Wiki User
∙ 10y agoThere are several reasons why actual yields typicallly are less than what would be calculated theoretically:
-not all reactions go to completion
-impure reactants produce less product than expected
-competing side reactions may consume some of the reactants
-some of the product may be lost when it is processed for purification
Wiki User
∙ 14y agoTheoretical yield is what would be if 100% of the reaction was complete and no amount of product was lost in any way, actually processes are not as efficient.
This all depends on the accuracy of the one doing the experiment and on the reaction. Some reactions are reversible so less than 100% of the reaction goes to completion; other reactions do not go to completion because they require high amounts of energy or more time etc. Substances in the reaction can be lost during the procedure or be hard to separate from other parts of the experiment. In chemistry there is always an expected amount of error to a degree.
The percent of error can be calculated with this formula:
% error = (|actual yield - theoretical yield| / theoretical yield) x 100%
Wiki User
∙ 9y agoThere are several factors, chief of them is there is no perfect measuring apparatus. Time is also another important factor to take into consideration.
Wiki User
∙ 12y agoactual yield is less than theoretical yield because it is greater than theoretical yield
Wiki User
∙ 12y agoBecause according to calculations the whale mass is quite large compared to a ducks mass
lenpollock
This will due to loss from spillage, gas escape, filter paper holding some product etc.,
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Is actual yield greater or less than the theoretical yield?
The percent yield is the ratio of the actual yield to the theoretical yield. A mole ratio is a conversion factor derived from the coefficient of a balanced chemical equation interpreted in terms of moles.
Why could an actual yield be more than a theoretical yield?
If actual yield is higher than theoretical yield then it means the required products contains impurities.
How do the values of the theoretical and actual yields generally compare?
The actual yield is the amount of products that are actually produced in the reaction. Theoretical yield is the maximum possible amount of products that can be obtained giving the amount of the limiting reactant. The actual yield is often lower than the theoretical yield due to reasons like incomplete reaction, loss of reactants when transferring between containers, impure reactants etc.
Relationship between the concentration of reactants and the total number of collisions?
For any chemical reaction, there is a theoretical yield for the products. The theoretical yield is based on the balanced equation for that reaction. If any of the reactants is present at a lower amount, then your actual yield will be less than the theoretical yield.
How do you obtain percent yield of a reaction?
the amount of product obtained over the amount possible multiplied by 100
Is actual yield greater or less than theoretical yield?
The actual yield is less than the theoretical yield.
Is actual yield greater or less than the theoretical yield?
The percent yield is the ratio of the actual yield to the theoretical yield. A mole ratio is a conversion factor derived from the coefficient of a balanced chemical equation interpreted in terms of moles.
Is competing side reaction a reason why actual yield is less than theoretical yield?
No, competing side reaction is a reson why the actual yield is more than the theoretical yield.
What is the difference between actual yield and theoretical yield?
Theoretical= calculated
Is impure reactants present a reason why actual yield is less than theoretical yield?
yes
Why could an actual yield be more than a theoretical yield?
If actual yield is higher than theoretical yield then it means the required products contains impurities.
Why actual yield is always less than theoratical yield?
Actual yield is always less than theoretical yield because: 1) Much amount of product is lost in experimental techniques i.e. filtration, evaporation etc. 2) Much amount of product is lost in energy i.e. heat energy.
How do the values of the theoretical and actual yields generally compare?
The actual yield is the amount of products that are actually produced in the reaction. Theoretical yield is the maximum possible amount of products that can be obtained giving the amount of the limiting reactant. The actual yield is often lower than the theoretical yield due to reasons like incomplete reaction, loss of reactants when transferring between containers, impure reactants etc.
What is the difference between the predicted and actual yield in a chemical reaction?
The actual yield of a reaction product is always less than the yield from the chemical equation. This is because of error.
Relationship between the concentration of reactants and the total number of collisions?
For any chemical reaction, there is a theoretical yield for the products. The theoretical yield is based on the balanced equation for that reaction. If any of the reactants is present at a lower amount, then your actual yield will be less than the theoretical yield.
How do you obtain percent yield of a reaction?
the amount of product obtained over the amount possible multiplied by 100
Why actual cop of vapour compression refrigeration is less than theoretical cop?
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