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Which of the following is not a reason why actual yield is less than theoretical yield?

A. presence of impure reactants

B. conservation of mass

C. competing side reactions

D. loss of product during purification

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Your answer is B, conservation of mass


Recall that percent yield is given by: %Yeild = actual yeild/theoretical yeild x100

During experiments, there are errors made:

• uncertainty in measurements

• losses of reactants and products

• impurity in reactants

• losses during separation (e.g. filtration or purification)

• Some side reactions might also happen.



Among the given options, only conservation of mass does not contribute to a lower actual yield compared to the theoretical yield.

The option that isn't a reason why the actual yield is less than theoretical yield is B. conservation of mass.

It should be noted that the formula for the percent yield is given as:

= Actual yield / Theoretical Yield × 100

  • The actual yield is experimentally determined, and it's the quantity of a product that is gotten from a chemical reaction.

  • The theoretical yield is the amount of product that can be obtained from a reaction when the reactants are changed to products.

Actual yield can be less than theoretical yield due to the presence of impure reactants ,competing side reactions, and loss of product during purification.

In conclusion, the correct option is B.

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