SiO2+6HF-----> H2SiF6+2H2O actual yield is 52.8 what is percent yield
Here is a worked example of a stoichiometry problem to find the theoretical yield.
% yield = (actual yield/theoretical yield)*100 = ?
To calculate the percent yield, you need to compare the actual yield to the theoretical yield. The theoretical yield is the maximum amount of product that could be obtained under ideal conditions assuming the reaction goes to completion.
To determine the theoretical yield, you need to use the balanced chemical equation and the stoichiometry of the reaction. The balanced chemical equation for the reaction is:
SiO2 + 6 HF → H2SiF6 + 2 H2O
In this equation, the stoichiometric ratio between SiO2 and H2SiF6 is 1:1. Therefore, the theoretical yield of H2SiF6 can be calculated by considering the amount of SiO2 reacted.
Let's assume that you have the mass of SiO2 used in the reaction. Multiply the mass of SiO2 by its molar mass to convert it to moles. Then, use the stoichiometric ratio to determine the number of moles of H2SiF6 produced. Finally, multiply the number of moles of H2SiF6 by its molar mass to convert it back to grams. This calculated value will give you the theoretical yield.
Once you have the theoretical yield and the actual yield, you can calculate the percent yield using the following formula:
Percent Yield = (Actual Yield / Theoretical Yield) × 100
Substituting the values into the formula:
Percent Yield = (52.8 / Theoretical Yield) × 100
Now, you can substitute the actual yield (52.8) into the formula and solve for the theoretical yield.
Note: The theoretical yield is not provided in the question, which means you would need additional information or prior knowledge to calculate it.