For the following reaction, 4.07 grams of aluminum oxide are mixed with excess sulfuric acid. the reaction yields 10.4 grams of aluminum sulfate. aluminum oxide (s) + sulfuric acid (aq) aluminum sulfate (aq) + water (l) what is the theoretical yield of aluminum sulfate? grams what is the percent yield for this reaction? %

Theoretical yield = 13.7 g

% yield =76 %

Explanation:

For

Mass of  = 4.07 g

Molar mass of  = 101.96 g/mol

The formula for the calculation of moles is shown below:

Thus,

According to the reaction:

1 mole of  on reaction produces 1 mole of

So,  

0.0399 mole of  on reaction produces 0.0399 mole of

Moles of  obtained = 0.0399 mole

Molar mass of = 342.2 g/mol

The formula for the calculation of moles is shown below:

Thus,

Theoretical yield = 13.7 g

The expression for the calculation of the percentage yield for a chemical reaction is shown below as:-

Given , Values from the question:-

Theoretical yield = 13.7 g

Experimental yield = 10.4 g

Applying the values in the above expression as:-

% yield =76 %

the correct answer is:

a. formation of precipitation

the ratio of the conjugate base to the acid required to attain the desired ph.