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 %

hydrocarbons are organic compounds that contain only hydrogens and carbons. they can be saturated (those which contain only carbon-carbon single bonds) or unsaturated (those which contain carbon-carbon double or triple bonds) in nature. hydrocarbons can undergo several reactions like substitution, elimination etc.  

on substituting one or more hydrogen atoms in hydrocarbon it results in the formation of haloalkane. as the halogen atoms are large compared to the carbon and hydrogen atoms, due to which the molecular weight increases and the bond become polar because of presence electronegative halogen atom and results in the increase in boiling point of the haloalkane.

thus, the correct option is (b) that is the boiling point of the new compound increases on substituting a hydrogen atom with a halogen in a hydrocarbon.