Suppose the theoretical yield in a reaction is 10.5 g and the percent yield is 75.5%. what is the actual yield of product obtained?

7.875 gram is the actual yield of product obtained.

Explanation:

We are given:

Theoretical yield of reaction =  10.5 g

Experimental or actual yield = x

Percentage yield of the product = 75.5 %

The formula we used to determine percentage yield is:

x = 7.875 g

7.875 gram is the actual yield of product obtained.

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.