Calculate the heat required to melt 7.35 g of benzene at its normal melting point. heat of fusion (benzene) = 9.92 kj/mol heat = kj

calculate the heat required to vaporize 7.35 g of benzene at its normal boiling point. heat of vaporization (benzene) = 30.7 kj/mol heat = kj

The heat required to melt 7.35 g of benzene at its normal melting point is 934.8 Joules.

The heat required to vaporize 7.35 g of benzene at its normal melting point is 2,893 Joules.

Explanation:

Mass of benzene = 7.35 g

Moles of benzene =

Heat fusion of benzene,

1) Heat required to melt 7.35 g of benzene at its normal melting point = Q

(1 kJ = 1000 J)

2) Heat vaporization of benzene,

Heat required to vaporize 7.35 g of benzene at its normal melting point = Q

(1 kJ = 1000 J)

specific gravity is the density of a substance divided by the density of water. since (at standard temperature and pressure) water has a density of 1 gram/cm3, and since all of the units cancel, specific gravity is usually very close to the same value as density

so "c" is the answer

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the correct option is c.

isotopes refers to different forms of the same element with the same atomic number but different mass number as a result of difference in their neutron numbers. isotopes have different relative atomic mass but share the same chemical properties.