How much energy is required to vaporize 98.6 g of ethanol (c2h5oh) at its boiling point, if its δhvap is 40.5 kj/mol? how much energy is required to vaporize 98.6 g of ethanol (c2h5oh) at its boiling point, if its δhvap is 40.5 kj/mol? 52.8 kj 11.5 kj 86.7 kj 39.9 kj 18.9 kj

The amount of energy required will be 86.7 kJ.

Explanation:

Mass of ethanol = 98.6 g

Moles of ethanol =

Enthalpy of vaporization of ethanol =

To vaporize 1 mol of ethanol we need 40.5 kJ of energy.

Then for 2.1434 moles the energy required will be:

The closest answer from the given options is 86.7 kJ.

each  column  of the  table  is called a group. elements in a group share similar properties. groups are  read  from  top  to  bottom. metal. metalloid. nonmetal. solid. liquid. gas. fe. hg. o.  2. 3. 4. 5. 6. 7. 8. 9.  2. beryllium. 9.012. 4.  sodium. 22.990.  11. 3.  magnesium. 24.305.  12.  potassium. 39.098.  19. 4.  calcium. 40.078.  20. i guess  i