Isopropyl alcohol, C3H8O, is used in rubbing alcohol mixture. Alcohol on the skin cools by evaporation. How much heat(in kJ) is absorbred by the alcohol of 2.25g EVAPORATED? THE HEAT VAPORIZATION OF Isopropyl alcohol is 42.1 kJ/MOL

Compute the number of moles of C3H8O that correspond to 2.25 g. Then multiply that number of moles by 42.1 kJ/mol. That will be the answer, in kJ.

To compute the number of moles of C3H8O (isopropyl alcohol) corresponding to 2.25 g, you need to use the molar mass of isopropyl alcohol.

Molar mass of C3H8O = (3 x molar mass of C) + (8 x molar mass of H) + (1 x molar mass of O)

The molar masses of C, H, and O are:
- Carbon (C): 12.01 g/mol
- Hydrogen (H): 1.01 g/mol
- Oxygen (O): 16.00 g/mol

Substituting these values into the equation for molar mass of C3H8O:

Molar mass of C3H8O = (3 x 12.01 g/mol) + (8 x 1.01 g/mol) + (1 x 16.00 g/mol) = 60.10 g/mol

Now, to calculate the number of moles (n) of isopropyl alcohol corresponding to 2.25 g, you can use the equation:

n = mass / molar mass

n = 2.25 g / 60.10 g/mol ≈ 0.0375 mol

Finally, to calculate the heat absorbed by the alcohol when 2.25 g evaporates, you multiply the number of moles (0.0375 mol) by the heat of vaporization of isopropyl alcohol (42.1 kJ/mol):

Heat absorbed = number of moles x heat of vaporization
Heat absorbed = 0.0375 mol x 42.1 kJ/mol = 1.575 kJ

Therefore, the amount of heat absorbed by the alcohol when 2.25 g evaporates is approximately 1.575 kJ.