When 8.70 kj of thermal energy is added to 2.50 mol of liquid methanol, it vaporizes. determine the heat of vaporization in kj/mol of methanol.

The heat of vaporization in kJ/mol of methanol

= 3.48 kJ/mole

Explanation:

Here,the heat of vaporization in kJ/mol is asked to calculate.This means it is asked to calculate heat required for 1 mole of methanol. Since the substance vaporizes , so this is called heat of vaporization.

Divide the thermal energy with the number of moles .

This is simple mathematics :

If 2.50 mol of liquid require = 8.70 kJ of energy

Then, 1 mole will need =

= 3.48 kJ/mole

Follow the units :

The heat of vaporization in kJ/mol of methanol is asked.

Unit = kJ /Mole

the answer is   c.) 1575 j.

explanation:

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: