Question

PLEASE HELP ME

If the enthalpy of vaporization of water is 40.7 KJ/mol at normal boiling point, calculate the entropy accompanying the vaporization of 2 moles of H20 at 100 degrees Celcius and 1 atm.

Answer 1

@agent0smith
@Elsa213
@ganeshie8
@inkyvoyd
@Jaynator495
@kropot72
@Preetha
@Rushwr
@sleepyjess

Answer 2

notice the hint here is normal boiling point. this means exactly what it means, the boiling point of water at 1 atm. the normal boiling point of water is 100Celcius at 1 atm. If you notice something, it's a molar quantity which means that this is the amount of heat required to vaporize one mole of water. so all we need to do is multiply this quantity given by the number of moles of water.

interesting though if you do change the external pressure you can affect the boiling point of water.

\[(\frac{ 40.7kJ }{ mol })*(2*moles~H_2O) = ?~kJ\]

Answer 3

is that the entire answer?
@Photon336