[Vsevolod12345]

Well, I tried to solve a problem, where the pressure 1 atm is kept constant, and the water was condensed using the pressure give above.
I want to know the change in enthalpy, heat, work, change in entropy, and change in the internal energy

I immediately set internal energy change to zero, because I assume that the system has no internal energy

I note that
H = U - PV
H = -PV
U=q+W
q=-W
q=H
dH = q
S = q/T for a hypothetical entropy

my problem is what is the difference between "change in entropy"  and change in "enthalpy of vaporization"

Vaporization is the inverse process of condensation
H-condens = - H_evap
I find the enthalpy of vaporization given and I find the
"enthapy of condensation" of water  = 970 kcal/mol
What is the difference between "enthalpy change for condensation" and "standard enthalpy change of condensation"
Can you equate those quantities without making an error
 
I quess, I would like to discuss this matter with fellow chemists, and chemistry students.

[Phlogiston]

Well, I tried to solve a problem, where the pressure 1 atm is kept constant, and the water was condensed using the pressure give above.
I want to know the change in enthalpy, heat, work, change in entropy, and change in the internal energy

I immediately set internal energy change to zero, because I assume that the system has no internal energy

This is not correct.  Every system has internal energy.

I note that
H = U - PV
H = -PV
U=q+W
q=-W
q=H
dH = q
S = q/T for a hypothetical entropy

my problem is what is the difference between "change in entropy"  and change in "enthalpy of vaporization"

Entropy and enthalpy are not the same thing.

Vaporization is the inverse process of condensation
H-condens = - H_evap
I find the enthalpy of vaporization given and I find the
"enthapy of condensation" of water  = 970 kcal/mol

This is not correct, for one thing it's way too large and for another it should be negative.

What is the difference between "enthalpy change for condensation" and "standard enthalpy change of condensation"
Can you equate those quantities without making an error
 
I quess, I would like to discuss this matter with fellow chemists, and chemistry students.

Standard refers to a standard state, typically P = 1 bar or concentrations = 1 mol/L for solutions, whereas a non-standard quantity can be at any pressure or concentration.