What is the change in the entropy of 2.0 kg of H2O molecules when transform at a constant pressure of 1 atm from water at 100˚C to steam at the same temperature?
Answers
First of all, it increases (as gas molecules are more disordered so have higher entropy but be mindful as steam isn't gas, just closer and with higher energy ) so your answer will be positive.
Step-by-step explanation:
The nth term formula goes by :if a system has x times different environments and y times particles, the entropy is y^x that's for a small number of particles. You can't use that here.
Okay, sorry, listen here. You're going to need two formulas :
a) the formula for gibbs free energy (Gibbs free energy as it relates enthalpy change to entropy change) which is ==> GibbsFE change= Enthalpy change - Entropy change×temperature
b) The molar gas formula PV=nRT
c) find the molecular formula of H2O which will be 16+2= 18
d) the formula for entropy change which is :Entropy change= Reversible energy transfered \Kelvin temperature
So 2.0kg x 1000= 2000 grams
2000\18 will give you the number of moles.
Anyway what I'm telling you is based on the A level qualification, so it might not be more into depth. I've got a whole lot of math to learn rn so sorry i couldn't finish. Any of you here that could help me with math?