CHEM 1A03 Study Guide - Final Guide: Stoichiometry, Process Function, Phase Transition

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CHEM 1A03 Full Course Notes

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Entropy of dissolution: entropy drives the process of dissolution of solutes. If a solute is very ordered and a solvent is somewhat disordered, then when they are mixed they produce a solution that is even more disordered. If i added the entropy of the solute and the entropy of the solvent, then they would total less than the entropy of the solution: therefore, mixing creates additional entropy. If the number of moles of gas decreases, then s rxn is negative. If heat flows into the surroundings from the system then the qsurroundings is -qsystem: qsystem is hsystem at constant temperature, heat is transferred irreversible so qsurroundings is - hsystem, spontaneity is predicted based on properties of the system only. If a reaction is exothermic then h is negative which makes g more negative. If we are at temperatures above the melting point, the t s term dominates and melting is spontaneous.

Related Questions

1) WHY does the dissolution of HCl(g) in water to formconcentrated hydrochloric acid INCREASE the change in entropy

Comments on 1:I know the answer, but need explaining.
I thought gas to liquid causes a decrease in entropy? What isdifferent about HCl (g)?

2)Please also answer this: Why does separating a mixture of N2and O2 into two separate samples, one that is pure N2 and one thatis pure O2 decrease change in entropy?

Comments on 2:I guess I don't really understand thequestion. I know it has to do with microstates, but what does itmean exactly? Is it because, when together, the molecules cancombine (thus increasing the number of possible arrangement ofatoms). But in separate containers they have more room tomove, which I thought would incrase entropy?

raspberrysnake855

Mixing Gases: Take two containers, each with volume 0.1 m³, containing ideal gases of monatomic He at T= 126 K and diatomic N₂ at T = 245 K, respectively. Each gas is at pressure p= 10⁶ Pa. A valve is opened allowing these two gases to mix. They are kept thermally isolated from the outside. Total Energy, Ui=400000 J and Uf=400000J

a)What is the final temperature of the mixed gas? T =

b) Now we want to calculate the change in entropy during this process. What is the change of dimensionless entropy solely due to the fact that the gases have more volume accessible? ÎÏ_vol =

cWhat is the change of dimensionless entropy solely due to the fact that the gasses' temperatures have changed?

ÎÏ_temp =

d)What is then the total change of dimensionless entropy? eq:ÎÏ =ÎÏvol+ÎÏtemp

ÎÏ =

e)What is the change of the standard entropy in this process? Eq:ÎS=kÎÏ

ÎS =

CHEM 1A03 Study Guide - Final Guide: Stoichiometry, Process Function, Phase Transition

CHEM 1A03 Full Course Notes

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