Search Results
| Search type | Search syntax |
|---|---|
| Tags | [tag] |
| Exact | "words here" |
| Author |
user:1234 user:me (yours) |
| Score |
score:3 (3+) score:0 (none) |
| Answers |
answers:3 (3+) answers:0 (none) isaccepted:yes hasaccepted:no inquestion:1234 |
| Views | views:250 |
| Code | code:"if (foo != bar)" |
| Sections |
title:apples body:"apples oranges" |
| URL | url:"*.example.com" |
| Saves | in:saves |
| Status |
closed:yes duplicate:no migrated:no wiki:no |
| Types |
is:question is:answer |
| Exclude |
-[tag] -apples |
| For more details on advanced search visit our help page | |
Results tagged with equilibrium
Search options not deleted
user 101509
The state in which both reactants and products are present at concentrations which have no further tendency to change with time.
9
votes
3
answers
855
views
Why is standard state useful?
We fill the container with $\ce{A}$ and after some time has passed equilibrium is established. … At least for gases it doesn't make sense because in equilibrium is their partial pressure that matters. …
- 766
2
votes
1
answer
210
views
Can we have an equilibrium constant for a reaction at constant volume?
Can the equilibrium state now be predicted? … I mean if the piston was movable (e.g. coupled to an external pressure of $1$ atm) the system would reach equilibrium and we could find the equilibrium state (e.g. the gas composition) by using the equilibrium …
- 766
5
votes
0
answers
38
views
Do the differential expressions of second law of thermodynamics imply a smooth increase in e... [closed]
Suppose that the system is at equilibrium state (state $1$) at time $t$. Something happens (e.g. a chemical reaction takes place) so the system will reach a new equilibrium state (state $2$). … To be honest I haven't seen any reaction reaching equilibrium in that way but I can't find a reason why it should not behave this way. …
- 766
1
vote
2
answers
1k
views
Is it valid to calculate concentrations given equilibrium constant and initial concentration?
Now if we are given that initial we have $x$ mol of $\ce{A}$ and no amount of $\ce{B}$ and $\ce{C}$, one can calculate the amount of B and C present at equilibrium using the equilibrium constant $K$:
$ … It is a common exercise in many general Chemistry textbooks where you are given a reaction with an equilibrium constant and you must find the concentrations at equilibrium. …
- 766
1
vote
0
answers
182
views
Understanding Pourbaix diagram
I was taught that the lines in the Pourbaix diagrams are equilibrium lines. … The reaction describing this equilibrium line is (with equilibrium constant $K$):
$$\ce{2H+_{(aq)} + 2e- <=> H2_{(g)}}$$
Now at equilibrium taking the $\log K$ and equilibrium constant we obtaing:
$$\log …
- 766