CHEM 126 Final
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
|
|
||||
|---|---|---|---|---|---|
| relationship between forward and reverse rexn rates at equilibrium | rate(forward) = rate(reverse)
🗑
|
||||
| expression for equilibrium constant (Keq) | [C]c*[D]d/[A]a*[B]b = Keq
* all elements at eq
🗑
|
||||
| expression for reaction quotient (Q) | [C]c*[D]d/[A]a*[B]b = Q
* all elements at t (point in time)
🗑
|
||||
| solids/liquids in equilibrium constant | - solids/liquids not calculated for K/Q -> won't affect equation
🗑
|
||||
| Determine Keq when... | - reverse reaction: negative Kc
- multiply rxn by constant: multiply Kc by factor
- Adding multiple rxns: Qoverall = Q1 x Q2 x Q3 VS Koverall = K1 x K2 x K3
🗑
|
||||
| compare Q & K, what direction will it proceed in? | - Q < K -> need to make more product, go right
- Q > K -> need to make more reactant, go left
- Q = K -> rxn at equilibrium
🗑
|
||||
| concentration vs pressure values for K or Q | - Kp = Kc(RT)^ (change number gas moles)
- Kc = values in concentration, mol/L
- Kp = values in pressure, atm or Pa
🗑
|
||||
| Le Chatelier's principle | - chem system at equilibrium disturbs -> reattains equation by undergoing a net rxn that decreases effect of disturbance
🗑
|
||||
| Concentration changes (le chateliers principle) | - - concentration change: direction changes to re-establish original rations, no effect on K
- Volume decrease by 1/2 -> conc. increase by 2
- Volume increase -> pressure becomes lower -> total number of gas molecules increase
🗑
|
||||
| pressure changes (le chateliers principle) | - pressure change: change to reestablish original P ration, no effect on K (only for gases)
- Increase: shift to side with less gas moles
- Decrease: shift to side with larger gas moles
🗑
|
||||
| [A] -> B + heat | - endothermic
- temp increases because system absorbs heat by decomposing B -> increase Kc
🗑
|
||||
| [A] <- B + heat = endothermic | - temp increases because system absorbs heat by decomposing B -> increase Kc
🗑
|
||||
| catalyst | - non direction change/effect on K
- rate forward increase -> reverse rate increase
- get to same place faster
🗑
|
||||
| calculate new value of K at different temps | ln(k2/k1) = (-∆Hrxn/r)*)(1/T2 - 1/T1)
🗑
|
Review the information in the table. When you are ready to quiz yourself you can hide individual columns or the entire table. Then you can click on the empty cells to reveal the answer. Try to recall what will be displayed before clicking the empty cell.
To hide a column, click on the column name.
To hide the entire table, click on the "Hide All" button.
You may also shuffle the rows of the table by clicking on the "Shuffle" button.
Or sort by any of the columns using the down arrow next to any column heading.
If you know all the data on any row, you can temporarily remove it by tapping the trash can to the right of the row.
To hide a column, click on the column name.
To hide the entire table, click on the "Hide All" button.
You may also shuffle the rows of the table by clicking on the "Shuffle" button.
Or sort by any of the columns using the down arrow next to any column heading.
If you know all the data on any row, you can temporarily remove it by tapping the trash can to the right of the row.
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
Created by:
ccottrel
Popular Chemistry sets