Question | Answer |
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) |