Splitting
For the exothermic reaction
Mg(s) + 2 H+(aq) <> Mg2+(aq) + H2(g)
at equilibrium, what will increasing the container volume do to Q?
Q will decrease
The following complex ions are colorless (can choose multiple or none also)
a) InCl4-
b) Lu(OH)64-
c) Zr(NO2)64-
What is InCl4-?
Q > K, which way is the reaction going to progress
What is backwards.
Tricky question: Q and K were reversed, it actually is going backwards.
I promise, no more tricks outside the tricky category...
What is wrong here?
A(l) + B(s) <> C(s)
Qc = 1/A
QC equals what at equilibrium
KC
When does an electron go to a higher orbital before the lower orbitals are all paired?
When there are no strong field ligands present
Which d-electron configurations are colorful and which are colorless?
Colorful: d1-d9
Colorless: d0 & d10
The value of Kc for the following reaction
6 C(s) + O2(g) + 8H2(g) <> 2 CH3CH2CH2OH(l) Kp = 5.69 x 10-3
What is 1.79 x 1010
What is wrong in the following?
2 PH3(g) <> 3 H2(g) + P(s)
I 0 0.90 atm 1 mol
C +2x -3x -3x
E 2x .30 atm 1 mol - 3x
The Phosphorous is a solid, so we don't need to write end for it here. Writing it out like this will end up mixing you up when you find your Q.
The QP of the following reaction
Br2(g) + 5F2 -> 2BrF5(g)
PBrF5
------------------
(PBr2) * (PF2)5
If the pairing energy is less than the splitting energy, are the ligands strong field or weak field?
Strong field
Calculate the splitting energy in Joules/photon for a complex ion emitting a photon of wavelength 520nm
3.825 x 10-19 J/photon
What is the formula for Kp for
6C(s) + O2(g) + 8H2(g) <> 2 CH3CH2CH2OH(l) Kc = 1.787 x 1010
Kp = 5.69 x 1010
(Letter names are spelled out)
Lambdamax = hc deltanought
Actually
Lambdamax = hc / deltanoughtIf we raise the temperature of the endothermic reaction
Mg2+(aq) + H2(g) <> Mg(s) + 2H+(aq)
the Q will ___ and according to Le Chatelier's Principle the reaction will go ___
Stay the same
Go backwards
Is Co(en)32+ Low spin or high spin?
Low spin
What range of electrons can be present in d-shells for them to have high and low spin complexes
d4-d7
2 P2O3(s) + O2(g) <> P4O8(s)
P4(s) + 3O2(g) <> 2 P2O3(s) Kc = 6.15 x 10-3
P4(s) + 4O2(g) <> P4O8(s) Kc = 0.35
What is 56.9
Which has stronger ligands, a red or a green octahedral complex?
(hint: rainbows go from longest to shortest wavelength)
Green (Roy G. Biv going from longest wavelength being red)
Wavelength \/
Deltaought /\
Ligand strength /\
Consider the equilibrium reaction at 25C
3 H2(g) + 2P(s) <> 2 PH3(g)
10.0g of solid phosphorus is introduced into a 400.0mL flask that contains 0.60 atm of H2(g) but not any PH3(g). The flask is then sealed, and the system is allowed to reach equilibrium. At equilibrium, the partial pressure of H2(g) is 0.30 atm. (Molar mass of phosphorus = 30.97 g/mol.
Set up an ICE chart and find the KP of this reaction.
KP = 1.5
The d-orbital splitting energy diagram of MX64-
where it is d5
/\ ___ ___
| /\ \/ /\ \/ /\ __
Which combinations are possible
Colorful, paramagnetic Colorless, paramagnetic
Colorful, diamagnetic Colorless, diamagnetic
Colorful paramagnetic,
Colorful diamagnetic,
Colorless, diamagnetic
NOT colorless paramagnetic (no unpaired electrons if colorless)
Consider the equilibrium reaction at 25C
3 H2(g) + 2P(s) <> 2 PH3(g)
10.0g of solid phosphorus is introduced into a 400.0mL flask that contains 0.60 atm of H2(g) but not any PH3(g). The flask is then sealed, and the system is allowed to reach equilibrium. At equilibrium, the partial pressure of H2(g) is 0.30 atm. (Molar mass of phosphorus = 30.97 g/mol.
Set up an ICE chart and find the KP of this reaction.
KP = 1.5
Where is the mistake?
AgC2H3O2(aq) <> Ag+(aq) + C2H3O2-(aq)
I 0.250M 0 0
C -x +x +x
E 0.250 - x x x
Kp = 0.045 = x2 / ( 0.250 - x)
(0.045)(0.250 - x) = x2
0.01125 -0.045x = x2
0 = x2 + 0.045x - 0.01125
x = [ (-0.045 +- ( (0.045)2 - 4(1)(-0.01125)2 ) 1/2 ] / 2*
x = -0.0435, -0.133 ??????
* 1/2 means square root
(.01125)2 should not be squared
Consider the following reaction at 35C
AgC2H3O2(aq) <> Ag+ (aq) + C2H3O2-(aq) KC = 0.045
A solution that initially contains 0.250 M of AgC2H3O2(aq) is allowed to reach equilibrium at constant temperature. Determine the concentration of Ag+ ions at equilibrium.
[Ag+] = 0.0859 M