Acid Base
Kinetics
Equilibrium
Electrochemistry/Thermochemistry
Miscellaneous
100
What happens to the pH of water when it is heated greater than 25ㅇC?
the pH becomes lower than 7
100
At which point is the Kinetic Energy the highest?
3
100
At equilibrium, what happens to pressure when adding an inert gas?
Pressure increases
100
Is this reaction spontaneous or non-spontaneous?
Pt(s) + Cu2+(Aq) ➝ Pt2+(aq) + Cu(s)
It's non-spontaneous
100
Name any solubility rule
NH4 & group 1 metal cations never form ppts
200
Which one is the Strongest acid:
a) sulfuric acid
b) orange juice
c) battery acid
d) lemon juice
c) battery acid
200
the rate= k[A]²
Which of the following plots will give a straight line? And why?
a) [A]² versus time
b) [A] versus time
c) 1/[A] versus time
c), because second-order rate law
200
Exothermic reaction: what happens when:
a) You add heat
b)decrease heat
and what happens with K at these temperatures?
T increases: shift toward reactants
T decreases: shift towards products
K > @ low temp
K < @ high temp
200
label a galvanic cell and write the cell diagram for the equation 2Ag+(aq)+Cu(s)⇌Cu2+(aq)+2Ag(s)
A:Cu+ B:Cu C:Ag+ D:Ag E:salt bridge with KNO3. Cu(s)|Cu2+||Ag+|Ag(s)
200
Name the molecular and electron geometry for SF2
M - bent E - tetrahedral
300
Find pOH and pH of .33 M solution
Given: Kb = 4.4 x 10^-4
CH3NH2 + H2O → ← CH3NH3 + OH-
pOH = 1.93
pH = 12.07
300
Define Activation Energy (Ea) and label it in a diagram
Known as the barrier that reactants have to overcome to get reaction going
300
Endothermic reaction: what happens when:
a) You add heat
b)decrease heat
and what happens with K at these temperatures?
T increases: shift toward products
T decreases: shift towards reactants
K <@ low temp
K > @ high temp
300
How many minutes will take to plate out 40.00 g of Ni form a solution of NiSO4 using a current of 3.450 amp?
635.3 min
300
Assign Oxidation Numbers CO3^ 2-
C = +4 O = -2
400
Sketch the graph of the titration curve for a diprotic acid titrated with a strong base and indicate roughly the pH at the equivalent points.
The first equivalence point should be below 7 and the second should be above 7
400
For reaction:
2A + B2 ➝ C + D
the rate law = k[A]2[B]0
Which is most likely the rate determining step?
A) A + B2 ➝ X B)A + B ➝ X
C)A + A ➝ X D) 2A + B ➝ X
C)
400
Which way will the system go to reach equilibrium?C(s) + CO2 (g) + 2Cl2 (g)↔️ 2COCl2 (g)
.1M=CO2 .2M=Cl2 .368M=COCl2
K = 3.1 x1015
Q<K It will go forwards to reach equilibrium.
400
What is the cell potential for I2 (s)+ 2Rb(s) ➝ 2I- (aq)+ 2Rb+(aq)?
E° = 3.47 V
400
Name one rule of the Kinetic Molecular Theory
V of gas particles is negligible compared to the space between them
KE energy is proportional to the Kelvin Temp
Collisions are perfectly elastic
500
Will a precipitate form when 150 mL of 0.10 M Pb(NO3)2 are combined with 100 mL of 0.20 M NaCl? (Ksp=1.2 x 10-5 for PbCl2 (s))
PbCl2 (s) ↔ Pb2+ (aq) + 2 Cl— (aq)
.06M .08M
Q = [Pb2+][Cl—] 2 = (0.060)(0.080)2 = 3.8 x 10—4
Q>ksp so precipitate will form
500
What is the overall reaction order and rate law
2Mg + O2➝ 2MgO | Rate = k[Mg]n[O2]m | ||
Trial | Initial [Mg] (mol/L) | Initial [O2] (mol/L) | Measured Rate (mol/L*s) |
1 | .10 | .10 | 2.0x10^-3 |
2 | .20 | .10 | 4.0x10^-3 |
3 | .10 | .20 | 8.0x10^-3 |
rate law= k[Mg]1[O2]2
The overall order is 3.
500
3.00 moles of N2 gas and 1.00 mole of H2 gas are combined in a 1 L reaction vessel. At equilibrium 0.663 moles of H2 remain. What are the resulting concentrations?
N2 + 3H2⇔2NH3
N2: 2.89 M
H2: 0.663 M
NH3: 0.225 M
500
Given the voltaic cell calculate the change in free energy (△G)
(Hint: △G = -nFE० and F = 96,485 C/mol)
△G = -212 kj
500
Solve Hess’s Law
Given:
2NO + O2 → 2NO2 △H = -113.1 kJ/mol rxn
N2 + O2 → 2NO △H = +182.6 kJ/mol rxn
2N2O → 2N2 + O2 △H = -163.2 kJ/mol rxn
N2O + NO2 → 3NO △H = ?
△H = +157.55 kJ/mol rxn