Oxidation States
Voltaic Cells
Redox Reactions
Cell Potential
Misc
100
The oxidation number of any metal in its elemental state.
What is 0.
100
Oxidation takes place at the ______ and reduction takes place at the ______ .
What is the anode, cathode.
100
The difference between oxidation and reduction.
What is oxidation is loss of electrons and reduction is gain of electrons
100
The no-freaking-way equation.
What is Delta G = -n x F x Ecell.
100
The ox and cat in electrochemistry help you remember.
What is anode and cathode.
200
The oxidation number of this type of ion is the same as its charge.
What is a monotomic ion.
200
The device used to maintain electrical neutrality.
What is the salt bridge.
200
The oxidizing agent in this reaction. Zn(s) + 2H+(aq) --> Zn+2(aq) + H2(g)
What is 2H+.
200
Find the cell potential of a galvanic cell based on the following reduction half-reactions at 25 °C Cd2+ + 2 e- → Cd E0 = -0.403 V Pb2+ + 2 e- → Pb E0 = -0.126 V where [Cd2+] = 0.020 M and [Pb2+] = 0.200 M.
What is the cell potential for the two reactions at 25 °C and [Cd2+] = 0.020 M and [Pb2+] = 0.200 M is 0.290 volts.
200
The name of this equation: n DE° log K = -------- 0.0592
What is the Nernst equation.
300
The oxidation number for Magnesium in MgF2.
What is +2.
300
The electrons flow towards the ______ . http://projectshum.org/wp-content/uploads/Zn-Cu-galvanic-cell.png
What is towards the copper electrode.
300
The equation that represents a reaction that is not a redox reaction is: 1. 2H2 + O2 → 2H2O 2. Zn + CuSO4 → ZnSO4 + Cu 3. 2H2O2 → 2H2O + O2 4. H2O + CO2 → H2CO3
What is Reaction 4.
300
Find the standard cell potential for an electrochemical cell with the following cell reaction. Zn(s) + Cu2+(aq) Zn2+(aq) + Cu(s) Eoreduction of Cu2+ = + 0.339 V Eoreduction of Zn2+ = - 0.762 V
What is Eocell = + 1.101 V Zn(s) Zn2+(aq) + 2 e- Cu2+(aq) + 2 e- Cu(s) Eooxidation of Zn = - ( - 0.762 V) = + 0.762 V
300
With a current of 20 amps, how long would it take to generate 1.00 kilograms of aluminum by the reaction: Al3+ + 3e- → Al(s)
What is 0.368 g
400
The oxidation number for each element in PO4-3
What is -2 for oxygen and +5 for phosphorus.
400
A concentration cell is constructed by placing identical Cu electrodes in two Cu2+ solutions. If the concentrations of the two Cu2+ solutions are 1.0 M and 0.0020 M, calculate the potential of the cell.
What is 0.080 Volts.
400
Fe+2 + MnO4-1 --> Fe+3 + Mn+2 Balance this equation.
What is 5Fe+2 +MnO4-1 + 8H+ --> 5Fe+3 + Mn+2 + 4H2O
400
21.2 M(s) + 3 Zn2+(aq) → 2 M3+(aq) + 3 Zn2+(aq) E° = 0.90 V Zn2+(aq) + 2e– → Zn(s) E° = –0.76 V Using the above information, determine the standard reduction potential for the following reaction: M3+(aq) + 3e–→ M(s)
What is 1.66 V
400
The equilibrium constant (K) for the reaction below is approximately: ◦Cl2 + 2e- → 2Cl- (E0 = 1.36v) ◦Cu+ + e- → Cu (E0 = 0.52v)
What is 10 x 10^28
500
The oxidation number zinc in this reaction changes from. Zn + I2 --> ZnI2
What is 0 to +2.
500
Using a galvanic cell containing Zinc and Copper, write the shorthand notation. Zn+2 + 2e- --> Zn(s) = -0.76 Volts Cu+2 + 2e- --> Cu(s) = 0.34 Volts
What is Zn(s) | Zn2+(aq) || Cu2+(aq) | Cu(s)
500
MnO4-(aq) + 5 Fe2+(aq) + 8 H+(aq) → Mn2+(aq) + 5 Fe3+(aq) + 4 H2O Calculate the volume of 0.100 M KMnO4 needed to react with 25.0 cm3 0.100 M Fe2+ and the concentration of Fe2+ in a solution if you know that 20.0 cm3 of solution reacts with 18.0 cm3 of 0.100 KMnO4
What is 5.00 cm^3
500
Predict the cell potential for the following reaction when the pressure of the oxygen gas is 2.50 atm, the hydrogen ion concentration is 0.10 M, and the bromide ion concentration is 0.25 M. O2(g) + 4 H+(aq) + 4 Br-(aq) 2 H2O(l) + 2 Br2(l)
What is Eocell = + 0.152 V
500
The best teacher.
What is Doc Louey.
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