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
Co+2 + 2e- → Co Eo = -0.277 V Ce+4 + e- → Ce+3 Eo = 1.61 V The substance that will be oxidized in the battery above.
Co
100
The an ox and red cat in electrochemistry help you remember this?
What is anode is oxidized and cathode is reduced
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
0.277 V
200
Identify the reducing agent of the following chemical reaction: Cd + NiO2 +2H2O --> Cd(OH)2 + Ni(OH)2
Cd
300
The oxidation number for Magnesium in MgF2.
What is +2.
300
In a voltaic cell, the electrons flow towards the ______ .
What is towards the cathode
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
300
Identify the substance that is oxidized and reduced in the following equation. Fe + V2O3 --> Fe2O3 + VO
Fe is oxidized, V is reduce
400
The oxidation number for each element in PO4-3
What is -2 for oxygen and +5 for phosphorus.
400
In the salt bridge the nitrate ions flow towards the ______ while the sodium ions flow towards the ________
What is anode and cathode
400
MoO3 + Zn + H2SO4 --> Mo2O3 + ZnSO4 + H2O Balance this equation.
2MoO3 + 3Zn + 3H2SO4 --> Mo2O3 + 3ZnSO4 + 3H2O
400
The correct balanced equation for the voltaic cell represented by the two half cell equations below. Co+2 + 2e- → Co Eo = -0.277 V Ce+4 + e- → Ce+3 Eo = 1.61 V
2Ce+4 + Co → 2Ce+3 + Co+2
400
Balance the following redox reaction. K2Cr2O7 + H2O + S --> SO2 + KOH + Cr2O3
2K2Cr2O7 + 2H2O + 3S --> 3SO2 + 4KOH + 2Cr2O3
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
Draw the voltaic cell for the following equation. Be sure to label anode and cathode and show the direction the electrons are flowing. Zn(s) + Cu2+(aq) → Cu(s) + Zn2+(aq)
Zinc is anode, copper is cathode, electrons are flowing from anode to cathode
500
Al(s)|Al3+||Pb2+|Pb(s) Calculate the Eo for the reaction.
1.53 V
500
The best science teacher you have ever had at Benilde
What is all of them
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