1) Assume that the reference half-cell is changed to a standard mercury-mercury (II) half-cell.
a) What would be the reduction potential of a standard chlorine half-cell.
c) What would be the cell potential of a standard chlorine-nickel cell.
2) For each of the following standard cells, write the cell notation, label electrodes, and determine the cell potential.
a) tin(IV) zinc standard cell.
If someone could explain the questions/help me with them so I can do the remaining work it would be greatly appreciated. Thanks!
For #1.
I do these this way. The dashed lines represent the voltage for the reduction reactions shown.
--------- Cl2 + 2e ==> 2Cl^-   +1.4
--------- Hg^+2 + 2e ==> Hg   +0.85
--------- 2H^+ + 2e ==> H2   0.0
The spacing is arbitrary; I just put the vertical spacing between the dashed lines to show how I do it. Normally, you see, the standard H cell is 0 voltage and the Cl2 reduction potential is +1.4 volts above H. The difference between 1.4 and 0 is of course 1.4 volts. Now if we replace that H reference cell with a mercury(II)/Mercury cell, that is +0.85 with reference to H. So the Cl2 potential measured against the Mercury as a reference cell will be 1.4 - 0.85 = 0.55 volts. These number I am using are from an OLD OLD text I had in graduate school and you need to look in your text/notes and pick up the up to date numbers. I hope this helps. I think the drawing with the dashed lines is the only way I can see how to do these. It may or may not help you.
I don't know your trouble with the Zn/Ni cell. I don't understand the last problem.
Sure, I can help you with those questions. Let's go step-by-step.
1) a) To determine the reduction potential of a standard chlorine half-cell, we need to look up the standard reduction potential for the chlorine half-reaction. The reduction half-reaction for chlorine gas is:
Cl2(g) + 2e- -> 2Cl-(aq)
The standard reduction potential for this half-reaction is given as +1.36V. So, the reduction potential of a standard chlorine half-cell would be +1.36V.
b) To find the cell potential of a standard chlorine-nickel cell, we need to consider the reduction potentials of both the chlorine and nickel half-reactions. The half-reactions are:
Chlorine half-reaction: Cl2(g) + 2e- -> 2Cl-(aq) with its standard reduction potential of +1.36V.
Nickel half-reaction: Ni2+(aq) + 2e- -> Ni(s) with its standard reduction potential of -0.25V (given).
The overall cell potential can be calculated by taking the difference between the reduction potentials of the two half-reactions:
Cell potential = Reduction potential of chlorine half-cell - Reduction potential of nickel half-cell
= (+1.36V) - (-0.25V)
= +1.36V + 0.25V
= +1.61V
Therefore, the cell potential of a standard chlorine-nickel cell is +1.61V.
2) For the second set of questions, we need to determine the cell notation, label the electrodes, and calculate the cell potential for each standard cell.
a) For the tin(IV) zinc standard cell, the half-reactions are:
Tin(IV) half-reaction: Sn4+(aq) + 2e- -> Sn2+(aq) with an unknown standard reduction potential.
Zinc half-reaction: Zn2+(aq) + 2e- -> Zn(s) with a known standard reduction potential of -0.76V (given).
To write the cell notation, we write the oxidation half-reaction on the left side and the reduction half-reaction on the right side, separated by a vertical line:
Sn4+(aq) | Sn2+(aq) || Zn2+(aq) | Zn(s)
The anode (where oxidation occurs) is on the left side, and the cathode (where reduction occurs) is on the right side.
To determine the cell potential, we subtract the reduction potential of the anode half-reaction from the reduction potential of the cathode half-reaction:
Cell potential = Reduction potential of cathode - Reduction potential of anode
= -0.76V - (unknown reduction potential of the Sn4+ half-reaction)
Since the reduction potential of the Sn4+ half-reaction was not given, we cannot determine the value of the cell potential without that information.
I hope this helps! If you have any further questions, feel free to ask.
To answer these questions, you need to understand the basics of electrochemical cells and standard reduction potentials. I'll explain the concepts and guide you through the calculations.
1) Assume that the reference half-cell is changed to a standard mercury-mercury (II) half-cell.
a) What would be the reduction potential of a standard chlorine half-cell?
First, we need to find the reduction potential of a standard chlorine half-cell relative to the standard mercury-mercury (II) half-cell. The reduction potential is the tendency of a half-reaction to gain electrons.
The reduction potential values can be found in standard reduction potential tables. The reduction potential of the standard mercury-mercury (II) half-cell is 0.85 V.
Subtract the reduction potential of the standard mercury-mercury (II) half-cell from the reduction potential of the chlorine half-cell to get the answer:
Reduction potential of the chlorine half-cell = Reduction potential of chlorine - Reduction potential of mercury-mercury (II) half-cell
2) What would be the cell potential of a standard chlorine-nickel cell?
To determine the cell potential, you need to find the difference in the reduction potentials of the cathode (nickel) and anode (chlorine) half-cells.
Once again, refer to the standard reduction potential tables and note the reduction potentials of the nickel half-cell and chlorine half-cell.
The cell potential can be calculated using the equation:
Cell potential = Reduction potential of cathode - Reduction potential of anode
2) For each of the following standard cells, write the cell notation, label electrodes, and determine the cell potential.
a) tin(IV) zinc standard cell.
In a cell notation, the anode is always specified on the left, and the cathode is specified on the right. The anode is the electrode where oxidation occurs (loses electrons), and the cathode is the electrode where reduction occurs (gains electrons).
For the given cell, tin(IV) zinc standard cell, the cell notation would be:
Anode: Tin (IV) | Tin (IV) ion
Cathode: Zinc ion | Zinc
To determine the cell potential, subtract the reduction potential of the anode from the reduction potential of the cathode.
Cell potential = Reduction potential of cathode - Reduction potential of anode
Remember to look up the standard reduction potentials for tin (IV) and zinc in the standard reduction potential tables.
I hope this explanation helps you understand how to approach these questions. Let me know if you have any further questions!