Magnesium metal is oxidized and silver ions are reduced in a voltaic cell using:
Mg(s) | Mg2+ (aq, 1M) || Ag+ (aq, 1M) | Ag(s)
a. Draw the voltaic cell. Label each part of the cell.
b. Write the equations for the half-reactions occurring at the anode and cathode.
c. Write the overall reaction for the cell.
d. Draw arrows to show the movement of electrons in the external circuit. Assuming the salt bridge contains NaNO3, indicate the movement of Na+ and NO3- ions in the salt bridge.
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
Magnesium metal is oxidized and silver ions are reduced in a voltaic cell using: Mg(s) |...
Consider the voltaic cell diagram shown below. Your cell is made up of a Magnesium and a Mercury electrode. Match the letters to the correct answers. Mg2+(aq)+2e --> Mg(s) Ered= -2.37V Hg22+ (aq)+2e --> 2Hg(s) Ered=0.80V [Choose ] CI- Salt Bridge Hg Anode Na+ MgNO3 Oxidation number Hg2NO3 Hg Cathode Mg(NO3)2 Hg2(NO3)2 Salt flow Mg Anode Mg Cathode Electron flow
Consider a galvanic cell in which Al3 is reduced to elemental aluminum, and magnesium metal is oxidized to Mg2 . Write the balanced half-cell reactions that take place at the cathode and at the anode. Consider a galvanic cell in which Al^3 is reduced to elemental aluminum, and magnesium metal is oxidized to Mg2 . Write the balanced half-cell reactions that take place at the cathode and at the anode. Half - cell reaction at the cathode Half - cell...
Consider the following voltaic cell: Sn(s) Sn2+ || Cu2+ Cu(s) Which metal is being oxidized? [Select] Which metal is being reduced? (Select] Identify and label the anode and cathode. anode (Select] cathode (Select] Salt bridge is made with potassium nitrate, show ion flow. [Select] Which electrode decreases in mass during cell operation? [Select] In which direction do electrons flow in the external circuit? [Select] At which electrode are electrons generated? [Select]
Enter electrons as e A voltaic cell is constructed in which the anode is a Mg Mg2+ half cell and the cathode is a Ni Ni2+ half cell. The half- cell compartments are connected by a salt bridge. (Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (ag) or (s). If a box is not needed, leave it blank.) The anode reaction is: The cathode reaction is: The net cell reaction is: In the external...
2. Write the cell notation for an electrochemical cell consisting of an anode where Mg (s) is oxidized to Mg2+(aq) and a cathode where Al3+(aq) is reduced to Al (s) . Assume all aqueous solutions have a concentration of 1 mol/L. Enter electrons as e Use smallest possible integer coefficients for ALL reactions. If a box is not needed, leave it blank. A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are connected by...
A voltaic electrochemical cell is constructed in which the anode is a Mg?+| Mg half cell and the cathode is a Zn?-Izn half cell. The half-cell compartments are connected by a salt bridge. Write the anode reaction Write the cathode reaction. + Write the net cell reaction the Zn?+ Zn electrode the Mg2+ Mg electrode In the external circuit, electrons migrate In the salt bridge, anions migrate the Zn2+ Zn compartment the Mg2+ Mg compartment. Submit Answer
Consider a galvanic cell in which A1+ is reduced to elemental aluminum and magnesium metal is oxidized to Mg2+ Write the balanced half-cell reactions that take place at the cathode and at the anode. half-cell reaction at the cathode: half-cell reaction at the anode:
A voltaic cell is constructed in which the anode is a Ag Ag half cell and the cathode is a CI Cl2 half cell. The half-cell compartments are connected by a salt bridge. (Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: The cathode reaction is: The net cell reaction is: the Ag Ag electrode. |the CIICl2 electrode In...
In a copper-zinc voltaic cell, one half-cell consists of a ZnZn electrode inserted in a solution of zinc sulfate and the other half-cell consists of a CuCu electrode inserted in a copper sulfate solution. These two half-cells are separated by a salt bridge. At the zinc electrode (anode), ZnZn metal undergoes oxidation by losing two electrons and enters the solution as Zn2+Zn2+ ions. The oxidation half-cell reaction that takes place at the anode is Zn(s)→Zn2+(aq)+2e−Zn(s)→Zn2+(aq)+2e− The CuCu ions undergo reduction...
A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. Co(s) + 2Ag+(aq)Co2+(aq) + 2Ag(s) Write the reactions that take place at the anode and at the cathode, the direction in which the electrons migrate in the external circuit, and the direction the anions in the salt bridge migrate. Use smallest possible integer coefficients. If a box is not needed, leave it blank. Enter the reaction that takes place at the...