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A voltaic cell is constructed with a Cr/Cr3+ half-cell (E° = -0.73 V) and a Ni/Ni2+ half-cell
(E° = -0.23 V).
a. Write balanced half-reactions and the overall spontaneous reaction.
b. Diagram the cell. Be a specific as possible including labeling electrodes with their
charges and names (anode and cathode), showing the direction of electron flow in
the circuit and showing the direction of cation and anion flow in the salt bridge.

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Step by stepSolved in 4 steps with 3 images
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C. Calculate the cell potential for the overall reaction.
D. Calculate the Gibbs free energy for the overall reaction.
E. Write the standard cell notation for the overall reaction.
C. Calculate the cell potential for the overall reaction.
D. Calculate the Gibbs free energy for the overall reaction.
E. Write the standard cell notation for the overall reaction.
- Enter electrons as e". Use smallest possible integer coefficients. If a box is not needed, leave it blank. A voltaic cell is constructed from a standard Pb2+|Pb half cell (E°,red :-0.126V) and a standard Zn2+|Zn half cell (E° red -0.763V). The anode reaction is: + + The cathode reaction is: + + The spontaneous cell reaction is: + + The cell voltage is V.arrow_forward2arrow_forwardHey im stuck on this sheet :) (no explanation or diagram needed)arrow_forward
- Enter electrons as e¯. Use smallest possible integer coefficients. If a box is not needed, leave it blank. A voltaic cell is constructed from a standard Co²+ | Co half cell (E° red = -0.280V) and a standard Mg2+ | Mg half cell (E°red = -2.370V). The anode reaction is: + The cathode reaction is: → + The spontaneous cell reaction is: + The cell voltage is V. ↑ +arrow_forwardA cvg.cengagenow.com eneral... Netflix Flipgrid | 50ffc... Content GRLContent Netflix Favorites My Home [Review Topics] [References] Use the References to access important values if needed for this question. What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Hg** concentration is 4.25×10-4 M and the Al3+ concentration is 1.06 M ? 3Hg²"(aq) + 2AI(s)3Hg(1) + 2AI³*(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given:arrow_forward|The electrolysis of Bio* produces pure bismuth. How long would it take to produce 7.50 g Bi by the electrolysis of a Bio* solution using a current of 27.5 A? Time min =arrow_forward
- Payliarrow_forwardFor a Magnesium-Aluminum cell [Mn2+ + 2e- --> Mn (-1.18V)] [Al3+ + 3e- --> Al (-1.66)]: 1. label anode, cathode2. write half reactions3. Write overall reaction4. Write cell notation5. Calculate E6. Calculate G = -nFe7. Show and give example of how G is related to K8. Calculate Nernst for various Molarity changes (show how E changes)9. Calculate grams at cathode for different amounts of timearrow_forwardDo not have to answer any questions. JUST WRITE THE OBJECTIVES IN YOUR OWN RODS: Objective: To measure Ecel for several voltaic cells and determine the standard potential for each half cell. To determine Ksp of AgCl and the K of [Cu(NH3)4]*.arrow_forward
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