Calculate the cell potential for Ca(s) + Mn2+(aq) ↔ Ca2+(aq) + Mn(s). Assume any aqueous species has a concentration of 1 M.
Ca2+(aq) + 2e- → Ca(s) Eº = -2.87 V
Mn2+(aq) + 2e- → Mn(s) Eº = -1.18 V
Calculate the cell potential for Ca(s) + Mn2+(aq) ↔ Ca2+(aq) + Mn(s). Assume any aqueous species...
Calculate the cell potential, the equilibrium constant, and the free-energy change for: Ca(s)+Mn2+(aq)(1M)⇌Ca2+(aq)(1M)+Mn(s) given the following Eo values: Ca2+(aq)+2e−→Ca(s) Eo = -1.59 V Mn2+(aq)+2e−→Mn(s) Eo = -0.54 V 1.) Calculate the equilibrium constant. 2.) Free-energy change?
Calculate the cell potential, the equilibrium constant, and the free energy change for Ca(s) + Mn2+ (aq)(1M)=Ca²+ (aq)(1M) + Mn(s) given the following E' values: Ca2+ (aq) + 2e →Ca(8) Eº = -1.50 V Mn2+ (aq) + 2e →Mn(s) E° = -0.58 V
What is Eº for the cell Mn| Mn2+ (aq) || Ag+ (aq) | Ag? Standard Reduction Potentials E° (V) Ag+(aq) + e + Ag(s) +0.80 Mn2+(aq) + 2e Mn(s) -1.18 V 1 2 3 Х 1
please help and answer all questions 4. What is the cell potential for Mn Mn2||Co2|Co, based on the standard potentials? (2 pts) Mn(s) +Co+2 (aq) → Co(s) + Mn+2(aq) 5. A Student constructed a Mg Mg2||Ag|Ag cell and measured a cell potential of 3.17 V. Calculate the cell potential of the Mg Mg2 half reaction. (2 pts) Mg(s) + 2Ag (aq) - 2Ag(s) + Mg(aq) 6. Will silver metal react spontaneously with HCl(aq) to produce H:()? Explain. (2 pts) 2Ag(8)...
Calculate the value of Eºcell for the reaction 2Ag(s) + Ca2+(aq) + 2Ag+(aq) + Ca(s), using the following standard reduction potentials. Ag+(aq) + e- → Ag(s) E° = 0.80 V Ca2+(aq) + 2e + Ca(s) E° = -2.87 V 2.07 V -3.67 V 3.67 V -2.29 V -2.07 V
calculate equilibrium constant and free energy change please Calculate the cell potential, the equilibrium constant, and the free-energy change for Ca(s) + M12+ (aq)(1M) = Cap+ (aq)(1M) + Mn(3) given the following E' values: Ca2+ (aq) + 2e + Ca(8) E° = -1.50 V Mn2+ (aq) + 2e - →Mn(s) E° = -0.58 V Part A Calculate the cell potential 0.920 V Previou Correct Part B Calculate the equilibrium constant I ALCO ? Submit Previous Answers Request Answer X Incorrect;...
A voltaic cell employs the following redox reaction: Sn2+(aq)+Mn(s)---- Sn(s)+Mn2+(aq) Calculate the cell potential of 25 degrees Celsius under each of the following conditions. Part A: Sn2+= 1.15*10^-2 M; and Mn2+= 2.37 M Part B: Sn2+= 2.37 M; and Mn2+= 1.15*10^-2
LABORATORY 10 DETERMINATION OF VITAMIN C CONCENTRATION 3. How many grams of (pure) vitamin C is contained in your unknown stock solution (Part A)? Hint: The solution is made in a 1-L bottle. 4. Consider the following titration: If 21.35 mL of 0.005 M iodine solution is needed to titrate a solution of commercial vitamin C tablet (500 mg) pre- pared in a 100-mL volumetric flask, then what is the mass (%) of vitamin C in the commercial tablet? 5....
Hi, if someone can explain how to do this for me, I'd appreciate it! Calculate the cell potential, the equilibrium constant, and the free-energy change for: Ca(s)+Mn2+(aq)(1M)⇌Ca2+(aq)(1M)+Mn(s) given the following Eo values: Ca2+(aq)+2e−→Ca(s) Eo = -1.57 V Mn2+(aq)+2e−→Mn(s) Eo = -0.63 V
For the cell shown, the measured cell potential, Ecell, is -0.3707 V at 25°C. Pt(s) H(8, 0.857 atm) H+ (aq.? M) || Cd2+ (aq, 1.00 M) | Cd() The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2e- H,(g) E° = 0.00 V Ca2+ (aq) + 2e Cd(s) E = -0.403 V Calculate the H* concentration.