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Calculate the cell potential, the equilibrium constant, and the free energy change for Ca(s) + Mn2+...
calculate equilibrium constant and free energy change please Calculate the cell potential, the equilibrium constant, and...
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;...
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...
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?
znt" + 2e nt 4. Calculate the cell potential, the equilibrium constant, and the free energy...
znt" + 2e nt 4. Calculate the cell potential, the equilibrium constant, and the free energy change for Ba(s) + Mn?' (aq, 1 M) → Ba?' (aq, 1 M) + Mn(s) Given the following Eº values: Ba2+(aq) + 2e → Ba(s) E'= -2.90V Mn²+(aq) + 2e → Mn(s) E°=+0.80 V
Calculate the cell potential for Ca(s) + Mn2+(aq) ↔ Ca2+(aq) + Mn(s). Assume any aqueous species...
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
Hi, if someone can explain how to do this for me, I'd appreciate it! Calculate the...
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
please help and answer all questions 4. What is the cell potential for Mn Mn2||Co2|Co, based...
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)...
LABORATORY 10 DETERMINATION OF VITAMIN C CONCENTRATION 3. How many grams of (pure) vitamin C is...
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....
For the cell shown, the measured cell potential, Ecell, is -0.3707 V at 25°C. Pt(s) H(8,...
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.
What is Eº for the cell Mn| Mn2+ (aq) || Ag+ (aq) | Ag? Standard Reduction...
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
Free-energy change, AGº, is related to cell potential, Eº, by the equation AG° = -nFE° where...
Free-energy change, AGº, is related to cell potential, Eº, by the equation AG° = -nFE° where n is the number of moles of electrons transferred and F = 96,500 C/(mol e ) is the Faraday constant. When Eº is measured in volts, AGⓇ must be in joules since 1 J =1C.V. Part A Calculate the standard free-energy change at 25°C for the following reaction: Mg(s) + Fe2+ (aq)Mg2+ (aq) + Fe(s) Express your answer to three significant figures and include...
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;...
znt" + 2e nt 4. Calculate the cell potential, the equilibrium constant, and the free energy change for Ba(s) + Mn?' (aq, 1 M) → Ba?' (aq, 1 M) + Mn(s) Given the following Eº values: Ba2+(aq) + 2e → Ba(s) E'= -2.90V Mn²+(aq) + 2e → Mn(s) E°=+0.80 V
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)...
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....
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.
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
Free-energy change, AGº, is related to cell potential, Eº, by the equation AG° = -nFE° where n is the number of moles of electrons transferred and F = 96,500 C/(mol e ) is the Faraday constant. When Eº is measured in volts, AGⓇ must be in joules since 1 J =1C.V. Part A Calculate the standard free-energy change at 25°C for the following reaction: Mg(s) + Fe2+ (aq)Mg2+ (aq) + Fe(s) Express your answer to three significant figures and include...
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