For spontaneous Ni, Al galvanic cell, calculate Ecell if [Al3+]=1.80M, and [Ni2+]=0.0096M
For spontaneous Ni, Al galvanic cell, calculate Ecell if [Al3+]=1.80M, and [Ni2+]=0.0096M
Homework Answers
For a spontaneous process, Ecell
and E0 both must be positive.
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For spontaneous Ni, Al galvanic cell, calculate Ecell if
[Al3+]=1.80M, and [Ni2+]=0.0096M
A voltaic cell consists of an Ni/Ni2+ half-cell and a Co/Co2+ half-cell. Calculate Ecell when conc....
A voltaic cell consists of an Ni/Ni2+ half-cell and a Co/Co2+ half-cell. Calculate Ecell when conc. of Ni2+ = 0.142 M and of Co2+ = 0.468 M. The reduction potential for Ni2+ is -0.247 V and for Co2+ is -0.277 V. Answer: 0.01467 A voltaic cell consists of an Al/Al3+ half-cell and a Cd/Cd2+ half-cell. Calculate {Al3+} when {Cd2+} = 0.401 M and Ecell = 1.299 V.Use reduction potential values of Al3+ = -1.66 V and for Cd2+ = -0.40...
If you construct a Galvanic / Voltaic cell using a Ni(s) / Ni2+(aq) half cell and...
If you construct a Galvanic / Voltaic cell using a Ni(s) / Ni2+(aq) half cell and an Al(s)/ Al3+(aq)half cell,and connect the whole cell to a voltmeter by connecting the Al half cell to the positive terminal of the voltmeter, what will be the display?
Al3 (aq) + Ni(s). 3. Consider the unbalanced reaction Al(s)+ Ni2 (aq) > a. write balanced...
Al3 (aq) + Ni(s). 3. Consider the unbalanced reaction Al(s)+ Ni2 (aq) > a. write balanced cathode half reaction b. write the balanced anode half reaction C. Write the balanced overall reaction d. Calculate E。, the cell potential. Is the reaction spontaneous as written? e Calculate Eolf [AP ] = 4.00 M, [Ni2+] = 2.00 x 10-5 M.
Question 4 A galvanic cell uses the reaction: 2Ag+(aq) + Ni(s) --> 2Ag(s) + Ni2+(aq) a)...
Question 4 A galvanic cell uses the reaction: 2Ag+(aq) + Ni(s) --> 2Ag(s) + Ni2+(aq) a) calculate the Standard Cell Potential (Ecell) of this galvanic cell and b) which metal is the cathode? a) 1.03 V; b) nickel a) 1.03 V; b) silver oooo a) 0.57 V; b) nickel a) 0.57V; b) silver
The value of Eocell for the cell shown below is +1.41 V. Al(s) | Al3+(aq) ||...
The value of Eocell for the cell shown below is +1.41 V. Al(s) | Al3+(aq) || Ni2+(aq) | Ni(s) The concentration of Al3+(aq) is 0.050 M and the concentration of Ni2+(aq) is 2.0 M. Estimate the value of Ecell at 25 oC. -1.41 V +1.34 V +1.38 V +1.48 V +1.44 V
Calculate the standard cell potential (∆Eo) for the galvanic cell: Ni (s) 1 Ni2+ (aq) II...
Calculate the standard cell potential (∆Eo) for the
galvanic cell:
Ni (s) 1 Ni2+ (aq) II Ag+ (aq) 1 Ag (5) Given: E Half Reaction Ag+ (aq) +e- → Ag (s) Ni2+ (aq) + 2e- → Ni (s) 0.79 Volts -0.23 Volts
A voltaic cell consists of an Al/Al3+ half-cell and an Fe2+/Fe3+ half-cell. Calculate Ecell when conc....
A voltaic cell consists of an Al/Al3+ half-cell and an Fe2+/Fe3+ half-cell. Calculate Ecell when conc. of Fe2+= 0.402 M, Fe3+= 0.073 M and Al3+= 0.239 M. Use the reduction potentials for Al3+ is -1.66 V and for Fe3+ is 0.77 V. How do you decide which is oxi, red.
A voltaic cell consists of an Al/Al3+ half-cell and a Cd/Cd2+ half-cell. Calculate {Cd2+} when {Al3+}...
A voltaic cell consists of an Al/Al3+ half-cell and a Cd/Cd2+ half-cell. Calculate {Cd2+} when {Al3+} = 0.306 M and Ecell = 1.27 V. Use reduction potential values of Al3+ = -1.66 V and for Cd2+ = -0.40 V.
Calculate the standard cell potential and determine if the reaction is spontaneous in the forward direction(as...
Calculate the standard cell potential and determine if the reaction is spontaneous in the forward direction(as written). Identify each oxidizing agent and reducing agent. Ni (s) + Zn2+(aq) ----> Ni2+(aq) + Zn (s) Ni (s) + Pb2+(aq) -------> Ni2+(aq) + Pb (s) Al (s) + 3 Ag+(aq) ---------> Al3+(aq) + Ag (s) Pb (s) + Mn2+(aq) ----------> Pb2+(aq) + Mn (s)
15) Consider a galvanic cell with a Ni electrode in 1.0 M Ni2+(aq) joined by a...
15) Consider a galvanic cell with a Ni electrode in 1.0 M Ni2+(aq) joined by a salt bridge to a silver electrode in 1.0 M Ag+(aq). Calculate the concentrations of Ag+(aq) and Ni2+(aq) once the cell is "dead". Answer: [Ag+] = 4.6 * 10-18 M, [Ni2+] = 1.5 M
Al3 (aq) + Ni(s). 3. Consider the unbalanced reaction Al(s)+ Ni2 (aq) > a. write balanced cathode half reaction b. write the balanced anode half reaction C. Write the balanced overall reaction d. Calculate E。, the cell potential. Is the reaction spontaneous as written? e Calculate Eolf [AP ] = 4.00 M, [Ni2+] = 2.00 x 10-5 M.
Question 4 A galvanic cell uses the reaction: 2Ag+(aq) + Ni(s) --> 2Ag(s) + Ni2+(aq) a) calculate the Standard Cell Potential (Ecell) of this galvanic cell and b) which metal is the cathode? a) 1.03 V; b) nickel a) 1.03 V; b) silver oooo a) 0.57 V; b) nickel a) 0.57V; b) silver
Calculate the standard cell potential (∆Eo) for the
galvanic cell:
Ni (s) 1 Ni2+ (aq) II Ag+ (aq) 1 Ag (5) Given: E Half Reaction Ag+ (aq) +e- → Ag (s) Ni2+ (aq) + 2e- → Ni (s) 0.79 Volts -0.23 Volts
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