An electrochemical cell is constructed such that on one side a pure nickel electrode is in contact with a solution containing Ni2+ ions at a concentration of 5*10-3 M. The other cell half consists of a pure Fe electrode that is immersed in a solution of Fe2+ ions having a concentration of 0.3 M. At what temperature will the potential between the two electrodes be +0.140 V?
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An electrochemical cell is constructed such that on one side a pure nickel electrode is in...
13. (10 marks) One half of an electrochemical cell consists of a pure Ni electrode in a solution conatining Ni2+ ions; the other half is a Cd electrode in a Cd2+ solution. Both cells are at 25 ℃. The two half cells are connected with an electrical wire. (a) Under standard conditions, explain which half cell will be anodic? Write the full electrochemical reaction. (b) If the cell voltage output is measured to be 0.12 V when [Ni2+] = 0.3...
1-One-half of an electrochemical cell consists of a pure Zinc electrode in a solution of Zn2+ ions; the other half is a Lead electrode immersed in a solution of Pb2+ solution. The half-cell potentials for Zinc and Lead are -0.763 V and -0.126 V, respectively. (a) If the cell is a standard one, write the spontaneous overall reaction and calculate the voltage that is generated. (b) Compute the cell potential at 25oC if the Zn2+ and Pb2+ concentrations are 10-2...
a.) A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode (P(H2) = 1 atm) immersed in a solution of unknown [H+]. If the cell potential is 0.204 V, what is the pH of the unknown solution at 298 K? b.) An electrochemical cell is constructed in which a Cr3+(1.00 M)|Cr(s) half-cell is connected to an H3O+(aq)|H2(1 atm) half-cell with unknown H3O+ concentration. The measured cell voltage is 0.366...
A galvanic cell is assembled from one half cell with a nickel electrode immersed in Ni 2+ aqueous solutions in one beaker where [Ni2+] = 1.2 M coupled to a second half cell with a chromium electrode immersed in a Cr3+ aqueous solution to give Ecell = +0.55 V at 25 °C. 3Ni2+(aq) + 2Cr(s) → 3Ni(s) + 2Cr3+(aq) Eϴ cell = +0.50 V Calculate the concentration of the chromium ions [Cr3+] in solution. (A) 1.9 x10^–1 M (B) 6.7...
Consider an electrochemical cell with a zinc electrode immersed in a solution of ZnT and in electrical contact with a silver electrode immersed in a solution of Ag. If the initial concentrations of Zinc and Silver ions are 0.0050 M and 16.00 M respectively, calculate +2 cell Consider an electrochemical cell with a zinc electrode immersed in a solution of ZnT and in electrical contact with a silver electrode immersed in a solution of Ag. If the initial concentrations of...
Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge. a Fe electrode in 1.0 M FeCl2 solution a Sn electrode in 1.0 M Sn(NO3)2 solution Fe2+ + 2e- → Fe Eo = -0.44 V Sn2+ + 2e- → Sn Eo = -0.14 V When the cell is running spontaneously, which choice includes only true statements and no false ones? Select one: a. The iron electrode gains mass and the iron electrode is the...
Electrochemical Measurement of Concentration An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. What is the potential of this cell at 25°C if the copper electrode is placed in a solution in which [Cu2+] = 9.2×10-5 M? 1 pts Tries 0/8 The copper electrode of the above cell is placed in a solution of unknown [Cu2+]. The measured potential at 25°C is 0.160 V. What is [Cu2+] (in mol/L)? (Assume Cu2+ is reduced.) 1 pts...
Electrochemical Measurement of Concentration An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. a) What is the potential of this cell at 25°C if the copper electrode is placed in a solution in which [Cu2+] = 7.5×10-8 M? b) The copper electrode of the above cell is placed in a solution of unknown [Cu2+]. The measured potential at 25°C is 0.109 V. What is [Cu2+] (in mol/L)? (Assume Cu2+ is reduced.) c) A calibration curve...
(a) Compute the voltage at 25˚C of an electrochemical cell consisting of pure cadmium immersed in a 2 × 10-3 M solution of Cd2+ ions and pure iron in a 0.2 M solution of Fe2+ ions. (b)Determine the spontaneous electrochemical reaction for iron (reduced/oxidized) and cadmium (reduced/oxidized).
materials question electrochemistry table has associated voltages compute the voltage at 25c of an electrochemical cell consisting of pure copper immersed in 9x10^-2M solution of Cu^2+ ions and pure nickel in a 0.35 M solution of Ni^2+ ions. half reactions are: Cu-> Cu^2+ + 2e- @+0.345V electrode potential Ni-> Ni^2+ + 2e- @ -2.250V this is all the information I was given We were unable to transcribe this imageWe were unable to transcribe this imageWe were unable to transcribe this...