4. Determine the cell voltage of a concentration cell with Cr(s) in 0.000500 M Cr(aq) at one electrode and Cr(s) in 2.0 M Cr (aq) at the other electrode. Which concentration is at the cathode? (8...
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...
salt bridge ME Cr(s) electrode Cu(s) electrode 1.0 M Cr3+ (aq) 1.0 M Cu2+ (aq) A electrolytic cell similar to that shown in the figure above is constructed. The electronic device shown at the top of the figure is a power supply. One electrode compartment consists of a chromium strip placed in a 1.0 M CrCl3 solution, and the other has a copper strip placed in a 1.0 M CuSO4 solution. The overall cell reaction is: 2 Cr3+ (aq) +...
9) A galvanic cell Cr(s)|Cr2+(aq) || Pb2+(aq)|Pb(s) is constructed using a completely immersed Cr electrode that weighs 26.5 g and a Pb electrode immersed in 665 mL of 1.00 M Pb2+(aq) solution. A steady current of 0.0598 A is drawn from the cell as the electrons move from the Cr electrode to the Pb electrode. (a) Which reactant is the limiting reactant in this cell? ___ (b) How long does it take for the cell to be completely discharged? ___...
A galvanic cell Cr(s) Cr Taq) Co "(aq) Co(s) s constructed using a completely immersed Cr electrode that weighs 32.8 g and a Co electrode mmersed in 454 mL of 1.00 M Co2*(aq) solution. A steady current of 0.0768 A is drawn from the cell as the electrons move from the Cr electrode to the Co electrode. Enter symbol (b) How long does it take for the cell to be completely discharged? (c) How much mass has the Co electrode...
A galvanic cell Cr(s)/Cr2+(aq) || Sna+(aq)|Sn(s) is constructed using a completely immersed Cr electrode that weighs 35.5 g and a Sn electrode immersed in 535 mL of 1.00 M Sn2+(aq) solution. A steady current of 0.0692 A is drawn from the cell as the electrons move from the Cr electrode to the Sn electrode. (a) Which reactant is the limiting reactant in this cell? Enter symbol (b) How long does it take for the cell to be completely discharged? (c)...
A galvanic cell Cr(s)|Cr2+(aq) || Cu2+(aq)|Cu(s) is constructed using a completely immersed Cr electrode that weighs 35.4 g and a Cu electrode immersed in 462 mL of 1.00 M Cu2+(aq) solution. A steady current of 0.0795 A is drawn from the cell as the electrons move from the Cr electrode to the Cu electrode. (a) Which reactant is the limiting reactant in this cell? Enter symbol (b) How long does it take for the cell to be completely discharged? s...
4. If the half reaction s (aq)+ e 3(aq) occurs at the carbon counter electrode, is this electrode acting as the anode or cathode in the solar cell? 4. If the half reaction s (aq)+ e 3(aq) occurs at the carbon counter electrode, is this electrode acting as the anode or cathode in the solar cell?
Consider a galvanic cell where one compartment has Br2 (aq) at a concentration of 0.50 M and Br ̄ at a concentration of 0.10 M with a platinum electrode and the second compartment has Cr3+ at a concentration of 0.20 M and a Cr electrode. Use the following reduction potentials to answer the questions: Cr3+ (aq) + e ̄→Cr(s) εo = - 0.73 V Br2(aq) + 2e ̄→2Br ̄ (aq) εo =1.09V a. What is the standard cell potential for...
A concentration cell is constructed in which the concentrations differ in the two half-cells. The cell consists of a Cr3+ (aq, 0.640 M)Cr(s) half- cell connected to a Cr**(aq, 4.50x10M )Cr(s) half-cell. Determine which half-cell will be the anode compartment and calculate the cell voltage. The Cr3+concentration in the anode compartment will be: (_ A a. 0.640 M b. 4.50x10-3M Ecell =
A galvanic cell is built at 25 ºC using a Cr electrode inside a 2.0 M Cr3+ solution (100 mL) and a Ni electrode inside a 0.5 M Ni2+ solution (100 mL). Both solutions are connected with a salt bridge. a) (0.5 p) Write the cell notation and the global redox reaction. Indicate the anode and the cathode of the cell. Determine the cell potential with the given concentrations. b) (0.5 p) Determine how many of the previous cells must...