What is the standard cell potential of a cell created using a cadmium electrode in 0.45...
In the following cell, A is a standard Ni2+1 Ni electrode connected to a standard hydrogen electrode. For this cell the voltmeter reading is -0.23 V. What is the chemical equation for the cell reaction? Given: Standard reduction potential of the H+/H2 and Ni2+/Ni couples are 0.00 and -0.23 V, respectively. voltmeter saltbridge PLS) PAH2 (g) O Ni(s) + 2H+(aq) --> Ni2+(aq) + H2(g) O Ni2+(aq) + H2(g) --> Ni(s) + 2H+(aq)
Question 11 of 16 > A galvanic (voltaic) cell consists of an electrode composed of cadmium in a 1.0 M cadmium ion solution and a second electrode composed of cobalt in a 1.0 M cobalt(II) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Use this list of standard reduction potentials. V Ecel =
use tabulated standard electrode potential to calculate the standard cell potential for the reaction occurring in an electrochemical cell at 25 C. (The equation is balanced.) 3Ni^2+(aq)+2Cr(s)--->3Ni(s)2Cr^3+(aq) Express your answer to two significant figures and include the appropriate units. em 26 E (V) -0.45 -0.50 -0.73 -0.76 -1.18 Standard reduction half-cell potentials at 25°C Half-reaction E° (V) Half-reaction Aul+ (aq) + 3e +Au(s) 1.50 Fe2+ (aq) + 2eFe(s) Ag+ (aq) +e-Ag(s) 0.80 Cr3+ (aq) + Cr²+ (aq) Fe+(aq) + 3e...
For the cell Ni(s) Ni2+(aq) || Ag+(aq) Ag(s), the standard cell potential is 1.03 V. A cell using these reagents was made, and the observed potential was 0.80 V at 25°C. What is a possible explanation for the observed voltage? The volume of the Agt solution was larger than the volume of the Ni2+ solution. The Agt concentration was larger than the Ni2+ concentration. The Ag electrode was twice as large as the Ni electrode. The Ni2+ concentration was larger...
A voltaic cell contains two half-cells. One half-cell contains a titanium electrode immersed in a 1.00 M Ti(NO3)3 solution. The second half-cell contains a nickel electrode immersed in a 1.00 M Ni(NO3)2 solution. Ti3+(aq) + 3 e− → Ti(s) E⁰red = −1.370 V Ni2+(aq) + 2 e− → Ni(s) E⁰red = −0.257 V Write the overall balanced equation for the voltaic cell. (Include states-of-matter under the given conditions in your answer.)
If the standard potential of a cell where the following reaction occurs is -0.12V, what would the standard potential of the Pb electrode be if the Ni electrode is 0.25V? Pb(s) + Ni2+(aq) --> Pb2+(aq) + Ni(s)
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...
My Notes 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 copper strip placed in a 1.0 M CuSO4 solution, and the other has a cadmium strip placed in a 1.0 M Cd(NO3)2 solution. The overall cell reaction is: Cd2+(aq) + Cu(s) Cd(s) + Cu2+(aq) (a) Fill in the information necessary to complete the half reactions...
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...
A voltaic cell similar to that shown in the figure above is constructed. The electronic device shown at the top of the figure is a volt meter. One electrode compartment consists of a cadmium strip placed in a 1.0 M Ca(NO3), solution, and the other has a copper strip placed in a 1.0 M CUSO4 solution. The overall cell reaction is: Ca(s) + Cu2+ (aq) = Cd2+(aq) + Cu(s) (a) Fill in the information necessary to complete the half reactions...