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.)
A voltaic cell contains two half-cells. One half-cell contains a titanium electrode immersed in a 1.00...
A voltaic cell contains two half-cells. One half-cell contains a zinc electrode immersed in a 1.00 M Zn(NO3)2 solution. The second half-cell contains a titanium electrode immersed in a 1.00 M Ti(NO3)3 solution. Zn2+(aq) + 2 e− → Zn(s) E⁰red = −0.762 V Ti3+(aq) + 3 e− → Ti(s) E⁰red = −1.370 V (a) Using the standard reduction potentials given above, predict the standard cell potential of the voltaic cell. _____ V (b) Write the overall balanced equation for the...
A voltaic cell contains two half-cells. One half-cell contains a chromium electrode immersed in a 1.00 M Cr(NO_3)_3 solution. The second half-cell contains a nickel electrode immersed in a 1.00 M Ni(NO_3)_2 solution. Cr^3+(aq) + 3 e^- rightarrow Cr(s) E_red^degree = 0.744 V Ni^2+(aq) + 2e^- rightarrow Ni(s) E_red^degree = -0.257 V Using the standard reduction potentials given above, predict the standard cell potential of the voltaic cell. Write the overall balanced equation for the voltaic cell. (Include states-of-matter under...
A voltaic cell consists of two half-cells. One half-cell contains a chromium electrode immersed in 1.00 M Cr(NO3)3 solution. The second half-cell contains a nickel electrode immersed in 1.00 M NI(NO3)2 solution. Nickel plates out on the nickel electrode as the voltaic cell runs. The beginning voltage of the cell is +0.487 V at 25°C. The standard electrode potential (standard reduction potential) of chromium at 25°C is -0.744 V. (a) Write a balanced half-reaction equation for the reaction occurring at...
A voltaic cell contains two half-cells. One half-cell contains a gold electrode immersed in a 1.00 M Au(NO3)3 solution. The second half-cell contains a magnesium electrode immersed in a 1.00 M Mg(NO3)2 solution. Au ** (aq) + 3 e Au(s) Ered = +1.498 V Mg2+ (aq) + 2 + Mg(s) Ered = -2.372 V (a) Using the standard reduction potentials given above, predict the standard cell potential of the voltaic cell. (b) Write the overall balanced equation for the voltaic...
A voltaic cell consists of two half-cells. One half-cell contains a chromium electrode immersed in 1.00 M Cr(NO3)3 solution. The second half-cell contains a cobalt electrode immersed in 1.00 M Co(NO3)2 solution. Cobalt plates out on the cobalt electrode as the voltaic cell runs. The beginning voltage of the cell is +0.467 V at 25°C. The standard electrode potential (standard reduction potential) of chromium at 25°C is −0.744 V. (a) Write a balanced half-reaction equation for the reaction occurring at...
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.) 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...
Consider a voltaic (galvanic) cell with the following metal electrodes. Identify which metal is the cathode and which is the anode, and calculate the cell potential. (Use the table of Standard Electrode Potentials.) (a) Ca(II) and Sc(III) Cathode: . Ca(II) Sc(III) Anode: Ca(II) Sc(III) Ecell = 0.0591 x V (b) Pb(II) and In(III) Cathode: . Pb(II) In(III) Anode: Pb(II) In(III) Ecell - (c) Ni(II) and Zr(IV) Cathode: NI(II) Zr(IV) Anode: Ni(II) Zr(IV) Ecell - V Supporting Materials Periodic Table Supplemental...
One half-cell in a voltaic cell is constructed from a silver wire electrode in a AgNO3 solution of unknown concentration. The other half-cell consists of a zinc electrode in a 1.9 M solution of Zn(NO3)2. A potential of 1.48 V is measured for this cell. Use this information to calculate the concentration of Ag (aq). E® Zn/Zn2+ = -0.763 V Eº Ag/Ag+ = 0.7994 V Concentration = Submit Answer Try Another Version 6 item attempts remaining
Consider the voltaic cell and reduction half potentials: Zn(s) | Zn 2+(aq) (0.100 M) || Ni2+(aq) (1.50 M) | Ni(s) Zn 2+ (aq)/Zn (s) E o = - 0.760 V Ni2+ (aq)/Ni (s) E o = - 0.230 V a) Sketch the voltaic cell represented with the above line notation. Label the anode and cathode and indicate the half-reactions occurring at each electrode and the species present in each solution. Also indicate the direction of electron flow (3 marks). b)...