b. Write the cell notation for the following redox reaction. Here, Cu+ or CuNO3 is oxidized to Cu2+ or Cu(NO3)2in the oxidation half-cell. Since there is only aqueous species and there is no electrode (metal) in the oxidation half-cell, use platinum (Pt) as an inert electrode in the oxidation half-cell.
3CuNO3(aq) + Au(NO3)3(aq) ⟶ 3Cu(NO3)2(aq) + Au(s)
b. Write the cell notation for the following redox reaction. Here, Cu+ or CuNO3 is oxidized...
Write the cell notation for an electrochemical cell consisting of an anode where Cr2+(aq) is oxidized to Cr3+(aq) at a platinum electrode and a cathode where Co2+(aq) is reduced to Co(s). Assume all aqueous solutions have a concentration of 1 mol/L and gases have a pressure of 1 bar.
Write the cell notation for an electrochemical cell consisting of an anode where Cr2+(aq) is oxidized to Cr3+(aq) at a platinum electrode and a cathode where Cd2+(aq) is reduced to Cd (s) . Assume all aqueous solutions have a concentration of 1 mol/L and gases have a pressure of 1 bar.
Balance the redox reaction below using the half-reaction method. NbH(aq) + Mn(s) —+ND(8) + Mn2+ (aq) (a) To show your method, write the balanced half reactions below. Use the smallest integer coefficients possible and show electrons as e'. If a box is not needed, leave it blank. (Coefficients of I are not needed). Oxidation half-reaction: Reduction half-reaction: (b) To show your balanced equation, enter an integer in each of the boxes. If the integer is "1," do enter it even...
A) Write the cell notation for an electrochemical cell consisting of an anode where Mg (s) is oxidized to Mg2+(aq) and a cathode where Fe3+(aq) is reduced to Fe2+(aq) at a platinum electrode . Assume all aqueous solutions have a concentration of 1 mol/L. B) Write the cell notation for an electrochemical cell consisting of an anode where Mn (s) is oxidized to Mn2+(aq) and a cathode where Cr3+(aq) is reduced to Cr2+(aq) at a platinum electrode . Assume all...
In a particular redox reaction, NO2- is oxidized to NO3- and Cu2+ is reduced to Cu+. Complete and balance the equation for this reaction in acidic solution. Phases are optional. What is the balanced redox reaction? Can you elaborate why the answer is not " NO2- + Cu2+ + H2O ---> NO3- + Cu+ + 2H+ "
help with these please Write the cell notation for an electrochemical cell consisting of an anode where Al () is oxidized to AP+ (aq) and a cathode where Pb2+ (aq) is reduced to Pb (s). Assume all aqueous solutions have a concentration of 1 mol/L. Write the cell notation for an electrochemical cell consisting of an anode where Sn (s) is oxidized to Sn2+ (aq) and a cathode where H(aq) is reduced to H2 (g) at a platinum electrode. Assume...
In a particular redox reaction, NO2– is oxidized to NO3– and Cu2 is reduced to Cu . Complete and balance the equation for this reaction in acidic solution.
A) Write the cell notation for an electrochemical cell consisting of an anode where Mn (s) is oxidized to Mn2+(aq) and a cathode where Cd2+(aq) is reduced to Cd (s) . Assume all aqueous solutions have a concentration of 1 mol/L. B) Write the cell notation for an electrochemical cell consisting of an anode where Zn (s) is oxidized to Zn2+(aq) and a cathode where H+(aq) is reduced to H2(g) at a platinum electrode . Assume all aqueous solutions have...
In a particular redox reaction, NO2- is oxidized to NO3- and Cu2+ is reduced to Cu+. Complete and balance the equation for this reaction in acidic solution. Phases are optional.
Question 9 What is the cell notation for a voltaic cell that incorporates the following redox reaction? Cu2+ (aq) + Sn (s) Sn2+ (aq) + Cu(s) O a. Sn (s) | Sn2+ (aq) || Cu (8) | Cu2+ (aq) O b. Sn (s) | Sn2+ (aq) || Cu2+ (aq) | Cu (8) OC. Cu(s) | Cu2+ (aq) || Sn (s) | Sn2+ (aq) Od. Cu2+ (aq)|Cu () || Sn2+ (aq) | Sn (8) O e. Cu (s) | Cu2+ (aq)...