What additions must you make to the cell for it to generate a standard emf?
Check all that apply.
What additions must you make to the cell for it to generate a standard emf?
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
manganese strip placed in a 1.0 M Mn(NO3)2
solution, and the other has a cobalt strip placed in a 0.5 M
Co2(SO4)3 solution. The overall
cell reaction is:
3 Mn2+(aq) + 2 Co(s) 3 Mn(s) + 2 Co3+(aq)
(a) Fill in the information necessary to complete the...
What is the standard cell potential of a cell created using a cadmium electrode in 0.45 M Cd(NO3)2(aq) and a graphite electrode in an aqueous solution that is 0.45 M in both Fe2+ and Fe3+? 0.38 V 1.95 V 1.94 V 1.17 V 1.18 V What is the standard cell potential of a cell which utilizes the following reaction: Zn (s) + Ni2+ (aq) → Ni (s) + Zn2+ (aq) All solutions are 1.0 M and the reaction occurs at...
6. Consider the following galvanic cell and standard reduction potentials: Ag Pb E° = 0.80 V salt bridge Ag+ (aq) + e → Ag(s) Pb2+(aq) + 2e → Pb(s) E° = -0.13 V 1 M Ag+ 1 M Pb2+ Which one of the following statements is TRUE? a) The cell on the left containing Ag+(aq) is the anode. b) The initial reading on the voltmeter would be 0.67 V. c) Oxidation occurs in the cell on the right containing Pb²+(aq)....
In this lab, we will explore how different voltaic cells work. 1. Prepare a voltaic cell by placing the magnesium electrode and solution on the left, and the zinc electrode and solution on the right. Place the salt bridge between the two solutions. What is the voltage on this battery? 1.62v 2. Use the magnifying glass to look closely at the magnesium electrode and solution. a) What is happening at this electrode? Mg 2+ b) Write a half reaction showing...
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...
salt bridge Zn(s) electrode Culs) electrode 1.0M Zn (a 1.0 M Cu (aq 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 zinc strip placed in a 1.0 M ZnCl2 solution, and the other has a copper strip placed in a 1.0 M CuSOA solution. The overall cell reaction is: Zn(s)Cu2+(aq)= zn2+ (aq ) Cu (s)...
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...
First fill in your half cell and cell reactions. F in standard cell potentials as you calculate them. Oxidation at the Anode: The black (.) lead is attached to the electrode, which is the source of electrons. Write the anode half reaction: Reduction at the Cathode: The red lead (+) is attached to the electrode. Write the cathode half reaction: E degree - V. Overall Cell Reaction (Net Ionic equation): Write the overall cell reaction (balance electrons and add together):...
Please use the following to answer the below: A fictional galvanic (voltaic) cell consists of an electrode composed of a metal, M, in a 1.0 mol/L M2+ ion solution and a second electrode composed of an unreactive platinum metal (Pt) in a 1.0 mol/L X– ion solution, connected by a salt bridge and an external wire at 25.0 ⁰C. Consider the two entries below from a fictional table of standard reduction potentials. Reduction Equation Standard reduction potentials (E⁰reduction) M2+ (aq)...
Please explain what you do and why.
A galvanic cell is setup with the following two half-cells: A 250.0 mL solution of 0.15 M aluminum nitrate with a platinum electrode. A 250.0 mL solution of 0.85 M cobalt(II) nitrate with a cobalt electrode. a) Determine the cell potential that will be initially measured for this galvanic cell b) How much mass is gained/lost by the cobalt electrode after the cell reaches equilibrium? c) If it takes this galvanic cell 2.00...