A voltaic cell consists of a CO2(g)|H2C2O4(aq) electrode and a PbI2(s)|Pb(s) electrode. Calculate the value of the equilibrium constant for the cell.
E ○ cell for PbI |Pb 2(s) (s) = -0.365 V
E ○ cell for CO2(g)|H2C2O4(aq) = -0.49 V
A voltaic cell consists of a CO2(g)|H2C2O4(aq) electrode and a PbI2(s)|Pb(s) electrode. Calculate the value of...
Use the Nernst euation and the cell potential for the Pb-PbI2 cell and the known [Pb2+] to calculate the [Pb2+] in equilibrium with PbI2. The measured avgerage cell potential of Pb-PbI2 is 0.084 V the known [Pb2+] is 0.050 M Eo of Pb2+ (aq) + 2 e- --------> Pb(s) is -0.13 V 0.050 M KI Mixed 9 mL of 0.050 M KI with 3 mL of 0.050 M Pb(NO3)2 .
A voltaic cell consists of an Mn/Mn2+ half-cell and a Pb/Pb2+ half-cell. Pb2+(aq) + 2e- → Pb(s) Eo = -0.13V Mn2+(aq) + 2e- →Mn(s) Eo = -1.18V What is the cathode in this voltaic cell? Question options: a. Mn2+(aq) b. Pb(s) c. Pb2+(aq) d. Mn(s)
2. A voltaic cell consists of Pb/Pb2 and Al Al half-cells 9 points Pb Al' + 2 e + 3 Pb Al Ered = -0.126 V Ered = -1.662 V Write out the balanced reaction for the cell and calculate the standard cell potential, Ecall On the diagram below, label the anode, the cathode, the direction of electron flow Also indicate at which electrode the oxidation occurs and which electrode the reduction occurs m ayar yar salt bridge
A voltaic cell consists of an Mn/Mn2+ half-cell and a Pb/Pb2+ half-cell. Pb2+(aq) + 2e- → Pb(s) Eo = -0.13V Mn2+(aq) + 2e- →Mn(s) Eo = -1.18V What is the anode half-reaction for this voltaic cell? Question options: a. Mn2+(aq) + 2e- →Mn(s) b. Pb(s) → Pb2+(aq) + 2e- c. Pb2+(aq) + 2e- → Pb(s) d. Mn(s) →Mn2+(aq) + 2e-
1. A voltaic cell is constructed that is based on the following reaction: Sn2+(aq)+Pb(s)→Sn(s)+Pb2+(aq). A. If the concentration of Sn2+ in the cathode compartment is 1.30 M and the cell generates an emf of 0.25 V , what is the concentration of Pb2+ in the anode compartment? B. If the anode compartment contains [SO2−4]= 1.30 M in equilibrium with PbSO4(s), what is the Ksp of PbSO4? 2. A voltaic cell utilizes the following reaction: 2Fe3+(aq)+H2(g)→2Fe2+(aq)+2H+(aq). A. What is the emf...
A voltaic cell consists of an Mn/Mn2+ half-cell and a Pb/Pb2+ half-cell. Pb2+(aq) + 2e- → Pb(s) Eo = -0.13V Mn2+(aq) + 2e- →Mn(s) Eo = -1.18V What is the cell voltage of this voltaic cell? Question options: a. -1.31V b. +1.67V c. +1.05V
Design a voltaic cell with the following two reduction half-reactions: Ag+(aq) + e− ⟶ Ag(s) Eo = 0.80 V Pb2+(aq) + 2 e− ⟶ Pb(s) Eo = −0.13 V Calculate Eocell and the equilibrium constant K for the voltaic cell at 298 K. Click here for a copy of Final Exam cover sheet.
a concentration cell was made by putting 5 mL of 0.050 M Pb(NO3)2 solution into one half-cell in a test plate. for the neighboring well in the test plate, weplaced 5 mL of a PbI2 solution that was made by mixing 9 mL of 0.050 KI solution with 3 mL of 0.050 M Pb(NO3)2 solution inside. Pb Electrodes were placed in eachcell, and a KNO3-soaked string was used as the salt bridge.data was collected and we recorded the average cell...
A voltaic cell is based on two lead half cells: Pb+2(aq) + 2 e- → Pb(s) Eo = -0.13 v One half-cell has [Pb(NO3)2] = 0.25 M and one half-cell has [Pb(NO3)2] = 0.0020 M What is the initial potential produced by the voltaic cell. Express your answer in units of volts with 2 significant digits, but do not include the units on the submitted answer.
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)...