Ecell = 0 - 0.0592/n log(Cu anode/Cu Cathode)
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Ecell = 0 - 0.0592/n log(Cu anode/Cu Cathode) Q2. Write and identify the oxidation and reduction...
Ksp =[ Pb^+2][I^-]^2 Ecell = 0 - 0.0592/2 log(Pb^2+ Anode/Pb^2+ Cathode) Q3. Write and identify the oxidation and reduction half-reactions for the Pb-Pb concentration cell. Combine these to give the overall reaction equation. Use the Nernst equation to calculate [Pb2+] in the saturated Pbl2 solution and then calculate Ksp for Pbl2. Show all your work. (5.0)
1. Fill in the blanks. Identify Half-Reactions Identify Reaction in Half Reaction (Oxidation or Reduction) Cathode or Anode Cr2O72- + 14 H+ + 66 - 2 Cr + 7 H20 I Reduction Cathode [ Fet – Fet the xle Oxidation | Anode Give the balanced, overall redox equation between these half-reactions. 6fe tcr. O, 2- +14 tt lefest & zerst +7H.O
Galvanic Measured Cell Equation for Anode Equation for Cathode Ecell Anode Reaction Cathode Reaction Cu-Zn @jcu-Mg M010 LL Sof Mane t Mu ?. (imus -ur.- 3) Cu-Fe Zn-M 5) Fe-Mg ?) Zn-Fe -A Write balanced equations for the six cell reactions 2 + Compare the sum of the Zn-Mg and Cu-Zn cell potentials with the Cu-Mg cell potential. Explain your result. Compare the sum of the Zn-Fe and Zn-Mg cell potentials with the Fe-Mg cell potential. Explain your result.
Equation 18: (didnt mean to attach equation 15 oops) V-13 EXPERIMENT V: VOLTAIC CELLS, AND THE NERNST EQUATION PRELAB ASSIGNMENT (CONTINUED) 5. In aqueous solution Cu* ions are more stable than Cu ions because 2 Cu* (aq) + Cu2+ (aq) + Cu (s) (a) Give an oxidation half-cell reaction and a reduction half-cell reaction that can be combined to form this overall reaction. (0.5 marks) (b) Use Eq. 18 with your answer to (a) to calculate the theoretical K for...
Balance the following oxidation-reduction reactions using the half-reaction method. 1. HCOOH (aq) + MnO.. (aq) → CO2 (g) + Mn2. Acidie solution Identify the reduction half Identify the oxidation half Basic solution Identify the reduction half Identify the oxidation half Write a balanced equation for the electrode and overall cell reactions in the following galvanic cell and determine E°. Sketch the cell, labeling the anode and cathode and showing the direction of electron and ion flow. 2. 3. Circle the...
1. We will be building a Cu? and Zn galvanic cell. Write the two half reactions (one as a reduction and one as an oxidation based on forming a spontaneous reaction) and write the combined reaction. (Similar to equations 9.3-9.5 but for our system specifically). (3 pts) In the galvanic cell we are building in class, which is the anode and which is the cathode? (2 pts) 2. Calculate Ecel for our voltaic cell. (Use Table 16.1 in your OpenStax...
write oxidation and reduction (anode and cathode) reactions for given redox reactions, Write net equations as well: .1 M Cu(No3)2 added into Copper Magnesium Zinc .1 M Mg(No3)2 added into Copper Magnesium Zinc .1 M Zn(No3)2 added into Copper Magnesium Zinc Show all work please, Thank you
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):...
5. In aqueous solution Cuions are more stable than Cu ions because 2 Cu" (aq) + Cu (aq) + Cu(s) (a) Give an oxidation hall-cell reaction and a reduction half-cell reaction that can be combined to form this overall reaction. (0.5 marks) (b) Use Eq. 18 with your answer to (a) to calculate the theoretical K for the reaction. (1 mark) 6. Refer to Fig. 1. The salt bridge is to prevent wholesale mixing of the two solutions. Assume that...
A voltaic cell is based on the reduction of Ag^+(aq) to Ag(s) and the oxidation of Sn(s) to Sn^2+(aq). (a) Write half-reactions for the cell's anode and cathode. Include the phases of all species in the chemical equation. Anode Cathode (b) Write a balanced cell reaction. Include the phases of all species in the chemical equation.