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
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write oxidation and reduction (anode and cathode) reactions for given redox reactions, Write net equations as...
PART A: REDOX REACTIONS 1. For each of the metals, write the redox equations for reactions you observed in a table as shown below. Write NR for “no reaction” where none was observed. 2+ (**e.g., Cu + Zn → Cu + Zn , Ecell = 1.10 V) Cu(NO3)2 Pb(NO3)2 Zn(NO3)2 16 Cu(s) NR NR Pb(s) NR Zn(s) NR 2. Calculate the Eº for every cell, whether or not a reaction was observed, using equation (5) and values for the standard...
Ecell = 0 - 0.0592/n log(Cu anode/Cu Cathode) Q2. Write and identify the oxidation and reduction half-reactions for the Cu-Cu concentration cell. Combine these to give the overall reaction. Use the Nernst equation to calculate the theoretical value of Ecell and determine the percent error. Show all of your work. (4.0)
Write balanced equations for the following oxidation-reduction reactions. Show your work. a. The oxidation of Zn by MnO4- in an acidic solution to form Zn^2+ and MnO2 b. The oxidation of NO2 by Au^3+ in basic solution to form Au and NO3-
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.
need a little help with number 3 2. Write both cathode and anode reactions for the following cell reactions: Zn(s)[ZnCl2(aq)||Ci-(aq)|C12(1) Cu(s)/Cu(NO3)2(aq)||Fe(NO3)2(aq)|Fe(s) 3. Find Eº, AG, and K for the above reactions.
answer 4 please Laathode - Eanode Remember reduction occurs at the cath For the anode reactions, your rea Llculating these. per reduction occurs at the cathode: oxidation occurs at the anode actions, your reactant will be on the product side of the standard equation, but don't change any sign. The equation does that for you. say 1 Reaction Cathode Reaction Ecole Anode Reaction Ente Spontaneous | Cu+Ag Ag* + e → Ag .7996 Cu → Cu? + 2 . 34...
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
Can someone please tell me if I did the equations right and if the anode and cathode reactions are correct . Report sheet Exp. 11 Electrochemistry Date: Name: Partner's Name: Lab Section Anode Equation for the Cathode Equation for the Cathode Cell Ecell Reaction Anode Reaction oxidahon) Measured Cu-Zn MO Cu-Fe Zn-Mg M9 Fe-Mg Mg 2n
data collected Cu(NO3)2 | Zn(NO3)2 = 0.999 V Pb | 1.0 M Pb(NO3)2 || 1.0 M Zn(NO3)2 | Zn = 0.396 V PART B: REDUCTION POTENTIALS 1. Report the measured cell potential for each galvanic cell and state which electrode corresponds to the cathode and which to the anode. 2. Given E = -0.76 V for the Zn/Zn half-cell, and your measured Ecell, calculate the reduction potential at the Cu and Pb electrodes and write the redox half- 6 reactions...
In a galvanic cell, a spontaneous redox reaction occurs. However the reactants are separated such that the transfer of electrons is forced to occur across a wire. The resulting electricity is measured in volts (V) and is the sum of the potentials of the oxidation and reduction half-reactions: E^o cell = E^o red + E^o ox By reversing the reduction half-reactions, you get the corresponding oxidation half-reaction, for which E^o ox has the opposite sign of E^o red You can...