Question

In: Chemistry

Find the standard reduction potentials (voltages) expected for the following half reactions Cu+2 + 2e- ------------->...

Find the standard reduction potentials (voltages) expected for the following half reactions

Cu+2 + 2e- -------------> Cu

Pb+2 + 2 e- ------------> Pb

Zn+2 + 2 e- -------------> Zn

Fe+3 + e- ---------------> Fe+2

Br2 + 2e- --------------> 2Br-

Calculate expected voltages for the electrochemical cells made by connecting the copper(II) half reaction to each of the others in the list above. Note that one of the listed reductions must be reversed to become an oxidation for anything tooccur and that when a half rxn is reversed, the sign of its potential is reversed. For the voltage to be a positive number ( indicating a spontaneous reaction), Which half rxn will be the cathode in each pairing?

an example: Ag+  + e- -----------> Ag E0  = +.79v

Cl2   + 2e-  ------------> 2Cl-   E0  = + 1.36v

For a Ecell >0, silver half rxn must be reversed to become an oxidation: Ag -----------> Ag+   + e-   E0 = -.79

overall rxn is 2 Ag + Cl2 -------------> 2 Ag+   + 2Cl-   Ecell = -.79 + 1.36 = + .57v (Cl2 electrode is cathode)

(Note that you don't have to balance the reaction to figure out the Ecell : tabulated E0 reduction tables are for 1 mol of electrons transferred for all the half reactions, so you don't double the E0 number for silver to use it with the E0 for Cl2.)

Solutions

Expert Solution

queen_honey_blossom answered 2 years ago
Next > < Previous

Related Solutions

Assuming standard conditions, and considering the table of standard reduction potentials for half-reactions, given in your...
Assuming standard conditions, and considering the table of standard reduction potentials for half-reactions, given in your text, rank the following species according to their relative strength as reducing agents. For example, the most powerful reducing agent would be given rank "1", and the least "6". Cd Mn H2 (acidic half-cell solution) Na Cl- ClO2-
Standard reduction potentials are provided for two half reactions that involve the hypothetical metal "M" and...
Standard reduction potentials are provided for two half reactions that involve the hypothetical metal "M" and sulfide ion. Use them to calculate the value of the solubility product constant for the metal sulfide. (Hint: what is the balanced chemical reaction equation for the equilibrium reaction that gives Ksp?) M2+ + 2 e- ⇌ M(s) Eo = -0.057 V MS(s) + 2 e- ⇌ M(s) + S2- Eo = -1.208 V Ksp of MS(s) =
Consider a galvanic cell based upon the following half reactions: Cu2+ + 2e- → Cu 0.34...
Consider a galvanic cell based upon the following half reactions: Cu2+ + 2e- → Cu 0.34 V Fe3+ + 3e- → Fe -0.0036 V How many of the following responses are true? 1. Decreasing the concentration of Cu2+ (assuming no volume change) will decrease the potential of the cell 2. Increasing the concentration of Fe3+ (assuming no volume change) will increase the potential of the cell 3. Adding equal amounts of water to both half reaction vessels will increase the...
Explain why the sum of the potentials for the half-reactions Sn2+(aq) + 2e− → Sn(s) and...
Explain why the sum of the potentials for the half-reactions Sn2+(aq) + 2e− → Sn(s) and Sn4+(aq) + 2e− → Sn2+(aq) does not equal the potential for the reaction Sn4+(aq) + 4e−→ Sn(s). What is the net cell potential? Compare the values of ΔG° for the sum of the potentials and the actual net cell potential.
Problem A) The standard reduction potentials for the following reactions are given below. Pyruvate + 2H+...
Problem A) The standard reduction potentials for the following reactions are given below. Pyruvate + 2H+ + 2e- → Lactate E∘ = -0.190 V NAD+ + 2H+ + 2e- → NADH/H+ E∘ = -0.320V. Calculate △G∘ for the overall spontaneous reaction making use of the relationship between △E∘ and △G∘. Problem B) Calculate the △G∘ʹ for the reaction given the equilibrium constant is 1.97 and the physiological relevant temperature is 37 ∘C. fructose-6-phosphate → glucose-6-phosphate Problem C) Calculate the ratio...
Use the standard reduction potentials to calculate the equilibrium constant for each of the following reactions:...
Use the standard reduction potentials to calculate the equilibrium constant for each of the following reactions: Note if deltaG° for each reaction would be greater than or less than zero. Co2+(aq) + Sn(s) = Co(s) + Sn2+(aq) Ag+(aq) + Cr2+(aq) = Ag(s) + Cr3+(aq)
Refer to this table of reduction potentials to answer the questions. Reduction half-reaction Potential (V) F2(g)+2e−→2F−(aq)...
Refer to this table of reduction potentials to answer the questions. Reduction half-reaction Potential (V) F2(g)+2e−→2F−(aq) +2.87 O2(g)+4H+(aq)+4e−→2H2O(l) +1.23 Br2(l)+2e−→2Br−(aq) +1.07 Ag++e−→Ag(s) +0.80 2H2O(l)+2e−→H2(g)+2OH−(aq) −0.83 Na+(aq)+e−→Na(s) −2.71 What is produced at each electrode in the electrolysis of an aqueous solution of both NaBr and AgF? H2(g), Ag(s), Na(s), O2(g), Br(l), F2(g) sort to respective designation below Anode, Cathode, Not produced
Refer to this table of reduction potentials to answer the questions. Reduction half-reaction Potential (V) F2(g)+2e−→2F−(aq)...
Refer to this table of reduction potentials to answer the questions. Reduction half-reaction Potential (V) F2(g)+2e−→2F−(aq) +2.87 O2(g)+4H+(aq)+4e−→2H2O(l) +1.23 Br2(l)+2e−→2Br−(aq) +1.07 Ag++e−→Ag(s) +0.80 2H2O(l)+2e−→H2(g)+2OH−(aq) −0.83 Na+(aq)+e−→Na(s) −2.71 What is produced at each electrode in the electrolysis of an aqueous solution of both NaBr and AgF? Drag the appropriate items to their respective bins. Na(s) H2(g) F2(g) O2(g) Ag(s) Br2(l)
Given the following standard reduction potentials: Pb2+ (aq) +2e- ---> Pb (s) E= -.126V PbSO4(s) +...
Given the following standard reduction potentials: Pb2+ (aq) +2e- ---> Pb (s) E= -.126V PbSO4(s) + 2e- ---> Pb(s) + SO42- (aq) E= -.356V Determine the Ksp for PbSO4(s) at 25 degrees C
Ascorbate and Cu ions have the following electrochemical potentials; Dehydroascorbate + 2H+ + 2e- --> Ascorbate...
Ascorbate and Cu ions have the following electrochemical potentials; Dehydroascorbate + 2H+ + 2e- --> Ascorbate Eo' = +0.08V Cu2+ + e- --> Cu+ Eo' = 0.159 V 10 mL of a 0.02M solution of ascorbate in a buffered solution at pH 7.0; 25 degrees Celsius is mixed with 10mL of 0.02 M of Cu2+. Write a balanced chemical equation for the reaction, and figure out the equilibrium concentration of dehydroascorbate, ascorbate, Cu2+, and Cu+.
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT