Question

If the standard reduction potential of a certain half-reaction is -0.30 V, which statement below is...

If the standard reduction potential of a certain half-reaction is -0.30 V, which statement below is true for this half-reaction to proceed as a reduction?

A) This half-reaction will proceed if it is coupled to another half-reaction that has a standard reduction potential greater than +0.30 V.

B) This half-reaction will proceed if it is coupled to another half-reaction that has a standard reduction potential greater than -0.30 V.

C) This half-reaction will proceed if it is coupled to another half-reaction that has a standard reduction potential less than -0.30 V.

D) It doesn't matter what half-reaction this is coupled with, it will proceed spontaneously.

Homework Answers

Answer #1

If Standard Reduction potential is lower it will undergo oxidation reaction and if Standard Reduction potential is higher it will undergo Reduction reaction.

Simply we can justify two half coupled reaction will follow Oxidation - Reduction reaction or not.

Between two half reactions, one follows Oxidation when SRP is lower and another had reaction follows Reduction when SRP is higher.

The given half reaction SRP is -0.30 V it should proceed as Reduction

so another half reaction SRP should be lesser than -0.30 V then it will undergo Oxidation

Therefore the answer will be Option ( C )

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The standard-state reduction potential for Cu2+ to Cu is +0.342 V versus the SHE. Given that...
The standard-state reduction potential for Cu2+ to Cu is +0.342 V versus the SHE. Given that Cu2+ forms a very stable complex with the ligand EDTA, do you expect the standard-state reduction potential for Cu(EDTA)2– to be greater than +0.342 V, less than +0.342 V, or equal to +0.342 V? Explain your reasoning.
Short Answer 1) Reduction half-reactions with corresponding standard half-cell potentials are shown below. Zn2+(aq) + 2...
Short Answer 1) Reduction half-reactions with corresponding standard half-cell potentials are shown below. Zn2+(aq) + 2 e‐ → Zn(s) E° = ‐ 0.76 V Al3+(aq) + 3 e‐ → Al(s) E° = ‐ 1.66 V The standard potential for the galvanic cell that uses these two half-reactions is ________ V. 2)In the galvanic cell represented by the shorthand notation shown below, Cd(aq)|Cd2+(aq)|| I2(g)|I-(aq)|Pt(s) the inert electrode is ________, and the balanced cathode half-reaction reaction is ________.
Use the standard reduction potentials shown here to answer the questions. Reduction half-reaction E∘ (V) Cu2+(aq)+2e−→Cu(s)...
Use the standard reduction potentials shown here to answer the questions. Reduction half-reaction E∘ (V) Cu2+(aq)+2e−→Cu(s) 0.337 2H+(aq)+2e−→H2(g) 0.000 A copper, Cu(s), electrode is immersed in a solution that is 1.00 M in ammonia, NH3, and 1.00 M in tetraamminecopper(II), [Cu(NH3)4]2+. If a standard hydrogen electrode is used as the cathode, the cell potential, Ecell, is found to be 0.073 V at 298 K. Part A Based on the cell potential, what is the concentration of Cu2+ in this solution?...
Which of the following statement is not true. a. an endothermic reaction has an early transition...
Which of the following statement is not true. a. an endothermic reaction has an early transition state. b. the transition state of an exothermic reaction resembles reactants. c. the activation energy of the forward reaction of an exothermic reaction is less than the activation energy of its reverse reaction. d. an endothermic reaction requires energy to proceed in the forward direction.
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Cl2(g)+2e−→...
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Cl2(g)+2e−→ 2Cl−(aq)   E0red = +1.359V NO−3(aq)+4H+(aq)+3e−→ NO(g)+2H2O(l)   E0red = +0.96V Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode.   Write a balanced equation for the half-reaction that happens at the anode.   Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.   Do you have enough...
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential N2(g)+4H2O(l)+4e−→...
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential N2(g)+4H2O(l)+4e−→ N2H4(aq)+4OH−(aq) E0red = −1.16V Zn+2(aq)+2e−→ Zn(s) E0red = −0.763V Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode.   Write a balanced equation for the half-reaction that happens at the anode.   Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.   Do you have enough...
Choose all of the statements from below which are true about oxidation and reduction. A. Oxidation...
Choose all of the statements from below which are true about oxidation and reduction. A. Oxidation and reduction are opposite processes with respect to bookkeeping electrons. B. Oxidation is what happens when an element in a substance gains electrons. C. Electrons appear on the right side of an oxidation half reaction. D. An oxidant is an oxidizing agent, which becomes oxidized during the course of a redox reaction. E. Reduction is what happens when an element in a substance decreases...
1. The standard reduction potential for the reduction of Eu3+(aq) to Eu2+(aq) is -0.43 V. Using...
1. The standard reduction potential for the reduction of Eu3+(aq) to Eu2+(aq) is -0.43 V. Using Appendix E in the textbook, which of the following substances is capable of reducing Eu3+(aq) to Eu2+(aq) under standard conditions? a. Al B. Co C. H2O D. N2H5 E. H2C2O4 2. How many minutes will it take to plate out 4.56 g of Ni metal from a solution of Ni2+ using a current of 40.5 amps in an electrolytic cell? 3. Using the standard...
The process of corrosion can be viewed as an electrochemical cell with cathodic reactions such as:...
The process of corrosion can be viewed as an electrochemical cell with cathodic reactions such as: O2+2H2O+4e−⟶4OH− at +1.229 V H++e−⟶1/2H2(g) at 0 V M2++2e−⟶M(s) Where M is a metal. If this is the case, and we assume iron serves as the anode, Fe0(s)⟶Fe+2(aq)+2e− at −0.447 V what must be true of the cathode reactions for corrosion to occur? a. The standard reduction potential of the cathode must be less than 0 V. b.  The standard reduction potential of the cathode...
Balance the following oxidation-reduction reactions, which occur in acidic solution, using the half-reaction method. (Use the...
Balance the following oxidation-reduction reactions, which occur in acidic solution, using the half-reaction method. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.) (a) O2(g) + Pb(s) → H2O(l) + Pb2+(aq) (b) NO3−(aq) + Sn(s) → NO(g) + Sn2+(aq) (c) Cl2(g) + Cr3+(aq) → Cl −(aq) + Cr2O72−(aq) (d) F2(g) + Mn2+(aq) → F −(aq) + MnO4−(aq)