Consider only the species (at standard conditions), in answering the following questions. Give reasonfor your answers. (Use data from the Standard Reduction Potential table)Br¯,Br2, H*, H2, La3+, Ca and Cda. Which is the strongest oxidizing agent?b. Which is the strongest reducing agent?c. Which species can be oxidized by MnOs in acid?d. Which species can be reduced by Zn(s)?

Answered: Image /qna-images/answer/eb4560d0-e68d-44d9-8a33-7874be4a62df.jpg

Consider only the species (at standard conditions), in answering the following questions. Give reason for your answers. (Use data from the Standard Reduction Potential table) Br",Br2, H*, H2, La³+, Ca and Cd a. Which is the strongest oxidizing agent? b. Which is the strongest reducing agent? c. Which species can be oxidized by MnO4 in acid? d. Which species can be reduced by Zn(s)?

Consider only the species (at standard conditions), in answering the following questions. Give reason for your answers. (Use data from the Standard Reduction Potential table) Br",Br2, H*, H2, La³+, Ca and Cd a. Which is the strongest oxidizing agent? b. Which is the strongest reducing agent? c. Which species can be oxidized by MnO4 in acid? d. Which species can be reduced by Zn(s)?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Questions attached
plz explain step by step in detail :)
9. Corrosion of metals is a serious concern in industries. Some metals are made "rust proof" with the addition of a second metal. For example, galvanized nails are used in construction products outdoors as the nails won't easily rust even moist environments. Galvanized nails are made of iron coated in zinc. a. The oxidation of iron involves the reduction of oxygen gas with water. Find the reduction potential for this half reaction. (You'll need this number to help answer the other parts of this question!) b. The oxidation half reaction involves iron losing electrons. Iron ion, however, has two possible oxidation states. Which ion, Fe2+ or Fe³+, do you predict would form more spontaneously with the half reaction from part a. Explain.
The table of standard reduction potential is interpreted as follows: a. It is constructed with the most positive oxidation potential at the bottom b. It is arranged according to increasing reduction potential c. Elements listed below one in the series makes it good for oxidation half reaction d. Elements listed above one in the series makes it good for reduction half reaction e. All of the above
10. Refer to the attached photo below. Thank you!
1.Represent in the conventional manner, i.e., anode/cathode, the voltaic cell in which each of the following reactions occur spontaneously. A. Zn + Ni2* → Zn2* + Ni B. 2AI + 3CI2 → 2AICI3 С. Н2 + 2Ag* → 2H* +2Ag D. 2H* + Pb → H2 Pb2+ + 2. Write the half reactions occurring at the cathode and at the anode when each cell shown in problem #1 is delivering current. 3. Calculate the voltage of the cell shown in problem #1.
41. Balance each redox reaction occurring in basic aqueous solution. CIO, "(aq) + O,() -MnO(s) + Al(OH), (aq) b. Al(s) + Mn0, lag) -d (ag) + CIO (ag)
Please do #3 In the picture. I am confused if the answer is d since potassium has the lowest value of standard reduction potential and therefore it will be the strongest reducing agent. Or if it is a since K+ can’t be oxidized anymore (or can it?) and I think the reduction agent needs not be oxidized. And then so is the answer A or D? Thanks for you help.
3. write a report on the use of zinc as a “sacrificial anode” to minimise the corrosion of iron and steel such as on ships. Use the standard electrode potentials given in question 2 above to predict the cell emf and overall equation for the reaction that would occur in standard conditions between zinc and iron. With ocean-going ships, however, what is the solution in which the two metals are immersed? Is this solution always at an exact concentration of 1 mol dm-3? And in what ways does this real-life situation differ from the standard condition of 25oC / 298K Picture of question 2 is also given
II. In the table of standard reduction potentials, locate the half-reactions for the reductions of the following metal ions to the metal: Sn*?a0), Au*e), Zn²*a), Co?"a), Ag*), and Cu² ta9). Among the metal ions and metals that make up these half-reactions: a) oxidizing agent? b) oxidizing agent? c) reducing agent? Which metal ion is the weakest Which metal ion is the strongest Which metal is the strongest
Calculate Ecell (volts) for the galvanic cell containing the reaction shown below where the concentration of the ion at the anode is 0.500 M and the concentration of the ion at the cathode is 1.50 M. Use the standard reduction potentials from Appendix L in our textbook.
1) Construct a zinc-copper electrochemical cell using 1.0 M Zn2+ and 1.0 M Ni2+ solutions. a. Provide the shorthand notation. b. What is the EMF of this cell (include units)? c. For the voltage that you are measuring, is this E°cell or Ecell? Explain.