Given the half reactions and En values below,Fe2* + 2e → FeE° = -0.45 VH2O2 + 2H* + 2e → 2H20E° = +1.78 V2H + 2e - H2E° = 0.00V4H + NO, + 3e NO + 2H2O E° = +0.96VDetermine which species is the strongest reducing agent.O NOO H2H20Fe

Electrochemical series is series of elements arranged in increasing order of reduction potentials.…

Answered: Determine which species is the…

Science

Chemistry

Determine which species is the strongest reducing agent.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 35E: Consider the following galvanic cell: Label the reducing agent and the oxidizing agent, and describe...

See similar textbooks

Related questions

Q: Use reduction potentials to predict whether a redox reaction is spontaneous?

A: Given term, Spontaneity of a redox reaction

Q: Given the following standard reduction potentials:

A: To find the standard emf of a cell Ecello = ( Ered o)cathode -( Eredo )anode When two half…

Q: Assuming standard conditions, and considering the table of standard reduction potentials for…

A: More negative will be the reduction potential more strong will be the reducing agent.

Q: What current is required to produce 0.78 grams per hour by the electrolytic reduction Al+ + 3e Al?

A: The electrolytic reduction is the reduction of any substance in the presence of electric current.…

Q: 1. Based on the standard reduction potentials in Table 2, which of the following metals could…

A: The metals given are Al, Cu, Ni and Zn.

Q: Using the standard reduction potential table, compute for the corresponding E°cell of the following…

A: The given redox reaction of the cell is : Pb+2(aq)+Li(s)→Pb(s)+Li+(aq) To determine= Ecell°

Q: Which substance is the strongest reducing agent? Which is weakest?

A: In redox reaction, one reactant is reduced and another reactant is oxidized.

Q: Balance the following equation in acidic solution: Identify the reducing agent: Oxidizing agent:…

A: the process which involves loss of electron is called oxidation the process which involves gain of…

Q: What is the oxidizing agent and what is the reducing agent in the galvanic cell formed by Mg and Cu?

A: Given: Galvanic cell formed using Mg and Cu elements.

Q: B. Using the standard reduction potentials, calculate the standard emf. Cr + 2Cr³+ 3Cr²+

A: Standard EMF = 0.48 V

Q: Which substance is the weakest reducing agent?

A: Reducing Agent - A substance that reduces others and oxidizes itself is known as a reducing agent.…

Q: The redox reaction in acidic solution is shown below. What will be the coefficient of the Bros ion…

Q: What is the minimum voltage required to drive the reaction?

A: Standard reduction potential can be calculated as follows:

Q: From the standard reduction potential table, determine which of the following is the strongest…

Q: , calculate the standard reaction free energy AG° for the following redox reaction.

Q: The equilibrium constant for the following reaction is 5.6 x 10 at 25.0°C. M(s) + 2Cd²*(aq) → 2Cd(s)…

A: A reducing agent is defined as a compound or element that easily reduce other and itself get…

Q: Balance the following Redox reaction in basic solution: H2O2 + MnO4 → Mn + 02

Q: What is the standard reduction potential when: b. 02(g) is reduced to hydrogen peroxide

A: Reduction is the process when a compound accepts electrons. The standard reduction potential is the…

Q: What amount of Cu (in grams) is deposited at the cathode when a current intained for 15 minutes in a…

A: Faraday's second law of electrolysis explains that when a certain amount of charge is passed, the…

Q: Use the table 'Standard Reduction Potentials' located in the 'Tables', to predict if a reaction will…

A: We have to balance and find out the reaction will occur or not

Q: Calculate Ecell (volts) for the galvanic cell containing the reaction shown below where the…

Q: Which of the following metals is the best oxidizing agent and which is the best reducing agent? Zn,…

A: Oxidising agents are those species which itself undergoes reduction to oxidise the other species in…

Q: Balance the following redox reaction in basic solution. Br (aq)+N,(g) → Br,(1)+N,H,(aq)

A: From given the reaction is as follows Br- + N2 ----> Br2 + N2H4 Hence it is balanced with the…

Q: Complete and balance the following redox reaction in basic solution.

Q: Zn O ↑ ZnCl2 * OXIDIZING REDUCING

A: It is oxidizing

Q: Balance the following redox reaction in an basic solution using the oxidation number method.…

Q: Based on the standard reduction potentials in Table 2, which of the following metals could provide…

A: A question based on electrochemistry, which is to be accomplished.

Q: What methods are used to reduce the corrosion of metals?

A: Corrosion is a naturally occurring process where a metal is converted into its metal oxide by…

Q: Balance the following redox reaction in acidic solution.

A: 5 SO32- + 6 H+ + 2 MnO4- → 5 SO4-2 + 2 Mn+2 + 3 H2O

Q: 6. Which metal is the best reducing agent? (a) Ag (b) Mg (c) Fe (d) Pb

Q: Assuming standard conditions, arrange the following in order of increasing strength as oxidizing…

A: The more positive the standard reduction potential is, the stronger the oxidizing agent is on the…

Q: Balance this redox reaction in basic conditions: V2+ + V(OH)4+ → VO2+

A: The given redox reaction is: V2+ + V(OH)4+ → VO2+

Q: Balance the following redox reaction in acidic solution: Fe(s) + 03(g) → Fe203(s) + 02(g)?

A: Balancing a chemical equation means the no. Of elements in reactant side must be equal to the no.…

Q: From the standard reduction potential table, determine which of the following is the strongest…

A: Oxidizing agent-A substance that trends to bring about oxidation by being reduced and gaining…

Q: Which of the following metals is the best reducing agent? Mn O Mg O Cr O Cd

A: The provided metals are Mn, Mg, Cr, Cd Metal having greater standard oxidation potential value will…

Q: Consider the redox reaction below: O2(g) + 2H'(aq) + Fe(s) → Fe2"(aq) + H2O2aq) The reducing agent…

Q: What is electrochemical series. Give 2 elements that can be used to protect steel from corrosion…

A: Electrochemical series is a series of elements that are arranged on the basis of increasing…

Q: reacts rapidly with water according to the following scheme. [Co(H2O)6]*+ + H20 → [Co(H2O)6]²+ + O2…

Q: Balance each redox reaction occurring in acidic aqueous solution. b. Mg(s) + Cr"(aq) Mg"(aq) + Cr(s)

A: We have following redox reaction Mg (s) + Cr+3 (aq) → Mg+2 (aq)+ Cr(s) Step 1: Separate the overall…

Q: Balance the following redox reaction in acidic solution. CI (aq) +103(aq) Cl₂(g) +1₂(s)

A: We need to balance the given equation in acidic medium.

Q: Silver-Copper Sulver-Zinc Copper-Zinc Of all the possible components listed above, which is the…

A: After observing the electrochemical series the couple which have least value of reduction potential…

Q: How many seconds will it take to plate out 2.19 grams of chromium metal from a solution of chromium…

Q: Balance the following redox reaction in acidic solution. H,0(1)+Cl,(g) → 0,(g)+Cl (aq)

A: Please find the answer given below:

Q: Balance the following redox reaction in acidic solution. BiO, + Re- Bi + ReO,

A: Record the unbalanced equation, BiO3- + Re3- → Bi2- + ReO4-

Q: Complete and balance the following half-reaction in basic solution 5 X Cr(OH)3(s) → CrO42-(aq)

A: The given half cell reaction is: To balance, under basic medium, following steps are needed: First…

Q: Balance each redox reaction under the conditions indicated. 3. Fe(s) + CrO,² (aq) → Fe2O3(s) +…

A: Given that : We have to balance the redox reaction under basic solution :

Question

Given the half reactions and En values below,
Fe2* + 2e → Fe
E° = -0.45 V
H2O2 + 2H* + 2e → 2H20
E° = +1.78 V
2H + 2e - H2
E° = 0.00V
4H + NO, + 3e NO + 2H2O E° = +0.96V
Determine which species is the strongest reducing agent.
O NO
O H2
H20
Fe

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

The Nernst equation allows determination of the cell potential for a galvanic cell at nonstandard conditions. Write out the Nernst equation. What are nonstandard conditions? What do , n, and Q stand for in the Nernst equation? What does the Nernst equation reduce to when a redox reaction is at equilibrium? What are the signs of G and when K 1? When K 1? When K = 1? Explain the following statement: determines spontaneity, while determines the equilibrium position. Under what conditions can you use to predict spontaneity?
An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?
Why is it not possible for hydroxide ion (OH-) to appear in either of the half-reactions or the overall equation when balancing oxidation—reduction reactions in acidic solution?
What is electrochemistry? What are redox reactions? Explain the difference between a galvanic and an electrolytic cell.
A galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2, resulting in the reaction H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)K=? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2 solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate at the halfway point in the titration.
An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
In biological systems, acetate ion is converted to ethyl alcohol in a two-step process: CH3COO(aq)+3H+(aq)+2eCH3CHO(aq)+H2OE=0.581V CH3CHO(aq)+2H+(aq)+2eC2H5OH(aq)E=0.197V (E°' is the standard reduction voltage at 25°C and pH of 7.00.) (a) Calculate G°' for each step and for the overall conversion. (b) Calculate E°' for the overall conversion.
The saturated calomel electrode. abbreviated SCE. is often used as a reference electrode in making electrochemica1 measurements. The SCE is composed of mercury in contact with a saturated solution of calomel (Hg2Cl2). The electrolyte solution is saturated KCI. is +0.242 V relative to the standard hydrogen electrode. Calculate the potential for each of the following galvanic cells containing a saturated calomel electrode and the given half-cell components at standard conditions. In each case. indicate whether the SCE is the cathode or the anode. Standard reduction potentials are found in Table 17.1. a. Cu2++2eCu b. Fe3++e-Fe2+ c. AgCl+e-Ag+Cl- d. Al3++3eAl e. Ni2++2eNi
A solution contains the ions H+, Ag+, Pb2+, and Ba2+, each at a concentration of 1.0 M. (a) Which of these ions would be reduced first at the cathode during an electrolysis? (b) After the first ion has been completely removed by electrolysis, which is the second ion to be reduced? (c) Which, if any, of these ions cannot be reduced by the electrolysis of the aqueous solution?
(a) Is it easier to reduce water in acid or base? To evaluate this, consider the half-reaction 2H2O() + 2 e 2 OH(aq) + H2(g) E = 0.83 V (b) What is the reduction potential for water for solutions at pH = 7 (neutral) and pH = 1 (acid)? Comment on the value of E at pH = 1.
Atomic masses can be determined by electrolysis. In one hour, a current of 0.600 A deposits 2.42 g of a certain metal, M, which is present in solution as M+ ions. What is the atomic mass of the metal?
Consider the following galvanic cell: Label the reducing agent and the oxidizing agent, and describe the direction of the electron flow.