Answered: Q. Balance the following redox…

Q. Balance the following redox reactions in the solutions specified. a. Cu(NH3)42+ + S2O42- —> SO32- + Cu + NH3 in basic soln. b. MnO4- + S2O32- —> S4O62- + Mn2+ in acid.

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter8: Electrochemistry And Ionic Solutions

Section: Chapter Questions

Problem 8.25E

See similar textbooks

Related questions

Q: Balance each redox reaction occurring in acidic aqueous solution.a. PbO2(s) +…

A: Redox reactions are the reactions in which oxidation and reduction reactions happen simultaneously.…

Q: Determine the temperature at which the redox couples are in equilibrium, use nernst equation E =…

A: The equation that connects the half cell potential value to the temperature, and the reaction…

Q: Balance by half reaction in acidic solution: Zn + NO3- --> Zn2+ + NO

Q: Balance the reaction below by the half reaction method. When balanced, what is the coefficient of…

A: Given a Redox reaction to balance by half reaction method: Mg2+(aq) + H2S (aq) --> SO2 (g) + Mg…

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

Q: The Standard potential for the reduction of AgClcS) °sto. 222V. Ag Gles)te→ Agcs) +Cl (aq) 0Singthis…

A: Given: RHE: AgCl(s)+e-↔Ag+Cl- …ER=0.222 V To find: Solubility product constant, Ksp

Q: With the half reaction method, balance the redox equation under acidic conditions. MnO4- + NO2- =>…

A: The given redox reaction is as follows: MnO4- + NO2- → NO3- + Mn2+ A redox reaction is balanced…

Q: Balancing redox reactions in basic solution 7) Ag25 + CN' + O2 ---> Ag(CN)Z + S8 + OH 8) N2H4+…

A: Balancing of a redox reaction is done by using following steps. First determine oxidation and…

Q: with solution) 5. Fe +

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: Balance the following redox reaction and show all steps (Fictitous Reaction)

Q: Using s rd reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy…

A: Using equation: ∆G0= -nFE0 cell ∆G0 = standard Gibbs free energy n = no. of electron in that…

Q: Hg(l) + H₃IO6-2(aq) → Hg₂O(s) + IO3-(aq) Balance using the half-reaction method, under basic…

A: Given unbalanced chemical reaction, Hg(l) + H3IO6–2(aq) → Hg2O(s) + IO3– (aq)

Q: A sample of impure tin of mass 0.535 g is dissolved in strong acidto give a solution of Sn2+. The…

A: Redox reaction or Oxidation-reduction reaction: The reaction in which the oxidation and reduction…

Q: A. Balance the equation by oxidation number methad and Identify the oxidizing and veducing agents.…

A: A. Balance by oxidation number method. MnSO4 + PbO2 + H2SO4 → HMnO4 + PbSO4 + H2O Assign oxidation…

Q: The eqalibrium constant, K, for a redox reaction. 18 related to the standard potentials to, by the…

A: Given: Equilibrium constant for the reaction = 9.10 × 10-4 And the reaction is X (s) + Y+ (aq) → X+…

Q: Balance the following redox equations using the half-reaction method: +HPO(OH) d) N031- + BizSs Bi3+…

A: Since we are entitled to answer up to 3 sub-parts, we’ll answer the first 3 as you have not…

Q: For a particular redox reaction, MnO2MnO2 is oxidized to MnO4- and Ag+A is reduced to Ag. Complete…

Q: Refer to the galvanic cell below (the contents of each half-cell are written beneath each…

Q: Hg(l) + H₃IO6-2(aq) → Hg₂O(s) + IO3-(aq) Balance using the half-reaction method

Q: Balance each redox reaction in basic solution (First balance in acidic medium and then change into…

Q: Given the reduction reaction and reduction potentials. Which of the reactions (a-e) are spontaneous?…

A: ΔG is negative for a spontaneous reaction. Therefore, the value of electromotive force(emf) or…

Q: Using data from the table below, place the following in order of decreasing strength as oxidizing…

Q: From the below data: Please show a detail on how to calculate Q and Ecell (calc) Ecell = 0.941V…

A: Nernst equation :- The Nernst equation provides a relation between the cell potential of an…

Q: Balance the equation occurring in basic solution:I-(aq) + MnO4 -(aq)¡I2(aq) + MnO2(s)SolutionTo…

A: Redox reactions are reactions in which, oxidation and reduction take place simultaneously. Oxidation…

Q: Given: Fe2+ + 2e- --> Fe Eº = -0.44V Fe3+ + 3e- --> Fe…

A: Fe + Cl2 ==> Fe2+ + 2 Cl-

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

Q: Balance the following redox equations: CrO42- + Fe2+ —> Cr3+ + Fe3+ (in acidic solution) MnO4- +…

A: The give reaction is balanced by half reaction method,First find the oxidation and reduction half…

Q: Balance by half reaction in acidic solution: Sn2+ + MnO4- --> Sn4+ + Mn2+

Q: Balance by half reaction: Cr3+ + S + H2O --> H2S + H+ + Cr2O72-

Q: Calculate the standard Gibbs free energy ΔG° and the E°cell voltage for the following redox…

A: GIVEN: Reactions: To Solve: Standard Gibbs free energy ΔG°=? E°cell voltage =?

Q: Q1/Determine the corrosion rate of carbon steel in salt solution from the following laboratory data.…

Q: Balance the equation using the half-reaction method: CN– + MnO4– --> CNO– + MnO2…

Q: Consider the following standard reduction potentials in acid solution: E (V) -1.66 A13+ + 3e - Al(S)…

A: Consider the given standard reduction potential in acid solution is as follows; Al3+ + 3e- →…

Q: O Fe(ag) The balanced half-reaction occuring at the cathode in the redox reaction shown below is…

A: Redox reaction is a reaction in which both oxidation and reduction occurs simultaneously. In…

Q: 1. Write balanced redox equations for the following reactions. Show the full balancing process and…

A: Solution

Q: The cell potential of the following cell is determined using an unspecified concentration of acid.…

Q: Using data from the table below, place the following in order of decreasing strength as oxidizing…

A: The species with the higher value of reduction potential undergoes reduction easily and therefore,…

Q: Calculate the standard reaction free energy (AGO) for the following unbalanced redox reaction in…

A: Oxidation means loss of electrons and reduction means gain of electrons during redox reaction.

Q: Write a balanced redox equation assuming the reaction takes place in acidic solution. H2O2 + Fe2+…

Q: Consider the following unbalanced oxidation-reductionreactions in aqueous solution:Ag+(aq) +…

Q: Balance the following redox reactions in basic solution: a. Se + Cr(OH)3 -> Cr + SeO32- b. MnO4- +…

A: To solve this problem we will have to balanced the given chemical equation .

Q: 10 16 18 19 20 26 (27 (28 29 « < Half-Reaction Standard Reduction Potentlal, E" (V) Ag+ (ag) + e-…

A: Given that: The cell is made of Pb.Pb(NO3)2 and Cu.Cu(NO3)2 half cells. To find, which among the…

Q: Balance the following in acid solution using the half reaction method. PbO2 + l2 ------> Pb^2+ +…

A: The question is based on concept of redox reactions. we have to balance the given reaction in acidic…

Q: Calculate the Free Gibb’s Energy, kJ/mol, for the following redox reaction at 25.0°C. 2Ce4+(aq) +…

A: Given The following redox reaction is - 2Ce4+ (aq) + 2Cl- (aq) →Cl2 (g) + 2Ce3+(aq) anode - 2Cl-…

Q: he oxidation–reduction reaction: S4O62- + Cr2+ → Cr3+ + S2O32- Half-reactions:

A: The given chemical reaction S4O62- + Cr+2 → Cr+3+ S2O32- In an electrochemical cell, oxidation…

Q: H3PO3 + Cl3- --> Cl2 + HPO3 Balance this redox equation for reaction in acidic solution, and…

A: Balance this reaction by oxidation number method. In this method first balance atom undergoing…

Q: Which redox reaction is spontaneous? OCr(s) + Al³+ (aq) → Cr** (aq) + Al(s) OPb(s) + Co²+ (aq) -…

Q: Given the following unbalanced redox reaction in acidic media: Fe2+ + Cr2O72- → Fe3+ +…

A: Oxidation half-reaction: The reaction in which a substance loses its electrons. In this, the…

Question

Q. Balance the following redox reactions in the solutions specified.

a. Cu(NH₃)₄²⁺ + S₂O₄^2- —> SO₃^2- + Cu + NH₃in basic soln.

b. MnO₄^- + S₂O₃^2- —> S₄O₆^2- + Mn²⁺in acid.

Definition Definition Chemical reactions involving both oxidation and reduction processes. During a redox reaction, electron transfer takes place in such a way that one chemical compound gets reduced and the other gets oxidized.

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

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

Using data from Table 17-1, place the following in order of increasing strength as reducing agents (all under standard conditions). Cu+,F,H,H2O,I2,K
Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
When jump-starting a car with a dead battery, the ground jumper should be attached to a remote part of the engine block. Why?
Calculate the equilibrium constant for the following reactions using data from the standard reduction potential tables. (a) Cl2(g)+2Br-(aq)Br2(g)+2Cl-(aq) (b) Ni(s)+2Ag+(aq)2Ag(s)+Ni2+(aq) (c) I2(s)+Sn2+(aq)2I(aq)+Sn4+(aq)
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.
What cathode potential (versus SCE) would be required to lower the total Hg(II) concentration of the following solutions to 1.00 10-6 M (assume reaction product in each case is elemental Hg): (a) an aqueous solution of Hg2+? (b) a solution with an equilibrium SCN- concentration of 0.100 M? Hg2+ + 2SCN- Hg(SCN)2(aq) = Kf = 1.8 107 c) a solution with an equilibrium Br- concentration of 0.100 M? HgBr42++ 2e- Hg(l) + 4Br- E0= 0.223 V
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)?
Consider the following galvanic cell: Label the reducing agent and the oxidizing agent, and describe the direction of the electron flow.