Question

In: Chemistry

Use the link Standard Reduction Potentials to answer the following questions. For each pair of redox...

Use the link Standard Reduction Potentials to answer the following questions.
For each pair of redox couples, write a balanced redox equation, determine the cell potential and the number of electrons transferred. Use the lowest possible coefficients. Include states-of-matter in your answer.

a) H¹⁺/H₂ + Ag¹⁺/Ag
chemPad Help
E^o = V	n (moles of e^-) =
b) H¹⁺/H₂ + Pb²⁺/Pb
chemPad Help
E^o = V	n (moles of e^- )=
c) Al³⁺/Al + Cu²⁺/Cu
chemPad Help
E^o = V	n (moles of e^- )=
d) Fe²⁺/Fe + Zn²⁺/Zn
chemPad Help
E^o = V	n (moles of e^-) =

Ox + ne¹

Expert Solution

1)

H1+/H2 + Ag1+/Ag 0 // +0.80

Recall, the most positive will reduce, the other will oxidize, therefore

Ag+1 + 1e- ---> Ag (will reduce)

2H+ + 2e- --> H2 ( will not reduce, you need to invert this)

Balance equations

2Ag+1(aq) + 2e- + H2(g) ---> 2H+(aq) + 2e- + 2Ag(s) (aq)

E cell = Ered + Eox = +0.80 +(0) = +0.80

2 mol of electrons were transfered

2)

H1+/H2 + Pb2+/Pb 0 // -0.13

2H+ + 2e- --> H2 (will reduce)

Pb+2 +2e- --> Pb ( will not reduce, you need to invert this)

Balance Equation

2H+(aq) + 2e- + Pb(aq) ---> Pb+2(aq) + 2e- + H2(g)

E cell = Ered + Eox = 0 - (-0.13) = +0.13

2 mol of e- were transferred

3)

Al3+/Al + Cu2+/Cu -1.66 // +0.34

Cu+2 + 2e- ---> Cu(s) (will reduce)

Al+3 + 3e- ---> Al(s) (will not reduce, invert it!)

Balance Equation

3Cu+2(aq) +6e- + 2Al(s) ---> 3Cu(s) + 2Al+3(aq) + 6e-

E cell = Ered + Eox = 0.34 + 1.66 = +2.0

6 moles of electrons were transferred

4)

Fe2+/Fe + Zn2+/Zn -0.44 // -0.76

Zn+2 + 2e- ---> Zn(s) (will not reduce, invert it)

Fe+2 + 2e- ---> Fe(s) (will reduce)

Fe+2(aq) + 2e- Zn(s) ---> Fe(s) + 2e- + Zn+2 (aq)

E cell = Ered + Eox = -0.44 + 0.76 = +0.32

2 moles of electrons were transferred

queen_honey_blossom answered 1 year ago

Assuming standard conditions, answer the following questions. (Use the table of Standard Reduction Potentials for common...

Assuming standard conditions, answer the following questions. (Use the table of Standard Reduction Potentials for common Half-reactions from your text. If hydrogen is one of the reagents, assume acidic solution.) 1) Is Cr3+(aq) capable of oxidizing Fe2+(aq) to Fe3+(aq)? 2) Is Cr metal capable of reducing Fe2+(aq)? 3) Is Sn metal capable of reducing Fe3+(aq) to Fe2+(aq)? 4)Is H2(g) capable of reducing Ni2+(aq)? 5) Is Fe2+(aq) capable of reducing Cr3+(aq) to Cr metal? 6)Is VO2+(aq) capable of oxidizing Fe2+(aq)?

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)

For each of the four respiratory complexes, list the redox centers and their reduction potentials. What...

For each of the four respiratory complexes, list the redox centers and their reduction potentials. What is the significance of the order each redox center is used in electron transport?

use the table of standard reduction potentials to ecplain why iron will reduce copper but it...

use the table of standard reduction potentials to ecplain why iron will reduce copper but it will not reduce sodium

1.) Use a table of Standard Reduction Potentials to predict if a reaction will occur when...

1.) Use a table of Standard Reduction Potentials to predict if a reaction will occur when Mg metal is put into a 1M aqueous H+solution. If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank. 2.) Use a table of Standard Reduction Potentials to predict if a reaction will occur between Zn metal and I2(s), when the two are brought in contact via standard half-cells in a...

1. Using a table of standard reduction potentials, standard conditions are assumed. (a) Arrange the following...

1. Using a table of standard reduction potentials, standard conditions are assumed. (a) Arrange the following chemical species: Zn(s), Cl-(aq), Cu(s), K(s), and H2(g) in order of their ease of oxidation, from easiest to oxidize to hardest to oxidize. (b) Arrange the following chemical species: H+(aq), I2(s), Na+(aq), Ag+(aq), and H2O(l) in order of their ease of reduction, from easiest to reduce to hardest to reduce. 2. Which of the following reactions is/are product favored? Zn(s) + I2(s) ? Zn+2...

Please use the link to the case study to answer the questions bellow. use the link...

Please use the link to the case study to answer the questions bellow. use the link to the case study please. this is due today. https://books.google.com/books?id=bzb3BQAAQBAJ&pg=PA198&lpg=PA198&dq=case:+cursory+exams+are+risky&source=bl&ots=W2jLZ9niMa&sig=uYHeQOv-uuQ7ISm0YAdp7JcURBc&hl=en&sa=X&ved=0ahUKEwjkhaPf7ZLZAhUl8IMKHfHnCN8Q6AEIMDAB#v=onepage&q=case%3A%20cursory%20exams%20are%20risky&f=false Case: Cursory Exams are Risky Questions The many lessons for discussion in Niles v. City of San Rafael include the following; 1.An organization can improve the quality of patient care rendered in the facility by establishing and adhering to policies, procedures and protocols that facilitate the delivery of high-quality care across all disciplines. 2....

Use standard reduction potentials to calculate ΔG° for the reaction: ClO4- + 6 Cl- + 6...

Use standard reduction potentials to calculate ΔG° for the reaction: ClO4- + 6 Cl- + 6 H3O+ →ClO- + 3 Cl2 + 9 H2O E°ClO4-/ClO-, H3O+ = +1.36, E°Cl2/Cl- = +1.35827

Use the table of standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 ∘C) for the following reaction:

Standard reduction potentials Reduction half-reaction E∘ (V) Ag+(aq)+e−→Ag(s) 0.80 Cu2+(aq)+2e−→Cu(s) 0.34 Sn4+(aq)+4e−→Sn(s) 0.15 2H+(aq)+2e−→H2(g) 0 Ni2+(aq)+2e−→Ni(s) −0.26 Fe2+(aq)+2e−→Fe(s) −0.45 Zn2+(aq)+2e−→Zn(s) −0.76 Al3+(aq)+3e−→Al(s) −1.66 Mg2+(aq)+2e−→Mg(s) −2.37 Part A Use the table of standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 ∘C) for the following reaction: Fe(s)+Ni2+(aq)→Fe2+(aq)+Ni(s) Express your answer numerically. Part B Calculate the standard cell potential (E∘) for the reaction X(s)+Y+(aq)→X+(aq)+Y(s) if K = 3.04×10−3. Express your answer to three significant figures and include the appropriate...

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...