Determine theredox potential for MnO4â conversion to Mn3+ atpH= 6. Ifound thepotential from a Latimer diagram: 1.5 V. I know Imust use theequation "POTENTIAL -(.059 X pH)," but I don't come up with the rightanswer (0.8 V)

OneClass: Determine theredox potential for MnO4â conversion to Mn3+ atpH= 6. Ifound thepotential fr...

Electrochemistry. Please show work, label all answers clearly, and write legibly. Standard reduction potentials are found in Appendix E of your textbook On your paper, at the TOP, write (a) the FULL NAME of your TA; and (b) your section as "SECTION ##". Failure to do this will result in a deduction of I pt The following diagram, called a Latimer diagram, summarizes the standard reduction potentials for various nitrogen-containing compounds and ions in acidic aqueous solution. It contains useful data for this HW set. 0.97 V 0.79 V 1.12 V 1.00 V 1.59 V 1.25 V 0.89 V An arrow represents the "properly balanced reduction half-reaction" between the oxidized species on the left and the reduced species on the right of the arrow. The potential value over each arrow is the standard reduction potential E'ned for that properly balanced half-reaction. For example, from this diagram, you can write No, (aq) + e + 2 H+(aq)-â NO2(g) + H20(/); E0ted _ +0.79 V (1) (18 pts) When H S(g) is bubbled into nitric acid solutions, S(s), NOg), NO(g), N2(g), and NH4 (a) all form. (a) (8 pts) Write the four balanced reactions that describe this complex process. (b) (8 pts) For each reaction in part (a), calculate the standard emf (in V) (c) (2 pts) Which of the four reactions has the greatest driving force and which has the least driving force per electron (2) (16 pts) Use the Latimer diagram above for this question. (a) (6 pts) NO (g) disproportionates spontaneously into nitric acid and nitrous acid in acidic media. Show this (b) (6 pts) Nitrous acid will not disproportionate spontaneously to nitrogen dioxide and nitric oxide. Show this (c) (4 pts) Given that the definition of 1 volt = 1 Joule Coulomb, show that the reduction of the nitrate ion to by writing the balanced chemical reaction and evaluating the standard emf for the reaction. by writing the balanced chemical reaction and evaluating the standard emf for the reaction. nitrogen gas in acidic media has a standard reduction potential of +1.25 V (3) (6 pts) Active metals like zinc will react with concentrated nitric acid to produce the ammonium ion and the Zn (a) ion at 25Â°C (a) (4 pts) Write the balanced chemical equation for this process using smallest whole number coefficients. (b) (2 pts) Evaluate ÎEo (V) for the reaction in part (a). (4) (6 pts) Less active metals like copper will react with concentrated nitric acid to produce nitric oxide gas and the Cu (aq) ion at 25Â°C. (a) (4 pts) Write the balanced chemical equation for this process using smallest whole number coefficients. (b) (2 pts) Evaluate AE for the reaction in part (a). BONUS (8 pts; and PRACTICE): Write all balanced half-reactions indicated by the Latimer diagram above

Need help with #4

Electrochemistry. Please show work, label all answers clearly, and write legibly. Standard reduction potentials are found in Appendix E of your textbook On your paper, at the TOP, write (a) the FULL NAME of your TA; and (b) your section as "SECTION ##". Failure to do this will result in a deduction of I pt The following diagram, called a Latimer diagram, summarizes the standard reduction potentials for various nitrogen-containing compounds and ions in acidic aqueous solution. It contains useful data for this HW set. 0.97 V 0.79 V 1.12 V 1.00 V 1.59 V 1.25 V 0.89 V An arrow represents the "properly balanced reduction half-reaction" between the oxidized species on the left and the reduced species on the right of the arrow. The potential value over each arrow is the standard reduction potential E'ned for that properly balanced half-reaction. For example, from this diagram, you can write No, (aq) + e + 2 H+(aq)-â NO2(g) + H20(/); E0ted _ +0.79 V (1) (18 pts) When H S(g) is bubbled into nitric acid solutions, S(s), NOg), NO(g), N2(g), and NH4 (a) all form. (a) (8 pts) Write the four balanced reactions that describe this complex process. (b) (8 pts) For each reaction in part (a), calculate the standard emf (in V) (c) (2 pts) Which of the four reactions has the greatest driving force and which has the least driving force per electron (2) (16 pts) Use the Latimer diagram above for this question. (a) (6 pts) NO (g) disproportionates spontaneously into nitric acid and nitrous acid in acidic media. Show this (b) (6 pts) Nitrous acid will not disproportionate spontaneously to nitrogen dioxide and nitric oxide. Show this (c) (4 pts) Given that the definition of 1 volt = 1 Joule Coulomb, show that the reduction of the nitrate ion to by writing the balanced chemical reaction and evaluating the standard emf for the reaction. by writing the balanced chemical reaction and evaluating the standard emf for the reaction. nitrogen gas in acidic media has a standard reduction potential of +1.25 V (3) (6 pts) Active metals like zinc will react with concentrated nitric acid to produce the ammonium ion and the Zn (a) ion at 25Â°C (a) (4 pts) Write the balanced chemical equation for this process using smallest whole number coefficients. (b) (2 pts) Evaluate ÎEo (V) for the reaction in part (a). (4) (6 pts) Less active metals like copper will react with concentrated nitric acid to produce nitric oxide gas and the Cu (aq) ion at 25Â°C. (a) (4 pts) Write the balanced chemical equation for this process using smallest whole number coefficients. (b) (2 pts) Evaluate AE for the reaction in part (a). BONUS (8 pts; and PRACTICE): Write all balanced half-reactions indicated by the Latimer diagram above

Use a Standard Reduction table to write a balanced redox equation, and to determine the cell potential and the number of electrons transferred for the spontaneous process that occurs. Use no special characters for subscripts and superscripts and include the coefficient with the substance. 3Fe2+ should be written as 3Fe2+. Note that Ox1 and Red2 are the oxidizing and reducing agents, and Red1 and Ox 2 are the other half of their couples.

a) An Fe2+/Fe couple is connected to Sn2+/Sn couple.

Ox1 + Red2 Red1 + Ox2
1 [Correct: Your answer is correct.] + 2 [Correct: Your answer is correct.] 3 [Correct: Your answer is correct.] + 4 [Correct: Your answer is correct.]

The standard cell potential is E =

5 [Correct: Your answer is correct.] V

The number of electrons transferred is n =

6 [Correct: Your answer is correct.]

b) An Ag1+/Ag couple is connected to Sn2+/Sn couple.

Ox1 + Red2 Red1 + Ox2
7 [Correct: Your answer is correct.] + 8 [Correct: Your answer is correct.] 9 [Correct: Your answer is correct.] + 10 [Correct: Your answer is correct.]

The standard cell potential is E =

11 [Correct: Your answer is correct.] V

The number of electrons transferred is n =

12 [Correct: Your answer is correct.]

c) Aluminum is placed in hydrochloric acid.

Ox1 + Red2 Red1 + Ox2
13 + 14 15 + 16

The standard cell potential is E =

17 V

The number of electrons transferred is n =

18

d) Copper is placed nitric acid.

Ox1 + Red2 + Other Red1 + Ox2 + Other
19 + 20 + 21 22 + 23 + 24

The standard cell potential is E =

25 V

The number of electrons transferred is n =

26

Please help I was able to figure out the first two, but the last two are a bit challenging. Thank you in advance! P.S. the numbers that go up to 26 aren't answers they are the question numbers from webassign normally hidden, I tried to remove them to make it neat, but I was not allowed to post my question without them, sorry for the lack of organization.

Determine theredox potential for MnO4â conversion to Mn3+ atpH= 6.

Ifound thepotential from a Latimer diagram: 1.5 V. I know Imust use theequation

"POTENTIAL -(.059 X pH)," but I don't come up with the rightanswer (0.8 V)

Unlock all answers

Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Principles of Chemistry Molecular Approach

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

Related questions

Weekly leaderboard

Determine theredox potential for MnO4â conversion to Mn3+ atpH= 6. Ifound thepotential from a Latimer diagram: 1.5 V. I know Imust use theequation "POTENTIAL -(.059 X pH)," but I don't come up with the rightanswer (0.8 V)

Unlock all answers

Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Principles of Chemistry Molecular Approach

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

Related questions

Weekly leaderboard

Determine theredox potential for MnO4â conversion to Mn3+ atpH= 6.

Ifound thepotential from a Latimer diagram: 1.5 V. I know Imust use theequation

"POTENTIAL -(.059 X pH)," but I don't come up with the rightanswer (0.8 V)