S4O6^2- + 2e- ==> 2S2O3^2- E* = 0.090V Pt(s) [ S4O6^2-(0.50M), S2O3^2- (1.0M) ][ S4O6^2- (1.0M),...
S4O6^2- + 2e- ==> 2S2O3^2- E* = 0.090V
Pt(s) [ S4O6^2-(0.50M), S2O3^2- (1.0M) ][ S4O6^2- (1.0M), S2O3^2- (0.50M) ] Pt(s)
Based on the cell described above, which of the following statements are true?
I. At 298K, Ecell = 0.042V
II. The value of Q for the cell shown is 0.125
III. The cell will stop functioning when Q=1
IV. At 298K, the E*cell = 0..027V
Homework Answers
Request Answer!
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
Add Answer to:
S4O6^2- + 2e- ==> 2S2O3^2- E* = 0.090V
Pt(s) [ S4O6^2-(0.50M), S2O3^2- (1.0M) ][ S4O6^2- (1.0M),...
Pb2+(aq) + 2e− ⇌ Pb(s) E° = -0.126 V 2H+(aq) + 2e− ⇌ H2(g) E° =...
Pb2+(aq) + 2e− ⇌ Pb(s) E° = -0.126 V 2H+(aq) + 2e− ⇌ H2(g) E° = 0.000 V E°cell (in V)= 0.126 V 2. The electrochemical cell is comprised of a Pb electrode in a 1.67 × 100 M solution of Pb2+ (aq) coupled to a Pt electrode in a solution containing H+ (aq) where the pH of the solution is 0.37 and the partial pressure of H2(g) is 0.571 atm. The temperature of the cell is held constant at...
For the cell shown, the measured cell potential, Ecell, is -0.3629 V at 25 °C. Pt(s)...
For the cell shown, the measured cell potential, Ecell, is -0.3629 V at 25 °C. Pt(s) | H,(g, 0.707 atm) | H+ (aq, ? M) || Cd2+ (aq, 1.00 M)| Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2e - H (9) E° = 0.00 V Cd2+ (aq) + 2e — Cd(s) E' = -0.403 V Calculate the H+ concentration. M = 0.031 Incorrect
For the cell shown, the measured cell potential, Ecell, is -0.3709 V at 25 °C. Pt(s)...
For the cell shown, the measured cell potential, Ecell, is -0.3709 V at 25 °C. Pt(s) | H,(g, 0.877 atm) | H+ (aq,? M) || Cd2+ (aq, 1.00 M) Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2e H (9) E' = 0.00 V Cd2+ (aq) + 2e - Cd(s) E' = -0.403 V Calculate the H concentration. [HT] = M
For the cell shown, the measured cell potential, Ecell, is -0.3687 V at 25 °C. Pt(s)...
For the cell shown, the measured cell potential, Ecell, is -0.3687 V at 25 °C. Pt(s) | H, (8,0.873 atm) | H+ (aq, ? M) || Cd2+ (aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2e → H, (g) E° = 0.00 v Cd2+ (aq) + 2e- Cd(s) E° = -0.403 V Calculate the H+ concentration. [H+) = .0588 M Incorrect
For the cell shown, the measured cell potential, Ecell, is -0.3707 V at 25°C. Pt(s) H(8,...
For the cell shown, the measured cell potential, Ecell, is -0.3707 V at 25°C. Pt(s) H(8, 0.857 atm) H+ (aq.? M) || Cd2+ (aq, 1.00 M) | Cd() The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2e- H,(g) E° = 0.00 V Ca2+ (aq) + 2e Cd(s) E = -0.403 V Calculate the H* concentration.
Pb^2+ +2e- __> Pb e=-0.13V Ag+ +1e-__> Ag e=+0.80V Pb(s)| Pb2+ (1M) || Ag+ (1M) |...
Pb^2+ +2e- __> Pb e=-0.13V Ag+ +1e-__> Ag e=+0.80V Pb(s)| Pb2+ (1M) || Ag+ (1M) | Ag(s) Determine which of the following statements about the cell shown are True or False. The silver half-cell is the cathode. True False The mass of the silver electrode is decreasing. True False Anions move to the silver half-cell. True False Electrons are spontaneously produced in the lead half-cell. True False The cell, as represented by the line notation, is a voltaic cell. True False The standard cell potential,...
For the cell shown, the measured cell potential, Ecell, is -0.3689 V at 25 °C. Pt(s)H,(g,...
For the cell shown, the measured cell potential, Ecell, is -0.3689 V at 25 °C. Pt(s)H,(g, 0.789 atm) | H(aq, ?M) || Cd²+ (aq, 1.00 M) Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 24 H, (g) E° = 0.00 V Cd²+ (aq) + 2e - Cd(s) E = -0.403 V Calculate the H+ concentration. [H+] =
Consider the two half reactions below: Sn^2+ + 2e^- rigntarrow Sn(s) E^0 = ____ ii) Fe^2+...
Consider the two half reactions below: Sn^2+ + 2e^- rigntarrow Sn(s) E^0 = ____ ii) Fe^2+ + 2e^- rigntarrow Fe(s) E^0 = ____ Find E^0 values for these half reactions from your textbook or other reference, and record them in the spaces provided above. b) Based on the E^0 values, provide the reactions below for a galvanic cell half reactions. Anode half-reaction: Cathode half reaction: Net cell reaction: c) Calculate the E^0 cell for this. galvanic cell.
Anode E A Cathode B 7 С D Ni2+ + 2e -0.40 V Cd2+ + 2e...
Anode E A Cathode B 7 С D Ni2+ + 2e -0.40 V Cd2+ + 2e -0.26 V Ni (s) Cd (s) Reduction Ni (8) Ereduction Cd (8) Ereduction Ni2+ (aq) Cd2+ (aq) Oxidation Salt Bridge Look at the voltaic cell diagram above and finish the following sentences using options given on the table above: i) Ais ii) B is metal on the left metal on the right solution on the left iii) Cis iv) Dis solution on the right...
3. (12 pt) Suppose that S is the subset of R2 that contains all vectors on...
3. (12 pt) Suppose that S is the subset of R2 that contains all vectors on the two lines y = x and y = -2 s={[x] € R: y=x or y = -x} ER2: y = r or y=- (a) In each of the following parts (i)-(iii), either show the statements is true or give a counterexample to show that the statement is false. Clearly state TRUE or FALSE. Graphs of y = x and y = -1 may...
For the cell shown, the measured cell potential, Ecell, is -0.3629 V at 25 °C. Pt(s) | H,(g, 0.707 atm) | H+ (aq, ? M) || Cd2+ (aq, 1.00 M)| Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2e - H (9) E° = 0.00 V Cd2+ (aq) + 2e — Cd(s) E' = -0.403 V Calculate the H+ concentration. M = 0.031 Incorrect
For the cell shown, the measured cell potential, Ecell, is -0.3709 V at 25 °C. Pt(s) | H,(g, 0.877 atm) | H+ (aq,? M) || Cd2+ (aq, 1.00 M) Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2e H (9) E' = 0.00 V Cd2+ (aq) + 2e - Cd(s) E' = -0.403 V Calculate the H concentration. [HT] = M
For the cell shown, the measured cell potential, Ecell, is -0.3687 V at 25 °C. Pt(s) | H, (8,0.873 atm) | H+ (aq, ? M) || Cd2+ (aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2e → H, (g) E° = 0.00 v Cd2+ (aq) + 2e- Cd(s) E° = -0.403 V Calculate the H+ concentration. [H+) = .0588 M Incorrect
For the cell shown, the measured cell potential, Ecell, is -0.3707 V at 25°C. Pt(s) H(8, 0.857 atm) H+ (aq.? M) || Cd2+ (aq, 1.00 M) | Cd() The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2e- H,(g) E° = 0.00 V Ca2+ (aq) + 2e Cd(s) E = -0.403 V Calculate the H* concentration.
For the cell shown, the measured cell potential, Ecell, is -0.3689 V at 25 °C. Pt(s)H,(g, 0.789 atm) | H(aq, ?M) || Cd²+ (aq, 1.00 M) Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 24 H, (g) E° = 0.00 V Cd²+ (aq) + 2e - Cd(s) E = -0.403 V Calculate the H+ concentration. [H+] =
Consider the two half reactions below: Sn^2+ + 2e^- rigntarrow Sn(s) E^0 = ____ ii) Fe^2+ + 2e^- rigntarrow Fe(s) E^0 = ____ Find E^0 values for these half reactions from your textbook or other reference, and record them in the spaces provided above. b) Based on the E^0 values, provide the reactions below for a galvanic cell half reactions. Anode half-reaction: Cathode half reaction: Net cell reaction: c) Calculate the E^0 cell for this. galvanic cell.
Anode E A Cathode B 7 С D Ni2+ + 2e -0.40 V Cd2+ + 2e -0.26 V Ni (s) Cd (s) Reduction Ni (8) Ereduction Cd (8) Ereduction Ni2+ (aq) Cd2+ (aq) Oxidation Salt Bridge Look at the voltaic cell diagram above and finish the following sentences using options given on the table above: i) Ais ii) B is metal on the left metal on the right solution on the left iii) Cis iv) Dis solution on the right...
3. (12 pt) Suppose that S is the subset of R2 that contains all vectors on the two lines y = x and y = -2 s={[x] € R: y=x or y = -x} ER2: y = r or y=- (a) In each of the following parts (i)-(iii), either show the statements is true or give a counterexample to show that the statement is false. Clearly state TRUE or FALSE. Graphs of y = x and y = -1 may...
Most questions answered within 3 hours.
-
The following base sequence is found for a mRNA fragment from
wild-type E. coli: 5'- UAUCAGUAGAUAAUGUAACC-3'...
asked 16 seconds from now -
For this exercise, round all regression parameters to three
decimal places.
One of the two tables...
asked 18 minutes ago -
What is the 5% level of significance for mean = 3.60, standard
deviation = 0.94, and...
asked 21 minutes ago -
Prior to beginning work on this discussion, please read the
article by Hayley Peterson, 15 Companies...
asked 50 minutes ago -
Which pair of aqueous solutions, when mixed, will form a
precipitate?
A) NaNO3 and AgC2H3O2
B)...
asked 1 hour ago -
1-Write an algorithm to get two numbers from the user (as
inputs) and calculate the sum...
asked 4 hours ago -
Define white-collar crime. What is the difference between
offender and offense-based definitions of white-collar crime? What...
asked 5 hours ago -
Consider a reaction which is 1st order with respect to A and 1st
order with respect...
asked 5 hours ago -
c++
The length of the hypotenuse of a right-angled triangle is the
square root of the...
asked 5 hours ago -
When a metal rod is heated, not only its resistance but also its
length and cross‐sectional...
asked 5 hours ago -
write a c++ program that computes the L^1 - Norm of a given
vector (L^1 norm...
asked 5 hours ago -
A manufacturer of banana chips would like to know whether its
bag filling machine works correctly...
asked 5 hours ago