Please give the correct answer for (e) the last problem
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E) If the cell potential as measured is 1.04 volts, what would be the reduction potential associa...
The reduction potential for the following non-standard half cell at 298K is volts. 24+ (1.83x10-3M) +...
The reduction potential for the following non-standard half cell at 298K is volts. 24+ (1.83x10-3M) + 2e —>H2 (1.68atm) The reduction potential for the following non-standard half cell at 298K is volts. Al3+ (4.93x10-*M)+ 3e —AI (S) What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the F2 pressure is 6.44x10 atm, the F concentration is 1.41M, and the Ni2+ concentration is 1.28M? F2(g) + Ni(s)— 2F" (aq) +...
please help the standrad reduction provided down What is the calculated value of the cell potential...
please help the standrad reduction provided down
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cu2+ concentration is 9.24x10 + M and the Cr3+ concentration is 1.47 M? 3Cu2+ (aq) + 2Cr(s) Answer: 3Cu(s) + 2Cr +(aq) v The cell reaction as written above is spontaneous for the concentrations given: What is the calculated value of the cell potential at 298K for an electrochemical cell with the...
Knowing that the standard reduction potential, E half-cell is +0.34V of the Cu'jCu(s) (or knowing that...
Knowing that the standard reduction potential, E half-cell is +0.34V of the Cu'jCu(s) (or knowing that the standard oxidation potential, Eoo of the Cu(s)]Cu* or knowing that the standard oxidation potential, E )u half-cell is -0.34 V), what is the potential of the nickel half-cell? Is this Ed or E hat is the potential of the nickel half-cell? Is this E, or E. red 8. What is the standard reduction potential (SRP, Eond) of the Ni2 |Ni(s) halfcell? What is...
Enter electrons as e A voltaic cell is constructed in which the anode is a Ni...
Enter electrons as e A voltaic cell is constructed in which the anode is a Ni Ni2+ half cell and the cathode is a Hg|Hg2+ half cell. The half-cell compartments are connected by a salt bridge. (Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: + + The cathode reaction is: + V> + The net cell reaction is:...
A galvanic cell using Ni2+(aq) / Ni(s) half-cell and Hg22+(aq) / Hg(l) half-cell is prepared. The...
A galvanic cell using Ni2+(aq) / Ni(s) half-cell and Hg22+(aq) / Hg(l) half-cell is prepared. The E°nickel = -0.25 V and E°mercury = 0.789 V. (blank 1) Write the balanced reaction that occurs at the anode. (blank 2) Write the balanced reaction that occurs at the cathode. (blank 3) Calculate the standard cell potential of this galvanic cell. (blank 4) Write the shorthand cell notation for the galvanic cell. Question 10 options: Blank # 1 Blank # 2 Blank #...
A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are connec...
A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are connected by a salt bridge. Hg2+ (aq) + 21 (aq) – Hg(l) +12(5) The anode reaction is: The cathode reaction is: In the external circuit, electrons migrate - the 1"12 electrode - the Hg/Hg2+ electrode. In the salt bridge, anions migrate - the I'll compartment the Hg/Hg2+ compartment. A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are...
If the standard reduction potential for A --> A+ + e- was 1.21 volts and the...
If the standard reduction potential for A --> A+ + e- was 1.21 volts and the standard reduction potential for B --> B+2 + 2 e- was 0.46 volts, what would be the standard potential for the following reaction: B+2 + 2 A --> 2 A+ + B? If the standard reduction potential for X --> X+2 + 2 e- was 0.53 volts and the standard potential for the reaction: X + Y+2 --> X+2 + Y was 0.4 volts,...
Given the half reactions below, what would be the standard cell potential (E° cell) in volts...
Given the half reactions below, what would be the standard cell potential (E° cell) in volts for the reaction below? (Report answer with 2 decimal places) 2 Cr3+ (aq)+3 Mn (s) 3 Cr (s) +3 Mn2+ (aq) Cr3+ (aq) +3 e Cr (s) Eored0.50 V Mn2+ (aq) 2 e-Mn (s) E red -1.18 v
Consider the following electrochemical cell at room temperature. 1.05 V N м Salt Bridge Ni2+an (110...
Consider the following electrochemical cell at room temperature. 1.05 V N м Salt Bridge Ni2+an (110 The half cell and the reuction potential for the anode is: Half-Reaction E (V) Ni2+ (aq) + 2e ® Ni(s) -0.25 Using this information from the diagram, determine the standard reduction potential of metal M. +0.25 V O-1.40V +0.80 v -0.80 V +1.40 V
Use measured cell potential to calculate concentration. When [ Hg2+ ]=1.35 M, the observed cell potential at 298K for a...
Use measured cell potential to calculate concentration. When [ Hg2+ ]=1.35 M, the observed cell potential at 298K for an electrochemical cell with the reaction shown below is 2.582 V. What is the Al** concentration in this cell? 3 Hg2+ (aq) + 2 Al (s) — 3 Hg (1) + 2 A1+ (aq) [A13+]= M
The reduction potential for the following non-standard half cell at 298K is volts. 24+ (1.83x10-3M) + 2e —>H2 (1.68atm) The reduction potential for the following non-standard half cell at 298K is volts. Al3+ (4.93x10-*M)+ 3e —AI (S) What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the F2 pressure is 6.44x10 atm, the F concentration is 1.41M, and the Ni2+ concentration is 1.28M? F2(g) + Ni(s)— 2F" (aq) +...
please help the standrad reduction provided down
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cu2+ concentration is 9.24x10 + M and the Cr3+ concentration is 1.47 M? 3Cu2+ (aq) + 2Cr(s) Answer: 3Cu(s) + 2Cr +(aq) v The cell reaction as written above is spontaneous for the concentrations given: What is the calculated value of the cell potential at 298K for an electrochemical cell with the...
Knowing that the standard reduction potential, E half-cell is +0.34V of the Cu'jCu(s) (or knowing that the standard oxidation potential, Eoo of the Cu(s)]Cu* or knowing that the standard oxidation potential, E )u half-cell is -0.34 V), what is the potential of the nickel half-cell? Is this Ed or E hat is the potential of the nickel half-cell? Is this E, or E. red 8. What is the standard reduction potential (SRP, Eond) of the Ni2 |Ni(s) halfcell? What is...
Enter electrons as e A voltaic cell is constructed in which the anode is a Ni Ni2+ half cell and the cathode is a Hg|Hg2+ half cell. The half-cell compartments are connected by a salt bridge. (Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: + + The cathode reaction is: + V> + The net cell reaction is:...
A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are connected by a salt bridge. Hg2+ (aq) + 21 (aq) – Hg(l) +12(5) The anode reaction is: The cathode reaction is: In the external circuit, electrons migrate - the 1"12 electrode - the Hg/Hg2+ electrode. In the salt bridge, anions migrate - the I'll compartment the Hg/Hg2+ compartment. A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are...
Given the half reactions below, what would be the standard cell potential (E° cell) in volts for the reaction below? (Report answer with 2 decimal places) 2 Cr3+ (aq)+3 Mn (s) 3 Cr (s) +3 Mn2+ (aq) Cr3+ (aq) +3 e Cr (s) Eored0.50 V Mn2+ (aq) 2 e-Mn (s) E red -1.18 v
Consider the following electrochemical cell at room temperature. 1.05 V N м Salt Bridge Ni2+an (110 The half cell and the reuction potential for the anode is: Half-Reaction E (V) Ni2+ (aq) + 2e ® Ni(s) -0.25 Using this information from the diagram, determine the standard reduction potential of metal M. +0.25 V O-1.40V +0.80 v -0.80 V +1.40 V
Use measured cell potential to calculate concentration. When [ Hg2+ ]=1.35 M, the observed cell potential at 298K for an electrochemical cell with the reaction shown below is 2.582 V. What is the Al** concentration in this cell? 3 Hg2+ (aq) + 2 Al (s) — 3 Hg (1) + 2 A1+ (aq) [A13+]= M
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