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For the following electrochemical cell:

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Chemistry
3. The diagram shows an electrochemical cell with a gold strip (left) and aluminum glasses (right). In your response, do the following: • Label the cathode and the anode, including the charge on each. • Show the flow of electrons. • Describe what type of electrochemical ...

chemistry- electrochemical cell
What makes this an oxidation-reaction? 3Ag2S+2Al(s) -> Al2S3+6 Ag(s)? Write the half-reactions showing the oxidation and reduction reactions. Identify which is the oxidation reaction and which is the reduction reason. What is oxidized in the reaction? What is reduced? In ...

Chemistry
The diagram shows an electrochemical cell with a gold strip (left) and aluminum glasses (right). In your response, do the following: • Label the cathode and the anode, including the charge on each. • Show the flow of electrons. • Describe what type of electrochemical ...

chemistry
The reaction described by the equation Zn + Hg2Cl2 <--> 2Hg +Zn+2 + 2Cl is run on electrochemical cell. The E^0 of the cell at 25 degrees C is 1.03V. In the same cell, [Cl-]=.10 M and [Zn+2] is unknown, and the measured cell voltage is 1.21V. Compute the value of [Zn+2] ...

Chemistry
Electrochemisry. Candy Chemist wishes to determine the concentration of CrO4^2- by electrochemical means in solution, and subsequently the Ksp of Ag2CrO4. She sets up one half-cell comprised of the Ag+|Ag couple (E=+0.799V) and a second half-cell in which a silver elctrode is ...

Chemistry
For the following electrochemical cell, Co(s)/Co2(aq,.0155M)// Ag+(aq,2.50M)/Ag(s) 1.Write the net cell equation. 2.Calculate the following values at 25 degrees celcius. Eocell, Ecell, deltaGo rxn, and delta Grxn

Science
describe how a simple electrochemical cell operates? how are electrochemical cells related to batteries?

CHEMISTRY
The half-cell, Tl | Tl+(1 mol L-1), is connected to a Pt | H+ | H2(1 atm) half-cell in which the concentration of H+ is unknown. The measured cell voltage is 0.0841 V and the Pt | H2 | H+ half-cell is the cathode. Standard reduction potentials are given on the next page. (a) ...

CHEMISTRY
The half-cell, Tl | Tl+(1 mol L-1), is connected to a Pt | H+ | H2(1 atm) half-cell in which the concentration of H+ is unknown. The measured cell voltage is 0.0841 V and the Pt | H2 | H+ half-cell is the cathode. Standard reduction potentials are given on the next page. (a) ...

CHEMISTRY
The half-cell, Tl | Tl+(1 mol L-1), is connected to a Pt | H+ | H2(1 atm) half-cell in which the concentration of H+ is unknown. The measured cell voltage is 0.0841 V and the Pt | H2 | H+ half-cell is the cathode. Standard reduction potentials are given on the next page. (a) ...

CHEMISTRY HELP PLEASE!!!
The cell potential of the following electrochemical cell depends on the pH of the solution in the anode half-cell: Pt(s)|H2(g,1atm)|H+(aq,?M)||Cu^2+(aq,1.0M)|Cu(s) what is the pH of the solution if Ecell is 375 mV? I first got .65 as my pH, but it said that it was wrong. ...

Chemistry
Calculate the standard cell potential for each of the following electrochemical cells. Ni^+2(aq)+Mg(s)--->Ni(s)+Mg^+2(aq) I used the e cell values from the back of my book. They are: Ni^+2(aq)+2e--->Ni(s) E^0= -0.23 V Mg^+2(aq)+2e--->Mg(s) E^0= -2.37 I did E^0= -0.23...

Chemistry Cell notations
Enter the balanced chemical equation including states that describes the electrochemical cell that is represented by the cell notation as shown. Pt(s) l H2O(l) l O2(g) l H+(aq) ll H+(aq), Cr2O72-(aq), Cr3+(aq) l Pt(s)

chemistry (electrochemistry)
1) For the following electrochemical cell Cu(s)|Cu2 (aq, 0.0155 M)||Ag (aq, 1.50 M)|Ag(s) write the net cell equation. Calculate the following values using standard potentials as needed. Eo cell and dGo for each reaction...

Chemistry
Consider the following electrochemical cell: Al(s) | Al^3+(aq)(0.155 M) || H^(aq) (0.00233 M), MnO4^-(aq)(0.0377 M), Mn^2+(aq) (0.0168 M) | C (graphite) Write a balanced equation for the redox reaction taking place in this cell. i am having trouble with the cathode half reaction.

chemistry
The electrochemical cell described by the cell notation has a standard cell potential of -0.35 V. Calculate the Wmax (kJ) the cell has done if 1893.5 g of MnO42-(aq) (Molar Mass - 118.94 g/mol) forms. Round your answer to 3 significant figures. Pt(s) | Hg22+(aq), Hg2+(aq)||...

Chemistry Please help!!
An electrochemical cell that uses the reaction Ti^3+ + 2Cr^2+ -> Ti^1+ + 2Cr^3+ Has a standard cell potential of E¢ªcell = +1.19V a. Write the two half-cell reactions. b. Determine the E¢ªred(reduction).

Chemistry
An electrochemical cell is based on the following two half-reactions: Ox: Sn(s)--> Sn^2+(aq, 1.70 M)+ 2e Red: ClO2(g, 0.220 atm)+e --> ClO2^-(aq, 1.80 M) Compute the cell potential at 25 C. I think I'm supposed to use the Nernst Equation for this, but I do not know how ...

chemistry(check my steps)
The electrochemical cell described by the cell notation has a standard cell potential of -0.35 V. Calculate the Wmax (kJ) the cell has done if 1893.5 g of MnO42-(aq) (Molar Mass - 118.94 g/mol) forms. Round your answer to 3 significant figures. Pt(s) | Hg22+(aq), Hg2+(aq)||...

chemistry
Why is it that an electrochemical cell(galvanic cell) cannot operate forever?

Chemistry
Design an electrochemical cell using Pb(s) and Mn(s) and their solutions to answer the following questions. I just want to see if my answers are correct. I drew the cell already. Thanks 1. Give the line notation for this electrochemical cell. Mn(s) ∣ Mn2+(aq) ∥ Pb2...

analytical chemistry
Shown below is a diagram of an electrochemical cell. Write the shorthand, or schematic, notation for this cell

chemistry
A balanced equation that represents an overall cell reaction is shown. Choose the cell notation which corresponds to the electrochemical cell that is described by this equation. 2H2O(l) → 2H2(g) + O2(g) i don't get why the answer is this. How can OH- appear in both sides...

chemistry
Calculate Ecell forthe following electrochemical cell at 25 C Pt(s) |H2(g, 1.00 bar) |H + (aq, 1.00 M) || Pb2+(aq, 0.150 M) | Pb(s)

Chemistry- Electrochemistry
Calculate the activity of KI, x, in the following electrochemical cell if the potential is +0.294 V Ag | AgCl(s),NaCl(aq,0.1) ||KI(aq, x),I (s) | Pt

Chemistry
For the following electrochemical cell, what is the correct, balanced reaction? Cu(s) | Cu2+(aq) || Ag+(aq) | Ag(s) A. Cu(s) + Cu2+(aq) → Ag+(aq) + Ag(s) B. Cu(s) + Ag+(aq) → Cu2+(aq) + Ag(s) C. Cu(s) + 2 Ag+(aq) → Cu2+(aq) + 2 Ag(s) D. Cu2+(aq) + Ag(s) &#...

Chemistry
The reduction potentials for the species involved in an electrochemical cell are as follows: M+ + e– => M is 0.20 V J+ + e– => J is 1.00 V. All solutions are 1.00 M and J+ J is connected to M+ M What is E*cell (in V)? * is a 0. It stands for E not

Chemistry
The reduction potentials for the species involved in an electrochemical cell are as follows: M+ + e– => M is 0.20 V J+ + e– => J is 1.00 V. All solutions are 1.00 M and J+ J is connected to M+ M What is E*cell (in V)? * is a 0. It stands for E not

Chemistry
Provide the balanced reaction, the value of K, and E(cell) at equilibrium for the for the electrochemical cell created from the two half-cell reactions below Cr^(3+) + e ==> Cr^(2+) Fe^(2+) + 2e ==> Fe Well, I got the balanced reaction: 2Cr^(2+) + Fe^(2+) ==> Fe + 2Cr...

science
What energy changes occur in an electrochemical cell when electric current flows from it? This is what I put down but I am not sure if it is right... In a primary cell, chemical reactions use up some of the materials in the cell as electrons flow from it. This causes an energy...

Chemistry
Consider an electrochemical cell based on the following cell diagram: Pt | Pu3+(aq), Pu4+(aq) || Cl2(g), Cl−(aq) | Pt Given that the standard cell emf is 0.35 V and that the standard reduction potential of chlorine is 1.36 V, what is the standard reduction potential E°(...

Chemistry
Write the equations describing the electrode reactions and the net cell reaction for this electrochemical cell containing tin and silver: Sn(s)|Sn2 (aq)||Ag (aq)|Ag(s) what is the equation for cathode, anode, and net cell reaction

Chemistry
Write the equations describing the electrode reactions and the net cell reaction for this electrochemical cell containing tin and silver: Sn(s)|Sn2 (aq)||Ag (aq)|Ag(s) what is the equation for cathode, anode, and net cell reaction

chemistry
an electrochemical cell uses Al and Al+3 in one compartment and Ag and Ag+ in the other write a balanced equation for the rxn that will occur spontaneously in this cell would that just be Al + Al+3 + 2e --> Ag + Ag+ ?

Chemistry
1)) The following two half-cells are paired up in a voltaic cell. How will lowering the pH affect the E of the overall cell? ClO3-(aq) + H2O(l) + 2e- ==> ClO2-(aq) + 2OH-(aq) Eo= 0.35 V I2(S) + 2e-==> 2I-(aq) Eo = 0.54 V A)dE will increase B)dE will decrease C)dE...

chemistry
1)) The following two half-cells are paired up in a voltaic cell. How will lowering the pH affect the E of the overall cell? ClO3-(aq) + H2O(l) + 2e- ==> ClO2-(aq) + 2OH-(aq) Eo= 0.35 V I2(S) + 2e-==> 2I-(aq) Eo = 0.54 V A)dE will increase B)dE will decrease C)dE...

chemistry
Answer the following questions based on the following electrochemical reaction: Al(s) + Cu 2+(aq) <====> Cu(s) + Al3+ (aq) Write the balanced chemical equation for this cell. I'm confused.. how would this be balanced?

chemistry
Give the cell diagram notation of the electrochemical cell that could be used to determine experimentally the dissociation constant (Kw) of water. The standard reduction potential for: O2 + 2H20 + 4e- ---------> 4 OH- 0.40 V

chemistry
The electrochemical cell described by the cell notation has a standard emf (electromotive force) of -0.68 V. Calculate the value (kJ) for the standard free energy change of the cell. Round your answer to 3 significant figures. Pt(s) l MnO2(s) l MnO4-(aq), H+(aq) ll H+(aq), VO2...

chemistry
I did a lab using an electrochemical cell to establish a relationship between cell potential and concentration. I derived two equations from lines of best fit. One is Cell potential of Ag vs. Cu Concentration: y = -0.04520x+0.5515. The other is cell potential of Zn vs. Cu ...

CHEMISTRY
The two half-reactions for the LeClanche dry cell battery are shown below. Describe the direction of spontaneous electron flow in this electrochemical cell. Zn(s) ---> Zn2+(aq) + 2e- 2NH4+(aq) + 2e- ---> 2NH3(g) + H2(g)

Chemistry
An electrochemical cell that uses the reaction Ti^3+ + 2Cr^2+ -> Ti^1+ + 2Cr^3+ Has a standard cell potential of E¢ªcell = +1.19V a. Write the two half-cell reactions. b. Labeling all parts and show the direction of flow of electrons. (Place the anode electrode on the ...

Chemistry
How would you start and finish these questions by a step by step process? Does Amp equal to Joules? 1. How many grams of aluminum can be produced by the electrolysis of aqueous aluminum chloride by a current of 5.00 amps for 5.00 hours? 2. Consider the following ...

chemistry
Calculate the standard cell potential for each of the electrochemical cells? 2Ag+(aq)+Pb(s)→2Ag(s)+Pb2+(aq) E∘cell......V? 2ClO2(g)+2I−(aq)→2ClO−2(aq)+I2(s) E∘cell......V? O2(g)+4H+(aq)+2Zn(s)→2H2O(l)+2Zn2+(aq) E∘cell......V?

Chemistry --Need Help!!
Ive posted twice, but no one's answered yet...I could really use any kind of guidance--particularly for the 1st question :) 1)) The following two half-cells are paired up in a voltaic cell. How will lowering the pH affect the ƒ´E of the overall cell? ClO3-(aq) + H2O(l) + 2e...

Chemistry
For the following electrochemical cell Cu(s)|Cu2 (aq, 0.0155 M)||Ag (aq, 3.50 M)|Ag(s) write the net cell equation. I presume it is Cu + 2Ag^2+ --> Cu2+ + 2Ag Calculate the following values at 25.0 C using standard potentials as needed. Eocell = ? dGorxn = ? Ecell = ? dGrxn...

General Chem - Electrochemistry
Give the cell diagram notation of the electrochemical cell that could be used to determine experimentally the dissociation constant (Kw) of water. The standard reduction potential for O2 + H20 + 4 e- ----> 4OH- is 0.40 V For other possible half-reactions, see your textbook...

chemistry
Consider an electrochemical cell based on the reaction: 2H+(aq) + Sn(s) = Sn2+(aq) + H2(g). Which of the following actions would NOT change the measured cell potential? lowering the pH in the cathode compartment addition of more tin metal to the anode compartment any of the ...

chemistry
Consider an electrochemical cell based on the reaction: 2H+(aq) + Sn(s) = Sn2+(aq) + H2(g). Which of the following actions would NOT change the measured cell potential? lowering the pH in the cathode compartment addition of more tin metal to the anode compartment any of the ...

Inorganic chemistry
The following electrochemical cell has the potential of +0.617V at 25 degrees Celsius Pt ! H2(g, 1.00 atm) ! H+ (aq, 1.00M !! Ag^+(aq) ! Ag The standard reduction potential, E naught, of Ag^+ = 0.799V. What is the Ag+ concentration?

Chemistry2
An electrochemical cell is created using gold and magnesium half-cells. a. Determine which half-cell will undergo oxidation and which will undergo reduction, identify anode and cathode, and calculate the voltage for the cell. You do not need to diagram the cell. b. If the mass...

Chemistry
An electrochemical cell is created using gold and magnesium half-cells. a. Determine which half-cell will undergo oxidation and which will undergo reduction, identify anode and cathode, and calculate the voltage for the cell. You do not need to diagram the cell. b. If the mass...

Chemistry
Calculate the standard cell potential for each of the electrochemical cells? What would the answers be to something like this? If someone could work out the answer I would really appreciate it. My online hw keeps telling me its wrong. 2Ag+(aq)+Pb(s)→2Ag(s)+Pb2+(aq) E&#...

Chemistry
Calculate the standard cell potential for each of the electrochemical cells? What would the answers be to something like this? If someone could work out the answer I would really appreciate it. My online hw keeps telling me its wrong. 2Ag+(aq)+Pb(s)→2Ag(s)+Pb2+(aq) E&#...

Chemistry
Calculate the cell potential for the electrochemical cell consisting of Ag metal in a 0.500 M AgNO3 solution and Fe metal in a 3.0 M Fe(NO3)3 solution.

Chemistry
Calculate the electrical voltage of an electrochemical cell using Pb(s) and Co(s) as electrodes along with their appropriate solutions. Co2+(aq) + 2e- --> Co(s) -0.28 V Pb2+(aq) + 2e- --> Pb(s) -0.13 V The oxidation reaction is Co(s) --> Co2+(aq) + 2e- +0.28V E0 net(...

Chemistry
Determine the potential (in V) of an electrochemical cell using a gold electrode and gold (III) [0.0243 M] solution in combination with a manganese/manganese (II) [0.00567 M] half cell How on earth would I do this question? I just know Au(3+) + 3e- = Au and E = 1.22 V

chemistry
The electrochemical cell described by the cell notation has an Eo of -0.37 V. Calculate the maximum electrical work (kJ) the cell has done if 331.73 g of Cu(s) (Molar Mass - 63.55 g/mol) reacts. Round your answer to 3 significant figures. Cu(s) l Cu+(aq) ll Sn4+(aq), Sn2+(aq) ...

chemistry
The electrochemical cell described by the cell notation has an Eo of -0.37 V. Calculate the maximum electrical work (kJ) the cell has done if 331.73 g of Cu(s) (Molar Mass - 63.55 g/mol) reacts. Round your answer to 3 significant figures. Cu(s) l Cu+(aq) ll Sn4+(aq), Sn2+(aq) ...

chemistry
The electrochemical cell described by the cell notation has an Eo of -0.37 V. Calculate the maximum electrical work (kJ) the cell has done if 331.73 g of Cu(s) (Molar Mass - 63.55 g/mol) reacts. Round your answer to 3 significant figures. Cu(s) l Cu+(aq) ll Sn4+(aq), Sn2+(aq) ...

chemistry
Write the equations describing the electrode reactions and the net cell reaction for this electrochemical cell containing indium and cadmium: This is what I have so far: anode: In(s) --> In^3+ + 3e- cathode: Cd^2+ + 2e- --> Cd (s) Need help writing the balanced net ...

Chemistry
The electrochemical cell described by the balanced chemical equation has a standard emf (electromotive force) of -0.35 V. Calculate the value (J) for the Wmax that the cell can do under standard conditions. Round your answer to 3 significant figures. 2MnO4-(aq) + Hg22+(aq) &#...

chemistry
2. The voltage of an electrochemical cell depends on the redox reaction occurring in the cell. Given a redox reaction below: Zn(s) + Pb2+(aq) --> Zn2+(aq) + Pb(s) Pb2+(aq) + 2 e--->Pb(s)Eº = -0.13V Zn2+(aq) + 2 e--->Zn(s)Eº = -0.76V Calculate the E.M.F (Voltage) of ...

chemistry
The voltage of an electrochemical cell depends on the redox reaction occurring in the cell. Given a redox reaction below: Zn(s) + Pb2+(aq) --> Zn2+(aq) + Pb(s) Pb2+(aq) + 2 e--->Pb(s)Eº = -0.13V Zn2+(aq) + 2 e--->Zn(s)Eº = -0.76V Calculate the E.M.F (Voltage) of the...

chemistry
Base your answer on the following redox reaction, which occurs spontaneously in an electrochemical cell. Zn + Cr3+ --> Zn2+ + Cr Write the half-reaction for the reduction that occurs.

c
The voltage of an electrochemical cell depends on the redox reaction occurring in the cell. Given a redox reaction below: Zn(s) + Pb2+(aq) --> Zn2+(aq) + Pb(s) Pb2+(aq) + 2 e--->Pb(s)Eº = -0.13V Zn2+(aq) + 2 e--->Zn(s)Eº = -0.76V Calculate the E.M.F (Voltage) of the...

Chem 1LC
Could someone please help me with this problem!!?!? Thanks you so much!!! The reduction potentials for the species involved in an electrochemical cell are as follows: M+ + e– M is 0.50 V J+ + e– J is 1.20 V. All solutions are 1.00 M and J+ J is connected to M+ M. A) What ...

Chemistry - Cell Notation
Enter the balanced chemical equation including states that describes the electrochemical cell that is represented by the cell notation as shown. Pt(s) | F-(aq) | F2(g) || Cl-(aq), AuCl4-(aq) | Au(s) I'm having trouble balancing this... I get AuCl4- + 2F- --> Au + 4Cl- + F2...

Science
Were can i find a coloured diagram of a aluminum-nickel electrochemical cell?

Chemistry
Zn (0.85M) + Cu (1.10M) in an electrochemical cell. what is the conc of the zinc ion?

Inorganic chemistry
Calc1ulate E for the following electrochemical cell at 25 degrees Celsius Pt(s) ! Sn^2+ (aq, 0.50M), S^4+(aq, 0.50M !!I^-(aq, 0.15M) ! AgI(s) ! Ag(s)! given the following standard reduction potentials. AgI(s) = e^- ==> Ag(s) + I^-(aq) E naught = -0.15V Sn^4+(aq) + 2e^- ==&...

College Chemistry (DrBob222)
Use the Nernst equation to calculate the iron (II) concentration for the following iron/copper electrochemical cell when [Cu2+] = 0.012 M and Ecell = 0.750 V at 35°C. Cu2+ (aq) + Fe (s) --> Cu (s) + Fe2+ (aq)

chemistry
The electrochemical cell described by the cell notation has an Eo of -0.37 V. Calculate the maximum electrical work (kJ) the cell has done if 331.73 g of Cu(s) (Molar Mass - 63.55 g/mol) reacts. Round your answer to 3 significant figures. Cu(s) l Cu+(aq) ll Sn4+(aq), Sn2+(aq) ...

chemistry
Discuss the spontaneity of an electrochemical reaction in terms of its standard emf (E¨¬cell)

AP Chemistry
A voltaic cell is constructed that uses the following half-cell reactions. Cu+(aq) + e- Cu(s) I2(s) + 2 e- 2 I -(aq) The cell is operated at 298 K with [Cu+ ] = 2.3 M and [I - ] = 3.3 M. (a) Determine E for the cell at these concentrations. (b) If [Cu+ ] were equal to 1.0 M, ...

AP Chemistry
A voltaic cell is constructed that uses the following half-cell reactions. Cu+(aq) + e- Cu(s) I2(s) + 2 e- 2 I -(aq) The cell is operated at 298 K with [Cu+ ] = 2.3 M and [I - ] = 3.3 M. (a) Determine E for the cell at these concentrations. (b) If [Cu+ ] were equal to 1.0 M, ...

Chemistry
Hi, if anyone can give me help for any part of the question that would be great! I know how to draw the cell diagram, but am not sure what the half-reactions would be.... Here is the question: Give the cell diagram notation of the electrochemical cell that could be used to ...

chemistry
A balanced equation that represents an overall cell reaction is shown. Choose the cell notation which corresponds to the electrochemical cell that is described by this equation. a) Sn2+(aq) + 2Cu+(aq) → Sn4+(aq) + 2Cu(s) b) Pt(s) l Sn2+(aq), Sn4+(aq) ll Cu+(aq) l Cu(s) c...

chem 1046
An electrochemical cell is based on these two half-reactions: Ox: Sn(s) → Sn2+(aq, 1.74 M) + 2 e- Red: ClO2(g, 0.120 atm) + e- → ClO2-(aq, 1.44 M) Calculate the cell potential at 25°C E Sn>Sn2+ = -.14 E ClO2 = .95

Chem 1046
An electrochemical cell is based on these two half-reactions: Ox: Sn(s) → Sn2+(aq, 1.74 M) + 2 e- Red: ClO2(g, 0.120 atm) + e- → ClO2-(aq, 1.44 M) Calculate the cell potential at 25°C E Sn>Sn2+ = -.14 E ClO2 = .95

Analytical Chem
The following electrochemical cell can be used to calculate the formation constant Kf for a metal and EDTA. The cell has a voltage of -0.262V. The right half cell contains a metal (M^2+) with a standard reduction potential of -0.236V. Calculate the Kf for the metal EDTA ...

Chemistry
The part of an electrochemical cell that carries electrons to a reacting ion is a(n) (1) cathode (2) anode (3) electrode (4) electrolyte

AP Chemistry
Q - An electrochemical reaction occurs between an unknown element and zinc. The half-cell reaction for the zinc is: Zn(s) → Zn2+(aq) + 2e− The cell potential for the reaction is Eºcell = 1.83 V. Is the reaction spontaneous or nonspontaneous? Explain. What is the ...

chemistry
The electrochemical cell described by the balanced chemical equation has a standard emf (electromotive force) of -4.05 V. Calculate the maximum electrical work (kJ) the cell has done if 6.8500 mol of F2(g) (Molar Mass - 38.00 g/mol) forms. Round your answer to 3 significant ...

AP Chemistry
Q - An electrochemical reaction occurs between an unknown element and zinc. The half-cell reaction for the zinc is: Zn(s) → Zn2+(aq) + 2e− The cell potential for the reaction is Eºcell = 1.83 V. Is the reaction spontaneous or nonspontaneous? Explain. What is the half-cell...

Science
Please compare and contrast the electrochemical events involved in the initiation and propagation of an action potential with the electrochemical events involved with the initiation of muscle contraction in skeletal muscle. Be sure to describe the electrochemical changes in ...

CHEM
1.) What is the correct net cell reaction for the electrochemical cell diagramed below? Ni(s) ∣ Ni2+(aq) || Ag+(aq) ∣ Ag(s) a.) Ag+(aq) + Ni(s) ---> Ag(s) + Ni2+(aq) b.) Ag(s) + Ni2+(aq) ---> Ag+(aq) + Ni(s) c.) 2Ag+(aq) + Ni(s) ---> 2 Ag(s) + Ni2+(aq) d...

chemistry, please help
say that I measured the voltage of electrochemical cells: Zn/Cu: -0.961 V Pb/Cu: -0.360 V Ag/Cu: 0.425 V Sn/Cu: -0.275 V Fe/Cu:-0.516 V Directions: If you assign Cu an arbitrary electrode potential value of 0.00 V, the numbers above are the reduction potentials for the other ...

Chemistry
The first electrochemical cell was invented by ____. Michael Faraday Alessandro Volta*** James Maxwell Benjamin Franklin

chemisry.Electrochemical Measurement of Concentrat
A calibration curve to show how the cell potential varies with [Cu2+] may be constructed. A plot of cell potential (in V, with the same sense as in question 1) versus log10[Cu2+] should yield a straight line. What is the slope of this line? The answer should be -0.0591/2 but ...

Chemistry
3. An electrochemical reaction occurs between an unknown element and zinc. The half-cell reaction for the zinc is: Zn(s) → Zn2+(aq) + 2e− The cell potential for the reaction is Eºcell = 1.83 V. a. Is the reaction spontaneous or nonspontaneous? Explain. (1 point) b...

College Chemistry
A Galvanic cell consists of Mg electrode in a 1.0 mol L -1 Mg(NO3)2 solution and a Ag electrode in a 1.0 mol L-1 AgNO3 solution. Calculate standard emf for the spontaneous reaction of this electrochemical cell at 25 C, given that the standard reduction potential Eo for Ag+ is...

Chem
The electrochemical cell described by the balanced chemical equation has a standard emf of -0.25 V. Calculate the value (kJ) for the ΔG˚ of the cell. Round your answer to 3 significant figures. MnO2(s) + Pb2+(aq) → Mn2+(aq) + PbO2(s) St. Red. Pot. (V) PbO2/Pb2...

chemistry
Which of the following half-reactions would occur at the anode of an electrochemical cell? A. H+(aq) + Cl− (aq) → HCl(aq) B. Li+(aq) + e− → Li(s) C. Cu+(aq) + e− → Cu(s) D. Cu(s) → Cu+(aq) + e−

chemistry
need help drawing an electrochemical cell that could be used to plate zinc onto other metals.labeling cathode and anode, and reactions that occur.

Chem Check Please!!!
Calculate for the electrochemical cell below, Ag(s) | AgCl(s) | Cl–(aq) || Cu2+(aq) | Cu(s) given the following standard reduction potentials. Cu2+(aq) + 2 e– -> Cu(s) E = +0.337 V AgCl(s) + e– -> Ag(s) + Cl–(aq) E = +0.222 V a. –0.115 V b. –0...

Chemistry
The following galvanic cell at standard conditions has a potential of 0.03 V: Ag+(aq) + Fe2+(aq) → Fe3+(aq) + Ag(s). What would be the effect of increasing the concentration of Ag+? A. The cell potential will decrease. B. The cell potential will increase. C. The cell ...

Chemistry
The following galvanic cell at standard conditions has a potential of 0.03 V: Ag+(aq) + Fe2+(aq) → Fe3+(aq) + Ag(s). What would be the effect of increasing the concentration of Ag+? A. The cell potential will decrease. B. The cell potential will increase. C. The cell ...

AP CHEMISTRY
A voltaic cell is constructed that uses the following half-cell reactions. Cu+(aq) + e− -> Cu(s) I2(s) + 2 e− -> 2 I−(aq) The cell is operated at 298 K with [Cu+ ] = 2.7 M and [I− ] = 2.7 M. (a) Determine E for the cell at these concentrations. (b...

AP CHEMISTRY
A voltaic cell is constructed that uses the following half-cell reactions. Cu+(aq) + e− -> Cu(s) I2(s) + 2 e− -> 2 I−(aq) The cell is operated at 298 K with [Cu+ ] = 2.7 M and [I− ] = 2.7 M. (a) Determine E for the cell at these concentrations. (b...

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