Voltaic cells chemistry
please help with A-C, H and I.
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Voltaic cells chemistry
please help with A-C, H and I.
3. A voltaic cell is built...
A voltaic cell consists of two half-cells. One half-cell contains a chromium electrode immersed in 1.00...
A voltaic cell consists of two half-cells. One half-cell contains a chromium electrode immersed in 1.00 M Cr(NO3)3 solution. The second half-cell contains a cobalt electrode immersed in 1.00 M Co(NO3)2 solution. Cobalt plates out on the cobalt electrode as the voltaic cell runs. The beginning voltage of the cell is +0.467 V at 25°C. The standard electrode potential (standard reduction potential) of chromium at 25°C is −0.744 V. (a) Write a balanced half-reaction equation for the reaction occurring at...
A voltaic cell consists of two half-cells. One half-cell contains a chromium electrode immersed in 1.00...
A voltaic cell consists of two half-cells. One half-cell contains a chromium electrode immersed in 1.00 M Cr(NO3)3 solution. The second half-cell contains a nickel electrode immersed in 1.00 M NI(NO3)2 solution. Nickel plates out on the nickel electrode as the voltaic cell runs. The beginning voltage of the cell is +0.487 V at 25°C. The standard electrode potential (standard reduction potential) of chromium at 25°C is -0.744 V. (a) Write a balanced half-reaction equation for the reaction occurring at...
I need help on 2. Sketch a voltaic cell based on the following reaction. (a) show...
I need help on 2.
Sketch a voltaic cell based on the following reaction. (a) show the direction of electron flow and the direction of ion migration: (b) identify the cathode and anode: (c) state the signs of the cathode and anode: (d) give the overall balanced reaction. (e) Write the half-reactions that occur in the two electrode compartments. (f) Calculate E degree, assume 25 degree C: (g) Write a cell diagram for the cell: (h) Calculate E when [Cr^3+]...
A voltaic cell contains two half-cells. One half-cell contains a chromium electrode immersed in a 1.00...
A voltaic cell contains two half-cells. One half-cell contains a chromium electrode immersed in a 1.00 M Cr(NO_3)_3 solution. The second half-cell contains a nickel electrode immersed in a 1.00 M Ni(NO_3)_2 solution. Cr^3+(aq) + 3 e^- rightarrow Cr(s) E_red^degree = 0.744 V Ni^2+(aq) + 2e^- rightarrow Ni(s) E_red^degree = -0.257 V Using the standard reduction potentials given above, predict the standard cell potential of the voltaic cell. Write the overall balanced equation for the voltaic cell. (Include states-of-matter under...
Consider a voltaic (galvanic) cell with the following metal electrodes. Identify which metal is the cathode...
Consider a voltaic (galvanic) cell with the following metal electrodes. Identify which metal is the cathode and which is the anode, and calculate the cell potential. (Use the table of Standard Electrode Potentials.) (a) Ca(II) and Sc(III) Cathode: . Ca(II) Sc(III) Anode: Ca(II) Sc(III) Ecell = 0.0591 x V (b) Pb(II) and In(III) Cathode: . Pb(II) In(III) Anode: Pb(II) In(III) Ecell - (c) Ni(II) and Zr(IV) Cathode: NI(II) Zr(IV) Anode: Ni(II) Zr(IV) Ecell - V Supporting Materials Periodic Table Supplemental...
Enter electrons as e. A voltaic cell is constructed in which the anode is a Cr...
Enter electrons as e. A voltaic cell is constructed in which the anode is a Cr Cr3+ half cell and the cathode is a SnSn2+ 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: The net cell reaction is: + + In the external...
A) B) C) C) Enter electrons as e. A voltaic cell is constructed in which the...
A) B)
C)
C)
Enter electrons as e. A voltaic cell is constructed in which the anode is a CuCu2+ half cell and the cathode is a II, 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: The net cell reaction is: In the...
The following problems are based upon the following voltaic cell (concentration of aqueous solutions are 1...
The following problems are based upon the following voltaic cell (concentration of aqueous solutions are 1 M): (Show all work for full credit.) Fe (s) Fe" (aq) | |Cu (aq) | Cu (s) (3) 1. The reduction potential for the iron half reaction is -0.040 v. Use your textbook to determine the reduction potential for the copper half reaction, and record that here. )2. From the voltaic cell written above, which half cell will be the anode, and which will...
The following problems are based upon the following voltaic cell (concentration of aqueous solutions are 1...
The following problems are based upon the following voltaic cell (concentration of aqueous solutions are 1 M): (Show all work for full credit.) Cr(s) c (aq) IlCut (aq) Cu (s) (3) I. From the voltaic cell written above, which half cell will be the anode, and which will be the cathode? Why? (3) 2. Write a balanced equation describing the redox reaction in this cell. (Molecular or Net lonic equation is correct) (2) 3. How many electrons are transferred in...
post lab queations help A voltaic cell consists of a Sn/Sn? half-cell and a Cr/Cr half-cell...
post lab queations help
A voltaic cell consists of a Sn/Sn? half-cell and a Cr/Cr half-cell at 25 °C. The initial concentrations of Snow and Creare 0.10 M and 0.30 M respectively. Standard reduction potentials are as follows: Sn + 2e → Sn, E = -0.14 V; C* + 3e → Cr, E = -0.76 V 1. Which is the anode, which is the cathode? 2. What is the value of E'cell? 3. What is the value of Q, the...
A voltaic cell consists of two half-cells. One half-cell contains a chromium electrode immersed in 1.00 M Cr(NO3)3 solution. The second half-cell contains a nickel electrode immersed in 1.00 M NI(NO3)2 solution. Nickel plates out on the nickel electrode as the voltaic cell runs. The beginning voltage of the cell is +0.487 V at 25°C. The standard electrode potential (standard reduction potential) of chromium at 25°C is -0.744 V. (a) Write a balanced half-reaction equation for the reaction occurring at...
I need help on 2.
Sketch a voltaic cell based on the following reaction. (a) show the direction of electron flow and the direction of ion migration: (b) identify the cathode and anode: (c) state the signs of the cathode and anode: (d) give the overall balanced reaction. (e) Write the half-reactions that occur in the two electrode compartments. (f) Calculate E degree, assume 25 degree C: (g) Write a cell diagram for the cell: (h) Calculate E when [Cr^3+]...
A voltaic cell contains two half-cells. One half-cell contains a chromium electrode immersed in a 1.00 M Cr(NO_3)_3 solution. The second half-cell contains a nickel electrode immersed in a 1.00 M Ni(NO_3)_2 solution. Cr^3+(aq) + 3 e^- rightarrow Cr(s) E_red^degree = 0.744 V Ni^2+(aq) + 2e^- rightarrow Ni(s) E_red^degree = -0.257 V Using the standard reduction potentials given above, predict the standard cell potential of the voltaic cell. Write the overall balanced equation for the voltaic cell. (Include states-of-matter under...
Consider a voltaic (galvanic) cell with the following metal electrodes. Identify which metal is the cathode and which is the anode, and calculate the cell potential. (Use the table of Standard Electrode Potentials.) (a) Ca(II) and Sc(III) Cathode: . Ca(II) Sc(III) Anode: Ca(II) Sc(III) Ecell = 0.0591 x V (b) Pb(II) and In(III) Cathode: . Pb(II) In(III) Anode: Pb(II) In(III) Ecell - (c) Ni(II) and Zr(IV) Cathode: NI(II) Zr(IV) Anode: Ni(II) Zr(IV) Ecell - V Supporting Materials Periodic Table Supplemental...
Enter electrons as e. A voltaic cell is constructed in which the anode is a Cr Cr3+ half cell and the cathode is a SnSn2+ 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: The net cell reaction is: + + In the external...
A) B)
C)
C)
Enter electrons as e. A voltaic cell is constructed in which the anode is a CuCu2+ half cell and the cathode is a II, 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: The net cell reaction is: In the...
The following problems are based upon the following voltaic cell (concentration of aqueous solutions are 1 M): (Show all work for full credit.) Fe (s) Fe" (aq) | |Cu (aq) | Cu (s) (3) 1. The reduction potential for the iron half reaction is -0.040 v. Use your textbook to determine the reduction potential for the copper half reaction, and record that here. )2. From the voltaic cell written above, which half cell will be the anode, and which will...
The following problems are based upon the following voltaic cell (concentration of aqueous solutions are 1 M): (Show all work for full credit.) Cr(s) c (aq) IlCut (aq) Cu (s) (3) I. From the voltaic cell written above, which half cell will be the anode, and which will be the cathode? Why? (3) 2. Write a balanced equation describing the redox reaction in this cell. (Molecular or Net lonic equation is correct) (2) 3. How many electrons are transferred in...
post lab queations help
A voltaic cell consists of a Sn/Sn? half-cell and a Cr/Cr half-cell at 25 °C. The initial concentrations of Snow and Creare 0.10 M and 0.30 M respectively. Standard reduction potentials are as follows: Sn + 2e → Sn, E = -0.14 V; C* + 3e → Cr, E = -0.76 V 1. Which is the anode, which is the cathode? 2. What is the value of E'cell? 3. What is the value of Q, the...
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