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One electrode of a spontaneous electrochemical cell contains a piece of lead metal dipped into saturated...
15. Consider the reaction occurring in a spontaneous electrochemical cell, starting with standard state conditions: Sn(s)...
15. Consider the reaction occurring in a spontaneous electrochemical cell, starting with standard state conditions: Sn(s) + 2H*(aq) → Snº(aq) + H2(g) Which of the following actions would cause the measured cell potential, Ecell, to be greater than Eºcell, (Ecell >Ecell) A. Reducing the mass of the Sn electrode B. Increasing the mass of the Sn electrode C. Increasing the Sn?* ion concentration in the anode compartment. D. Increasing the pressure of hydrogen gas in the hydrogen cell E. Lowering...
An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. a. What...
An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. a. What is the potential of the cell at 25°C if the copper electrode is placed in a solution in which = 3.8 x 10-4 M? Ecell = V b. The copper electrode is placed in a solution of unknown (Cu?+]. The measured potential at 25°C is 0.206 v. What is (cu?+]? (Assume Cu²+ is reduced.) [Cu²+] = M
2. Calculate the standard cell emf (cell potential) for electrochemical cells having the following overall cell...
2. Calculate the standard cell emf (cell potential) for electrochemical cells having the following overall cell reactions and predict if they are spontaneous: a) Sn(s) + Pb2+ (aq) → Sn?" (aq) + Pb(s) Eºcell = Volts. Spontaneous? b) 2002 (aq) + Zn?"(aq) → 2Co3+ (aq) + Zn(s) Eºcell__volts; Spontaneous? c) Cl2(g) + 2Br (aq) + 2Cl(aq) + Br2(1); E° = volts; Spontaneous?
In a galvanic cell, one half-cell consists of a lead strip dipped into a 1.00 M...
In a galvanic cell, one half-cell consists of a lead strip dipped into a 1.00 M solution of Pb(NO3)2. In the second half-cell, solid uranium is in contact with a 1.00 M solution of U(NO3)3. Pb is observed to plate out as the galvanic cell operates, and the initial cell voltage is measured to be 1.672 V at 25°C. (a) Write balanced equations for the half-reactions at the anode and the cathode. Show electrons as e-. Use the smallest integer...
2) In an electrochemical reaction, lead metal becomes Pb ions (Ered = -0.13 V) and Crions...
2) In an electrochemical reaction, lead metal becomes Pb ions (Ered = -0.13 V) and Crions become Crions (Ered = -0.41 V) a) Write both half reactions and then the overall balanced reaction for this redox process b) The is being oxidized and the is being reduced c) What is Ecell for the reaction? d) Based on part C, what is AGⓇ for the reaction? e) Based on part D, what is the value for the equilibrium constant for the...
An electrochemical cell uses Ni/Ni+2 and Cd/cd+2. a) Write the half reactions that will be spontaneous...
An electrochemical cell uses Ni/Ni+2 and Cd/cd+2. a) Write the half reactions that will be spontaneous for this cell. Oxidation- Reduction- b) Which metal is the anode and which is the cathode? anode cathode c) Calculate the emf (Ecell) for this cell. Eceu =
A concentration cell was made using a silver metal electrode in a saturated solution of Agl...
A concentration cell was made using a silver metal electrode in a saturated solution of Agl for the anode half cell, and a silver metal electrode in 1.00 M Ag* for the cathode half cell. E for the cell was 0.475 V at 25°C. Calculate the Ksp for Agl. (Note: For purposes of this exercise, carry out the calculation to three significant figures.)
An electrochemical cell is set up with a lead metal electrode immersed in a 0.1393 M...
An electrochemical cell is set up with a lead metal electrode immersed in a 0.1393 M solution of Pb2+ joined, through a salt bridge, to a 0.0511 M solution of Cd2+ into which is placed a cadmium metal electrode. Calculate the potential of this cell in its galvanic configuration and write out the shorthand notation for the galvanic cell.
The cell diagram for the lead-acid cell that is used in automobile and truck batteries is...
The cell diagram for the lead-acid cell that is used in automobile and truck batteries is Pb(s)|PbSO4(s)H, SO, (aq)|P60, (8), PbSO4) Pb(s) The comma between PbO,(s) and PbSO (3) denotes a heterogeneous mixture of the two solids. The right-hand lead electrode is nonreactive. Write the balanced equation for the net cell reaction. equation: Look up standard potentials for the oxidation and reduction half-reactions, and then calculate the value of Econ call = Calculate the value of AG an AG in...
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...
15. Consider the reaction occurring in a spontaneous electrochemical cell, starting with standard state conditions: Sn(s) + 2H*(aq) → Snº(aq) + H2(g) Which of the following actions would cause the measured cell potential, Ecell, to be greater than Eºcell, (Ecell >Ecell) A. Reducing the mass of the Sn electrode B. Increasing the mass of the Sn electrode C. Increasing the Sn?* ion concentration in the anode compartment. D. Increasing the pressure of hydrogen gas in the hydrogen cell E. Lowering...
An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. a. What is the potential of the cell at 25°C if the copper electrode is placed in a solution in which = 3.8 x 10-4 M? Ecell = V b. The copper electrode is placed in a solution of unknown (Cu?+]. The measured potential at 25°C is 0.206 v. What is (cu?+]? (Assume Cu²+ is reduced.) [Cu²+] = M
2. Calculate the standard cell emf (cell potential) for electrochemical cells having the following overall cell reactions and predict if they are spontaneous: a) Sn(s) + Pb2+ (aq) → Sn?" (aq) + Pb(s) Eºcell = Volts. Spontaneous? b) 2002 (aq) + Zn?"(aq) → 2Co3+ (aq) + Zn(s) Eºcell__volts; Spontaneous? c) Cl2(g) + 2Br (aq) + 2Cl(aq) + Br2(1); E° = volts; Spontaneous?
2) In an electrochemical reaction, lead metal becomes Pb ions (Ered = -0.13 V) and Crions become Crions (Ered = -0.41 V) a) Write both half reactions and then the overall balanced reaction for this redox process b) The is being oxidized and the is being reduced c) What is Ecell for the reaction? d) Based on part C, what is AGⓇ for the reaction? e) Based on part D, what is the value for the equilibrium constant for the...
An electrochemical cell uses Ni/Ni+2 and Cd/cd+2. a) Write the half reactions that will be spontaneous for this cell. Oxidation- Reduction- b) Which metal is the anode and which is the cathode? anode cathode c) Calculate the emf (Ecell) for this cell. Eceu =
A concentration cell was made using a silver metal electrode in a saturated solution of Agl for the anode half cell, and a silver metal electrode in 1.00 M Ag* for the cathode half cell. E for the cell was 0.475 V at 25°C. Calculate the Ksp for Agl. (Note: For purposes of this exercise, carry out the calculation to three significant figures.)
The cell diagram for the lead-acid cell that is used in automobile and truck batteries is Pb(s)|PbSO4(s)H, SO, (aq)|P60, (8), PbSO4) Pb(s) The comma between PbO,(s) and PbSO (3) denotes a heterogeneous mixture of the two solids. The right-hand lead electrode is nonreactive. Write the balanced equation for the net cell reaction. equation: Look up standard potentials for the oxidation and reduction half-reactions, and then calculate the value of Econ call = Calculate the value of AG an AG in...
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...
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