For a standard electrolytic cell, a power source forces the reaction Cu + Zn2+ -> Cu2+ + Zn to occur.
For a standard electrolytic cell, a power source forces the reaction Cu + Zn2+ -> Cu2+ + Zn to occur. Determine the mass of copper that is plated out when a current of 10.0 A is passed for 30.0 minutes through a solution containing Cu2+.
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For a standard electrolytic cell, a power source forces the reaction Cu + Zn2+ -> Cu2+ + Zn to occur.
The voltage of the cell combination of Cu/Cu2+ and Zn/Zn2+ is 0.953V. The standard reduction potential...
The voltage of the cell combination of Cu/Cu2+ and Zn/Zn2+ is 0.953V. The standard reduction potential for Cu/Cu2+ is expected to be 0.34V. Determine the reduction potential for Zn/Zn2+
9) A sol'n in an electrolytic cell contains the ions Cu2+, Fe2+ & Zn2+. If the voltage (initially...
9) A sol'n in an electrolytic cell contains the ions Cu2+, Fe2+ & Zn2+. If the voltage (initially very low) is turned up, in which order will the metals be plated out onto the cathode? Cu2+(aq)2e-Cu(s); E0.34V Fe"(aq) + 2e-→ Fe(s);E"--0.44V Zn2+(aq) + 2e-→ Zn(s): E。--0.76V 10) How long will it take to produce a sol'n of pH 2.00 by electrolysis of 500 mL of 0.100 M AgN03(aq) at 0.240 Amperes? Anode: 2H2O(l) → 4H-(aq) + O2(g) + 4e-, E°...
Given the following electrolytic cell: The current is discharged into the electrolytic cell containing the solution CuSO4(aq) 1.0M at 25 oC. During the operation of the cell, copper Cu(s) is deposite...
Given the following electrolytic cell:
The current is discharged into the electrolytic cell containing
the solution CuSO4(aq) 1.0M at 25 oC. During
the operation of the cell, copper Cu(s) is deposited on
one electrode and oxygen O2(g) gas is released, near the
second electrode.
O2(g) + 4H3O+(aq) +
4e-
6H2O(l) Eo= 1.23V
Cu2+(aq) + 2e- Cu(s)
Eo= 0.34V
A. Write the direction of the flow of electrons in the
cell.
B. Write the electrolysis equation that occurs in the cell....
Consider the cell: Zn(s)ǀ(Zn2+(0.20 M)ǁCu2+(0.20 M)ǀCu(s) with Eº(Cu2+/Cu = 0.34 v and Eº(Zn2+/Zn) = –0.76 v a)...
Consider the cell: Zn(s)ǀ(Zn2+(0.20 M)ǁCu2+(0.20 M)ǀCu(s) with Eº(Cu2+/Cu = 0.34 v and Eº(Zn2+/Zn) = –0.76 v a) Write the cell reaction which occurs when the cell produces current and calculate Ecell. b) If each cell compartment contains 25.0 mL of the corresponding metal salt solution and 25.0 mL of 3.00 M NH3(aq) is added to the Cu2+ solution, Ecell = 0.68 v. Use these data to calculate Kf for Cu(NH3)42+. Cu2+(aq) + 4 NH3(aq) ⇄ Cu(NH3)42+
Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn(s) + Cu2+...
Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn(s) + Cu2+ (aq) Cu(s) + Zn2+ (aq) ЕО cell = 1.1032 V What is the cell potential for a cell with a 2.440 M solution of Zn2+ (aq) and 0.1636 M solution of Cu²+ (aq) at 439.5 K?
- Zn2+ Choose... Choose... (1pts) Identify the complete redox reaction for a ZnZn2+1|Cu2+1Cu cell. A. Zn(s)...
- Zn2+ Choose... Choose... (1pts) Identify the complete redox reaction for a ZnZn2+1|Cu2+1Cu cell. A. Zn(s) + Cu?+ (aq) (aq) + Cu(s) B. Zn(s) + Cu(s) → Zn2+ (aq) + Cu2+ (aq) C. Zn2+ (aq) + Cu(s) Zn(s) + Cu2+ (aq) D. Zn (s) + 2 Cu(s) — Zn2+ (aq) + 2 Cu2+ (aq) (1pts) Identify the complete redox reaction for a Zn/Zn2+||Pb2+1Pb cell. A. Zn (s) + Pb(s) Zn2+ (aq) + Pb2+ (aq) B. Zn2+ (aq) + Pb(s) Zn(s)...
Consider the reaction corresponding to a voltaic cell and its standard cell potential. cell Zn(s) +...
Consider the reaction corresponding to a voltaic cell and its standard cell potential. cell Zn(s) + Cu2+ (aq) + Cu(s) + Zn2+ (aq) E = 1.1032 V As What is the cell potential for a cell with a 2.573 M solution of Zn²+ (aq) and 0.1055 M solution of Cu²+ (aq) at 432.4 K?
Given the following electrolytic cell: The current is discharged into the electrolytic cell containing the solution CuS...
Given the following electrolytic cell:
The current is discharged into the electrolytic cell containing
the solution CuSO4(aq) 1.0M at 25 oC. During
the operation of the cell, copper Cu(s) is deposited on
one electrode and oxygen O2(g) gas is released, near the
second electrode.
O2(g) + 4H3O+(aq) +
4e-
6H2O(l) Eo= 1.23V
Cu2+(aq) + 2e- Cu(s)
Eo= 0.34V
A. The current in the cell is 1.5 amperes. The current is
streamed in 40 minutes.
i. Calculate the mass of copper...
Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn(s) + Cu²+...
Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn(s) + Cu²+ (aq) + Cu(s) + Zn2+ (aq) = 1.1032 V What is the cell potential for a cell with a 2.401 M solution of Zn2+ (aq) and 0.1776 M solution of Cu²+ (aq) at 420.4 K? Answer:
A Cu-Zn voltaic cell based on the reaction in the equation given below. Zn(s)+Cu2+(aq)àZn2+(aq)+Cu(s) Which metal...
A Cu-Zn voltaic cell based on the reaction in the equation given below. Zn(s)+Cu2+(aq)àZn2+(aq)+Cu(s) Which metal is oxidized in this voltaic cell? A. Copper B. Zinc
9) A sol'n in an electrolytic cell contains the ions Cu2+, Fe2+ & Zn2+. If the voltage (initially very low) is turned up, in which order will the metals be plated out onto the cathode? Cu2+(aq)2e-Cu(s); E0.34V Fe"(aq) + 2e-→ Fe(s);E"--0.44V Zn2+(aq) + 2e-→ Zn(s): E。--0.76V 10) How long will it take to produce a sol'n of pH 2.00 by electrolysis of 500 mL of 0.100 M AgN03(aq) at 0.240 Amperes? Anode: 2H2O(l) → 4H-(aq) + O2(g) + 4e-, E°...
Given the following electrolytic cell:
The current is discharged into the electrolytic cell containing
the solution CuSO4(aq) 1.0M at 25 oC. During
the operation of the cell, copper Cu(s) is deposited on
one electrode and oxygen O2(g) gas is released, near the
second electrode.
O2(g) + 4H3O+(aq) +
4e-
6H2O(l) Eo= 1.23V
Cu2+(aq) + 2e- Cu(s)
Eo= 0.34V
A. Write the direction of the flow of electrons in the
cell.
B. Write the electrolysis equation that occurs in the cell....
Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn(s) + Cu2+ (aq) Cu(s) + Zn2+ (aq) ЕО cell = 1.1032 V What is the cell potential for a cell with a 2.440 M solution of Zn2+ (aq) and 0.1636 M solution of Cu²+ (aq) at 439.5 K?
- Zn2+ Choose... Choose... (1pts) Identify the complete redox reaction for a ZnZn2+1|Cu2+1Cu cell. A. Zn(s) + Cu?+ (aq) (aq) + Cu(s) B. Zn(s) + Cu(s) → Zn2+ (aq) + Cu2+ (aq) C. Zn2+ (aq) + Cu(s) Zn(s) + Cu2+ (aq) D. Zn (s) + 2 Cu(s) — Zn2+ (aq) + 2 Cu2+ (aq) (1pts) Identify the complete redox reaction for a Zn/Zn2+||Pb2+1Pb cell. A. Zn (s) + Pb(s) Zn2+ (aq) + Pb2+ (aq) B. Zn2+ (aq) + Pb(s) Zn(s)...
Consider the reaction corresponding to a voltaic cell and its standard cell potential. cell Zn(s) + Cu2+ (aq) + Cu(s) + Zn2+ (aq) E = 1.1032 V As What is the cell potential for a cell with a 2.573 M solution of Zn²+ (aq) and 0.1055 M solution of Cu²+ (aq) at 432.4 K?
Given the following electrolytic cell:
The current is discharged into the electrolytic cell containing
the solution CuSO4(aq) 1.0M at 25 oC. During
the operation of the cell, copper Cu(s) is deposited on
one electrode and oxygen O2(g) gas is released, near the
second electrode.
O2(g) + 4H3O+(aq) +
4e-
6H2O(l) Eo= 1.23V
Cu2+(aq) + 2e- Cu(s)
Eo= 0.34V
A. The current in the cell is 1.5 amperes. The current is
streamed in 40 minutes.
i. Calculate the mass of copper...
Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn(s) + Cu²+ (aq) + Cu(s) + Zn2+ (aq) = 1.1032 V What is the cell potential for a cell with a 2.401 M solution of Zn2+ (aq) and 0.1776 M solution of Cu²+ (aq) at 420.4 K? Answer:
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