help please! a piece of jewelry is connected to the cathode of an electrolytic cell and...
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a piece of jewelry is connected to the cathode of an
electrolytic cell and...
electrolytic cells An object of jewelry has a surface area of 4.20 cm2. It is to...
electrolytic cells
An object of jewelry has a surface area of 4.20 cm2. It is to be plated with silver (Ag) to a depth of 30.0 eters, requiring a total of 0.0126 cm3 of Ag. Given the density of silver (10.5 g/cm2), how long will it take to electroplate the silver using an electrolytic cell with the object connected to the cathode, a solution of AgNO3 (aq) and a current of 2.48 mA? Assume 100% cell efficiency.
2. For each of the following cell notations: a. Identify the cathode and anode. b. Write...
2. For each of the following cell notations: a. Identify the cathode and anode. b. Write the net cell equation. c. Calculate the cell potential. I) Pb(e) 1 Pb2+(ag) 11 Ni2+ (aq) 1 Ni(s) II) Pts 1 So,"caq) H(aq) 1 H2SO3(aq) 11 Ag‘aq) 1 Ago) 4. Balance the following redox reaction occurring in a basic medium. NO2 (aq) + Al(s) + NH3(g) + AlO2 (aq) 5. A student wishes to set up an electrolytic cell to plate copper onto a...
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°...
How many grams of Ag(s) could be plated out on the cathode of an electrolytic cell...
How many grams of Ag(s) could be plated out on the cathode of an electrolytic cell by the passage of 5.0 Amps of current through AgNO3 solution for 1 hour? A. 5.2 x 10-5 g B. 0.19 g C. 20 g D. 5.5 x 10-3 g
What mass of silver is deposited on the cathode of an electrolytic cell if an electric...
What mass of silver is deposited on the cathode of an electrolytic cell if an electric current of 2.86 A is run through a solution of AgNO3 for one hour? Select one: O a. 11.5 g O b. 5.76 g O c. Og O d. 0.11 g o e. 0.192 g
3. How many grams of Ag(s) could be plated out on the cathode of an electrolytic...
3. How many grams of Ag(s) could be plated out on the cathode of an electrolytic cell by the passage of 5.0 Amps of current through AgNO3 solution for 1 hour? Faraday's number = 96485 Coul/mol. a) 5.5 x 10-ºg b) 0.19 g c) 5.2 x 105 g d) 2.0 g e) 20 g
Help please! The subscript c on the E and n refers to the cathode and a...
Help please!
The subscript c on the E and n refers to the cathode and a refers to the anode and EP, E, ne and n, are obtained from the Chemistry Data Sheet. Combining (13) and (14) with Eq. (11) gives Een – Es – Ex = {E: -0.0592 109 Reumot} - {E:- 0.092 108 Quote} (15) V-12 EXPERIMENT V: VOLTAIC CELLS, AND THE NERNST EQUATION PRELAB ASSIGNMENT (CONTINUED) 4. You added 0.05 mL of 0.10 M AgNO3 to 4.0...
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...
help with these please A voltaic cell is constructed in which the cathode is a standard...
help with these please
A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode PHlatm) immersed in a solution of unknown [H]. If the cell potential is 0.181 V, what is the pH of the unknown solution at 298 K? pH A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode PHlatm) immersed in a solution of unknown...
If the following half-reactions are used in an electrolytic cell: Ag+(aq) + e− ⟶ Ag(s) Eo...
If the following half-reactions are used in an electrolytic cell: Ag+(aq) + e− ⟶ Ag(s) Eo = 0.80 V Ca2+(aq) + 2 e− ⟶ Ca(s) Eo = −2.76 V Click here for a copy of Final Exam cover sheet. 1) The metal solid that is plated out at the cathode is [Ag(s), Ca(s)] 2) It would take [3, 8. 16] hours to deposit 60 g of the solid with a current of 5.0 A.
electrolytic cells
An object of jewelry has a surface area of 4.20 cm2. It is to be plated with silver (Ag) to a depth of 30.0 eters, requiring a total of 0.0126 cm3 of Ag. Given the density of silver (10.5 g/cm2), how long will it take to electroplate the silver using an electrolytic cell with the object connected to the cathode, a solution of AgNO3 (aq) and a current of 2.48 mA? Assume 100% cell efficiency.
2. For each of the following cell notations: a. Identify the cathode and anode. b. Write the net cell equation. c. Calculate the cell potential. I) Pb(e) 1 Pb2+(ag) 11 Ni2+ (aq) 1 Ni(s) II) Pts 1 So,"caq) H(aq) 1 H2SO3(aq) 11 Ag‘aq) 1 Ago) 4. Balance the following redox reaction occurring in a basic medium. NO2 (aq) + Al(s) + NH3(g) + AlO2 (aq) 5. A student wishes to set up an electrolytic cell to plate copper onto a...
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°...
What mass of silver is deposited on the cathode of an electrolytic cell if an electric current of 2.86 A is run through a solution of AgNO3 for one hour? Select one: O a. 11.5 g O b. 5.76 g O c. Og O d. 0.11 g o e. 0.192 g
3. How many grams of Ag(s) could be plated out on the cathode of an electrolytic cell by the passage of 5.0 Amps of current through AgNO3 solution for 1 hour? Faraday's number = 96485 Coul/mol. a) 5.5 x 10-ºg b) 0.19 g c) 5.2 x 105 g d) 2.0 g e) 20 g
Help please!
The subscript c on the E and n refers to the cathode and a refers to the anode and EP, E, ne and n, are obtained from the Chemistry Data Sheet. Combining (13) and (14) with Eq. (11) gives Een – Es – Ex = {E: -0.0592 109 Reumot} - {E:- 0.092 108 Quote} (15) V-12 EXPERIMENT V: VOLTAIC CELLS, AND THE NERNST EQUATION PRELAB ASSIGNMENT (CONTINUED) 4. You added 0.05 mL of 0.10 M AgNO3 to 4.0...
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...
help with these please
A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode PHlatm) immersed in a solution of unknown [H]. If the cell potential is 0.181 V, what is the pH of the unknown solution at 298 K? pH A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode PHlatm) immersed in a solution of unknown...
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