What mass of Cu(s) is electroplated by running 30.0 A of current through a Cu2+(aq)Cu2+(aq) solution for 4.00 hours?
What mass of Cu(s) is electroplated by running 30.0 A of current through a Cu2+(aq)Cu2+(aq) solution...
What mass of Cu(s) is electroplated by running 25.5 A of current through a Cu2+(aq) solution for 4.00 h? Express your answer to three significant figures and include the appropriate units.
What mass (in grams) of Cu (s) is generated by running current of 15.0 A through a Cu2+ solution for 4.00 hours? As part of your answer, you must include the 12 reaction associated with the plating process.
Copper can be electroplated at the cathode of an electrolysis cell by the half-reaction: Cu2+(aq)+2e−→Cu(s) How much time would it take for 348 mgmg of copper to be plated at a current of 6.3 AA?
Copper can be electroplated at the cathode of an electrolysis cell by the half-reaction. Cu2+(aq)+2e−→Cu(s) How much time would it take for 329 mg of copper to be plated at a current of 7.1 A ? Express your answer using two significant figures.
A galvanic cell Cr(s)|Cr2+(aq) || Cu2+(aq)|Cu(s) is constructed using a completely immersed Cr electrode that weighs 35.4 g and a Cu electrode immersed in 462 mL of 1.00 M Cu2+(aq) solution. A steady current of 0.0795 A is drawn from the cell as the electrons move from the Cr electrode to the Cu electrode. (a) Which reactant is the limiting reactant in this cell? Enter symbol (b) How long does it take for the cell to be completely discharged? s...
Consider the following reaction: 2 Ag+(aq) + Cu(s)->2 Ag(s) + Cu2+(aq) Ecell^o = +0.46V Suppose an external power source is applied with a current of 1.50 A such that the reaction is reversed and electrolysis occurs. (a) If the current is applied for 2.00 hours, how many grams of Cu(s) could be recovered? What is the minimum mass of the silver electrode required to recover this mass of copper? (b) What is the minimum amount of work that must be...
Conceptual: Consider a Sn(s)|Sn2+(aq) || Cu2+(aq)|Cu(s) cell. If the Sn2+ concentration is increased, what will happen to the measured Ecell value? • Calculation, full-reaction Nernst equation: Use the full Nernst equation to calculate Ecell for the conditions described… • Easier: Ni | Ni2+(0.300 M) || Cu2+(0.002 M) | Cu • Harder: Al | Al3+(0.002 M) || Cu2+(4.00 M) | Cu • Calculation, half-reaction Nernst equation: Use the Nernst equation to calculate E at pH 3.00 and [Cl- ] = 0.0035...
In an electrochemical cell composed of Cu(s)/Cu2+(aq, o.10M)||Cu2+(aq, 1.0M) |Cu(s), Which concentration of Cu would the anode be sitting in? Which concentration of Cu would the cathode be sitting in?
Calculate the E°cell for the following reaction: Cu2+ (aq) + Ni (s) → Cu (s) + Ni2+ (aq) A) (-0.59 ± 0.01) V B) (-0.09 ± 0.01) V C) (0.59 ± 0.01) V D) (0.09 ± 0.01) V --------------------------------------------------------------------------------------------------------- What is the proper line notation for the following reaction? Cu (s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag (s) A) Cu2+ | Cu || Ag | Ag+ B) Ag+ | Ag || Cu | Cu2+ C) Cu |...
A concentration cell composed of Cu(s)/Cu2+(aq, 0.10M)||Cu2+(aq, 1.0M)| Cu(s) is connected to a voltmeter. Initially a reading of 29.6 mV was obtained. The cell was left sitting for a few minutes. How has the voltage change compared to the initial reading? Why did this change occur?