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(a)
Interpretation:
The reduction half and oxidation half-reaction of copper is to be stated.
Concept introduction:
Electrolytic cell is a setup in which electricity is required to carry out a non-spontaneous and not feasible reaction. In an electrolytic cell two electrodes are used. One is anode and other one is cathode. Anode is positively charged and cathode is negatively charged.
(b)
Interpretation:
The electrode at which two different half reactions are taking place is to be stated.
Concept introduction:
Electrolytic cell is a setup in which electricity is required to carry out a non-spontaneous and not feasible reaction. In an electrolytic cell two electrodes are used. One is anode and other one is cathode. Anode is positively charged and cathode is negatively charged.
(c)
Interpretation:
The electrodes “
Concept introduction:
Electrolytic cell is a setup in which electricity is required to carry out a non-spontaneous and not feasible reaction. In an electrolytic cell two electrodes are used. One is anode and other one is cathode. Anode is positively charged and cathode is negatively charged.
(d)
Interpretation:
The ions carrying the charge, with their direction of movement are to be stated.
Concept introduction:
Electrolytic cell is a setup in which electricity is required to carry out a non-spontaneous and not feasible reaction. In an electrolytic cell two electrodes are used. One is anode and other one is cathode. Anode is positively charged and cathode is negatively charged. Flow of electrons is carry out by the electrolyte present in it.
(e)
Interpretation:
The bubbles along with the electrode at which they are occurring are to be identified. The half reaction occurring at the electrode is to be stated. The answers are to be summarized.
Concept introduction:
Electrolytic cell is a setup in which electricity is required to carry out a non-spontaneous and not feasible reaction. In an electrolytic cell two electrodes are used. One is anode and other one is cathode. Anode is positively charged and cathode is negatively charged. Flow of electrons is carry out by the electrolyte present in it.
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Chapter 19 Solutions
Bundle: Introductory Chemistry: An Active Learning Approach, 6th + OWLv2, 1 term (6 months) Printed Access Card
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- What mass of each product is produced in each of the electrolytic cells of the previous problem if a total charge of 3.33105 C passes through each cell? Assume the voltage is sufficient to perform the reduction.arrow_forwardThe following two half-reactions arc involved in a voltaic cell. At standard conditions, what species is produced at each electrode? Ag++eAgE=0.80VNi2++2eNiE=0.25Varrow_forwardA solution of copper(II) sulfate is electrolyzed by passing a current through the solution using inert electrodes. Consequently, there is a decrease in the Cu2+ concentration and an increase in the hydronium ion concentration. Also, one electrode increases in mass and a gas evolves at the other electrode. Write half-reactions that occur at the anode and at the cathode.arrow_forward
- Predict the chemical reactions that will occur at the two electrodes in the electrolysis of an aqueous sodium hydroxide solution.arrow_forwardBased on the cell potential measured for the cells Co(s)|Co2+(aq) Cu 2+( aq)|Cu( s)E=0.614VFe(s)|Fe2+(aq) Cu 2+( aq)|Cu( s)E=0.777V what potential should you expect to find for the following cell? Fe(s)|Fe2+(aq)Co2+(aq)|Co(s)arrow_forwardA factory wants to produce 1.00 103 kg barium from the electrolysis of molten barium chloride. What current must be applied for 4.00 h to accomplish this?arrow_forward
- • write and balance half-reactions for simple redox processes.arrow_forwardGold is produced electrochemically from an aqueous solution of Au(CN)2 containing an excess of CN. Gold metal and oxygen gas are produced at the electrodes. What amount (moles) of O2 will be produced during the production of 1.00 mole of gold?arrow_forwardDetermine the overall reaction and its standard cell potential at 25 C for the reaction involving the galvanic cell in which cadmium metal is oxidized to 1 M cadmium(II) ion and a half—cell consisting of an aluminum electrode in 1 M aluminum nitrate solution. 15 the reaction spontaneous at standard conditions?arrow_forward
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