Concept explainers
Interpretation: The following reagent should be identified which can oxidase
Concept Introduction:
Redox reaction are those in which oxidation number changes.
Half reaction are the separated
Redox equation can be balanced via the half –reaction methods, which allows for the addition of
Standard EMF:
The electromotive force (EMF) is the maximum potential difference between two electrodes of a galvanic cell.
This quantity is related to the tendency for an element.
i.e- It has a great tendency to acquire or gain the compound.
Half-cell Reaction: A half-cell is one of the two electrodes in a galvanic cell.
Example, the Zn-Cu battery, the two half cells make an oxidizing couple.
Electrochemical cell:
An electrochemical cell in which a spontaneous
To identify: The following reagent which is responsible to convert water molecule into oxygen molecule.
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CHEM: ATOM FIRST V. 1 W/ACCESS >C<
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- A galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2, resulting in the reaction H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)K=? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2 solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate at the halfway point in the titration.arrow_forwardAn electrolysis experiment is performed to determine the value of the Faraday constant (number of coulombs per mole of electrons). In this experiment, 28.8 g of gold is plated out from a AuCN solution by running an electrolytic cell for two hours with a current of 2.00 A. What is the experimental value obtained for the Faraday Constant?arrow_forwardA solution contains the ions H+, Ag+, Pb2+, and Ba2+, each at a concentration of 1.0 M. (a) Which of these ions would be reduced first at the cathode during an electrolysis? (b) After the first ion has been completely removed by electrolysis, which is the second ion to be reduced? (c) Which, if any, of these ions cannot be reduced by the electrolysis of the aqueous solution?arrow_forward
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