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Chapter 19: Problem 79

Describe an experiment that would enable you to determine which is the cathode and which is the anode in a galvanic cell using copper and zinc electrodes.

Short Answer

Expert verified
The experiment involves setting up a galvanic cell with zinc and copper electrodes and observing the direction of current on the ammeter and the behavior of the electrodes over time. The anode is the electrode from which the current is flowing (where oxidation is taking place), and in this case, it would be the zinc electrode. The cathode is the electrode where the current is flowing to (where reduction is taking place), which would be the copper electrode.

Step by step solution

01

Setup the Galvanic Cell

First, set up your galvanic cell. Place a copper electrode in one beaker filled with a copper (II) sulphate solution (CuSO4), and a zinc electrode in another beaker filled with a zinc sulphate solution (ZnSO4). Connect the two electrodes with a wire that has an ammeter in the middle, and connect the two solutions with a salt bridge (a U-tube that has a solution of a non-reactive electrolyte, such as potassium nitrate).
02

Observe the Ammeter

Next, observe the ammeter. The direction of the current will indicate which is the anode and which is the cathode, since electric current (by convention) flows from positive to negative. If the current is flowing from the Zinc electrode to the copper electrode, then the Zinc electrode is the anode as oxidation is taking place on it, and the copper electrode is the cathode, where reduction is taking place.
03

Observe the Electrodes

Another way to determine the anode and cathode is to observe the electrodes over time. As the anode undergoes oxidation, it will slowly dissolve into the solution, while the cathode, where reduction takes place, will have copper plating onto it due to the reduction of Cu ions from the solution.

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Most popular questions from this chapter

Consider the following half-reactions: \(\mathrm{MnO}_{4}^{-}(a q)+8 \mathrm{H}^{+}(a q)+5 e^{-} \longrightarrow$$\mathrm{Mn}^{2+}(a q)+4 \mathrm{H}_{2} \mathrm{O}(l)\) \(\mathrm{NO}_{3}^{-}(a q)+4 \mathrm{H}^{+}(a q)+3 e^{-} \longrightarrow \mathrm{NO}(g)+2 \mathrm{H}_{2} \mathrm{O}(l)\) Predict whether \(\mathrm{NO}_{3}^{-}\) ions will oxidize \(\mathrm{Mn}^{2+}\) to \(\mathrm{MnO}_{4}^{-}\) under standard-state conditions.

Explain why most useful galvanic cells give voltages of no more than 1.5 to \(2.5 \mathrm{~V}\). What are the prospects for developing practical galvanic cells with voltages of \(5 \mathrm{~V}\) or more?

A quantity of \(0.300 \mathrm{~g}\) of copper was deposited from a \(\mathrm{CuSO}_{4}\) solution by passing a current of \(3.00 \mathrm{~A}\) through the solution for 304 s. Calculate the value of the faraday constant.

The \(\mathrm{SO}_{2}\) present in air is mainly responsible for the phenomenon of acid rain. The concentration of \(\mathrm{SO}_{2}\) can be determined by titrating against a standard permanganate solution as follows: $$ 5 \mathrm{SO}_{2}+2 \mathrm{MnO}_{4}^{-}+2 \mathrm{H}_{2} \mathrm{O} \longrightarrow{\mathrm{SSO}_{4}^{2-}}+2 \mathrm{Mn}^{2+}+4 \mathrm{H}^{+} $$ Calculate the number of grams of \(\mathrm{SO}_{2}\) in a sample of air if \(7.37 \mathrm{~mL}\) of \(0.00800 \mathrm{M} \mathrm{KMnO}_{4}\) solution are required for the titration.

Steel hardware, including nuts and bolts, is often coated with a thin plating of cadmium. Explain the function of the cadmium layer.
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