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Chapter 7: Problem 29

In a voltaic cell, if iron and silver electrodes are connected with each other then current flows (a) from iron to silver outside the cell (b) from silver to iron within the cell (c) from silver to iron outside the cell (d) current does not flow in this cell

Short Answer

Expert verified
Answer: (c) from silver to iron outside the cell

Step by step solution

01

Determine the anode and the cathode

First, we need to determine which of the two metals, iron and silver, will act as the anode and which will act as the cathode. To do this, we can look up the standard reduction potentials of both metals. The metal with the lower reduction potential (more negative) will more readily lose electrons and become oxidized, thus acting as the anode. The metal with the higher reduction potential (less negative) will more readily gain electrons and become reduced, thus acting as the cathode. The standard reduction potential for iron (Fe) is -0.44V, and for silver (Ag) is +0.80V. Since iron has the lower reduction potential, it will act as the anode, and silver will act as the cathode.
02

Determine the direction of current flow

Now, knowing the anode and the cathode in our voltaic cell, we can determine the direction of current flow. Recall that the flow of electrons is from the anode (iron) to the cathode (silver), while the flow of current is in the opposite direction. Therefore, the current will flow from the silver electrode to the iron electrode. We can now look at the given options and choose the one that correctly matches the current flow direction. From the given options, the correct answer is: (c) from silver to iron outside the cell

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Most popular questions from this chapter

The amount of copper deposited by the passage of 1 mole of electrons during the electrolysis of aqueous \(\mathrm{CuSO}_{4}\) solution is (a) \(63.5 \mathrm{~g}\) (b) \(31.75 \mathrm{~g}\) (c) \(159.5 \mathrm{~g}\) (d) \(79.75 \mathrm{~g}\)

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