Question 1:An unknown metal M and a 0.50 M solution of its divalent chloride sal

Question

Question 1:An unknown metal M and a 0.50 M solution of its divalent chloride salt, MCl2, are connected in a galvanic cell to a solution containing Cu(s) and a 0.050 M solution of Cu(NO3)2(aq). It is observed that the copper electrode is the cathode, and the measured cell potential is 0.56 V at a temperature of 298 K. What is the atomic symbol for this unknown metal M?

Question 2: Which metal is NOT commonly used as part of the anode in commercial batteries?

Select one:

a. Ag

b. Zn

c. Pb

d. Li

Question 3: What mass of Cr(s) (in g) may be electrodeposited from application of a 0.532 A current to a solution of Cr3+(aq) over 2.47 min?

Explanation / Answer

For question 1, we'll use the nerst equation:
E = E° - 0.059/nlogK

From here, we solve for E°:
E° = E + 0.059logK
E° = 0.56 + 0.059/2 log(0.50/0.050)
E° = 0.5895 V

Now the E° for Copper is +0.34 V
E2° = 0.34 - 0.5895 = -0.2495 V or -0.25 V

This E° corresponds to the Ni metal.

The other two questions, post them in another question thread.

Hope this helps

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