A student measures the potential of a cell made up with 1 M CuSO4 in one solution and 1 M AgNO3 in the other. There is a copper electrode in the CuSO4 and a silver electrode in the AgNO3 in one solution and 1 M AgNO3 in the other. There is a copper electrode in the CuSO4 and a silver electrode in the AgNO3. The student finds the potential of the cell, Eocell , is 0.47 V, and that the copper electrode is negative. 5. If EoAg+,Ag equals 0.80V, what is Eoanode? 6. Write the net ionic equation for the reaction that occurs in the cell studied by the student:
A student measures the potential of a cell made up with 1 M CuSO4 in one solution and 1 M AgNO3 in the other. There is a copper electrode in the CuSO4 and a silver electrode in the AgNO3 in one solution and 1 M AgNO3 in the other. There is a copper electrode in the CuSO4 and a silver electrode in the AgNO3. The student finds the potential of the cell, Eocell , is 0.47 V, and that the copper electrode is negative.
5. If EoAg+,Ag equals 0.80V, what is Eoanode?
6. Write the net ionic equation for the reaction that occurs in the cell studied by the student:
7.The student adds 6 M NH3 to the CuSO 4 solution until the Cu2+ ion is essentially all converted to Cu(NH3)42+ ion. The voltage of the cell, Ecell, goes up to 0.92V and the Cu electrode is still negative. Find the concentration of Cu2+ ion in the cell. (use this equation; Ecell =Eocell - 0.0592/2 * log([Cu2+]/[Ag+]2)
8. In question 7 the [Cu(NH3)42+] is about 0.05 M and [NH3] is about 3 M. Given these values and the [Cu2+] from question 7, calculate K for the reaction: Cu(NH3)42+(aq)---> Cu2+(aq) + 4 NH3 (aq)
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