Question

Use the standard reduction potentials located in the 'Tables' linked above to calculate the equilibrium constant for the reaction:
Ni2+(aq) + Cu(s) ---> Ni(s) + Cu2+(aq)
Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm.
Equilibrium constant: __________ delta G° for this reaction would be _________ ( greater /less ) than zero.
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cu2+ concentration is 4.38×10-4 M and the Al3+concentration is 1.08 M ?
3Cu2+(aq) + 2Al(s)----> 3Cu(s) + 2Al3+(aq)

Answer 1

Answer:

Check the explanation

Explanation:

cell CuE Ecell 0.337 (-0.14) Ecl0.477 V

Since $E^o_{ cell } > 0$ , the value of \Delta G^o will be negative.

$\Delta G^o < 0$

$\Delta G^o =-nFE^o_{ cell }.$.....(1)

But

$\Delta G^o =-RT ln K$......(2)

From (1) and (2)

$\Delta G^o =-RT ln K=-nFE^o_{ cell }$

ln K =$\frac{nFE^o_{ cell } }{RT }$

ln K =$\frac{ 2 \times 96500 \times 0.477 }{8.314 \times \left ( 25+273.15 \right ) }$

ln K =37.139

K =$1.3468 \times 10^{16}$

Hence, the value of the equilibrium constant is $1.35 \times 10^{16}$