Question

1. What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Pb²⁺ concentration is 4.09×10^-4 M and the Mg²⁺ concentration is 1.03 M ?
Pb²⁺(aq) + Mg(s) ---> Pb(s) + Mg²⁺(aq)

Answer: ___V
The cell reaction as written above is spontaneous for the concentrations given____. (true or false)

(From the table of standard reduction potentials: )

Pb2+(aq) + 2 e- --> Pb(s)

-0.126

Mg2+(aq) + 2 e- --> Mg(s)

-2.37

2. What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Ag⁺ concentration is 1.07 M and the Mn²⁺ concentration is 9.74×10^-4 M ?

2Ag⁺(aq) + Mn(s) --> 2Ag(s) + Mn²⁺(aq)

Answer: ___V
The cell reaction as written above is spontaneous for the concentrations given. __ (true or false)

(From the table of standard reduction potentials: )

Ag+(aq) + e- ---> Ag(s)

0.799

Mn2+(aq) + 2e- --> Mn(s)

-1.18

(I will thumbs up if you can answer both correctly please and thank you.)

Answer 1