Avoltaic cell is constructed with two zn2+-zn electrodes, where the half-reaction is zn2+ + 2e− → zn (s) e° = -0.763 v the concentrations of zinc ion in the two compartments are 4.50 m and 1.11 ⋅ 10−2 m, respectively. the cell emf is v.

Answer : The cell emf for this cell is 0.077 V

Solution :

The balanced cell reaction will be,  

Oxidation half reaction (anode):  

Reduction half reaction (cathode):  

In this case, the cathode and anode both are same. So, is equal to zero.

Now we have to calculate the cell emf.

Using Nernest equation :

where,

n = number of electrons in oxidation-reduction reaction = 2

= ?

= 0.0111 M

= 4.50 M

Now put all the given values in the above equation, we get:

Therefore, the cell emf for this cell is 0.077 V

the answer is b i think

f=ma newton

f=100x2.5=250n