Is the following reaction spontaneous at 50°c? ag/ag'(0.0078 m)||ni2 (0.023 m) ni

The reaction is non spontaneous at

Explanation:

= +ve, reaction is spontaneous

= -ve, reaction is non spontaneous

= 0, reaction is in equilibrium

Using Nernst equation :

where,

R = gas constant =

T= temperature in kelvin =

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

F= Faraday's constant = 96500 C

= standard electrode potential =

Where both are standard reduction potentials.

Thus as is negative , the reaction is no spontaneous.

i would say b

explanation:

but i think i would need more information than that