Which of the following reactions would have the smallest value of k at 298 k? which of the following reactions would have the smallest value of k at 298 k? a + b → 2 c; e°cell = -0.030 v a + 2 b → c; e°cell = +0.98 v a + b → c; e°cell = +1.22 v a + b → 3 c; e°cell = +0.15 v more information is needed to determine.

The reaction with smallest value of K is :

A + B → 2 C; E°cell = -0.030 V

Explanation:

where :

n = number of electrons transferred

F = Faraday's constant = 96500 C

= standard electrode potential of the cell

R = Gas constant = 8.314 J/K.mol

T = temperature of the reaction =

= equilibrium constant of the reaction

As we cans see, that standard electrode potential of the cell is directly linked to the equilibrium constant of the reaction.

So, the reaction with smallest value of electrode potential will have smallest value of equilibrium constant. And that reaction is:

A + B → 2 C;

water is used to store them because it would keep the radiation from getting out in the open and causing harm to the workers

there is none because earth is stationary and flat.