Eo cell = 0.0592 v n log(k) calculate the equilibrium constant for the following reaction at 25°c: 2ag(s) + fe2+(aq) ⇌ 2ag+(aq) + fe(s) enter your answer in scientific notation. k = × 10

Explanation:

Here Ag undergoes oxidation by loss of electrons, thus act as anode. iron undergoes reduction by gain of electrons and thus act as cathode.

Where both are standard reduction potentials.

The emf is related to equilibrium constant by following relation:

= standard emf  = -1.24 V

n= no of electrons gained or lost  = 2

K = equilibrium constant = ?

The equilibrium constant for the reaction is

more infor would

a lot

answer: option (a) is the correct answer.

explanation:

the measurement of hydrogen ions in a solution is known as ph.

if ph of a solution is less than 7 then the solution is acidic. if ph of a solution is greater than 7 then the solution is basic.

when the ph of a solution equals 7, then the solution is considered as neutral.

the ph of pure water is 7, therefore, it means that concentration of hydronium ions equals that of hydroxide ions.