What is the value of the equilibrium constant at 25 oc for the reaction between the pair: ag(s) and ni2+(aq) to give ni(s) and ag+(aq) use the reduction potential values for ag+(aq) of +0.80 v and for ni2+(aq) of -0.25 v give your answer using e-notation with no decimal places

Explanation:

The balanced chemical equation will be:

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

Where both are standard reduction potentials.

The standard emf of a cell is related to Gibbs free energy by following relation:

= gibbs free energy  

n= no of electrons gained or lost  =?

F= faraday's constant

= standard emf

The Gibbs free energy is related to equilibrium constant by following relation:

R = gas constant = 8.314 J/Kmol

T = temperature in kelvin =

K = equilibrium constant

Thus the value of the equilibrium constant at is

answer is: empirical formula is tl₂o. if we use 100 grams of compound, tha:

m(tl) = 96.2%  · 100 g ÷ 100%.

m(tl) = 96.2 g.

n(tl) = m(tl)  ÷ m(tl). n(tl) = 96.2 g  ÷ 204.4 g/mol.

n(tl) = 0.47 mol. m(o) = 3.77 g. n(o) = m(o)  ÷ m(o). n(o) = 3.77 g  ÷ 16 g/mol. n(ag) = 0.235 mol. n(tl) . n(o) = 0.47 mol : 0.235 mol /0.235. n(tl) . n(o) = 2 : 1.

m(tl₂o) = 204.4 g/mol  · 2 + 16 g/mol = 424.8 g/mol.

m(compound) = 456. 8 g/mol - 424.8 g/mol = 32 g/mol ( 2 oxygens); tl₂o₃.