Use the tabulated half-cell potentials to calculate the equilibrium constant (k) for the following balanced redox reaction at 25°c. 2 al(s) + 3 mg2+(aq) → 2 al3+(aq) + 3 mg(s) a) 1.1 × 1072 b) 8.9 × 10-73 c) 1.1 × 10-72 d) 1.0 × 1024 e) 4.6 × 1031

Thus the value of equilibrium constant for the balanced redox reaction at 25°C is

Explanation:

Here Al undergoes oxidation by loss of electrons, thus act as anode. magnesium 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 = 6

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 equilibrium constant for the balanced redox reaction at 25°C is

alkaline metals are lithium, sodium, rubidium, potassium, cesium and francium.

alkali metals have electronegativity from 0.7 to 1, lowest in periodic table of elements, which means that alkali metals (i group in periodic table) has positive oxidation number in compounds.

electronegativity is a chemical property that describes the tendency of an atom to attract a shared pair of electrons towards itself.

alkaline metals (far left in main group) have lowest ionizations energy and easy remove valence electrons,

for example, potassium is the alkali metal and has a single valence electron in the outer electron shell.

electron configuration of potassium is: ₁₉k 1s²2s²2p⁶3s²3p⁶4s¹.

they can not exist alone in nature, because they are very reactive.