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.

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.