In an analysis of the following reaction at a certain temperature, Br2(g) + Cl2(g) ⇌ 2BrCl(g)the equilibrium concentrations were found to be [Br2] = 4.5 ×10−3 M, [Cl2] = 2.6 ×10−2 M, and [BrCl] = 1.6 ×10−2 M. Write the equilibrium expression, and calculate the equilibrium constant for this reaction at this temperature.

The equilibrium expression is Equilibrium constant =  

Kc or equilibrium constant for this reaction is 0. 55 x

Explanation:

Br2(g) + Cl2(g) ⇌ 2BrCl(g)

Equilibrium constant =  

Kc =   equation 1

      the concentration of diatoms will be divided by 2

1.3 x 10^-2 is concentration of chlorine

0.45 x 10^-2 is concentration of bromine

1.6 ×10−2 is concentration of BrCl2

Putting the values in equation 1 to calculate equilibrium constant.

Kc=    

Kc =  

Kc= 0.55 x 10^2

equilibrium constant for this reaction is 0.55 x

the molar concentration or partial pressure of the gases is taken to find the equilibrium constant.

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.