What is the equilibrium constant for the reaction of agcl(s) with concentrated hcn? the ksp of agcl is 1.8 × 10−10 and the kf of ag(cn)2− is 1.0 × 1021.

The equilibrium constant for a reaction is simply the product of the solubility constant of the solute and the formation constant of the product, that is:

Keq = Ksp * Kf

Keq = 1.8 × 10^−10 * 1.0 × 10^21

Keq = 1.8 x 10^11

2b2t

explanation:

2b2t

as given the equation is

2al + 6 hcl > 2 alcl3 + 3 h2(g)

as per equation two moles of aluminum reacts with six moles of hcl to give two moles of alcl3 and three moles of hydrogen gas

given: three moles of al are present and 7 moles of hcl

for three moles of aluminum nine moles of hcl will be required

however as 7 moles of hcl are present so the limiting reagent is hcl

hcl is going to decide the number of moles of product formed

when six moles of hcl are present = 3 moles of h2 are formed

when one mole of hcl is present == 3/6 mole sof h2 will be formed

when 7 moles of hcl are present = 3 x 7/ 6 moles of h2 will be formed = 3.5 moles of h2