H2S(aq)⇌HS−(aq)+H+(aq), K1 = 9.06×10−8, and HS−(aq)⇌S2−(aq)+H+(aq), K2 = 1.18×10−19, what is the equilibrium constant Kfinal for the following reaction? S2−(aq)+2H+(aq)⇌H2S(aq)

Therefore the equilibrium constant   is 9.35× 10²⁵

Explanation:

Equilibrium constant:

Equilibrium constant is used to find out the ratio of the concentration of the product to that of reactant.

xA+yB→zC

The equilibrium constant K,

Here [A] is equilibrium concentration of A

[B] is equilibrium concentration of B

[C] is equilibrium concentration of C.

1.            

2.        

3.

Therefore,

⇒K₃=9.35× 10²⁵

Therefore the equilibrium constant   is 9.35× 10²⁵

1. for the first question, we must find the mass of the anhydrous salt, mgso₄. the molar mass for mgso₄·7h₂o is 246.47 g/mol, while that of mgso₄ is 120.37 g/mol.7.834 g mgso₄·7h₂o * 1 mol mgso₄·7h₂o/246.47 g * 1 mol mgso₄/1 mol mgso₄·7h₂o * 20.37 g mgso₄/mol = 0.647 g mgso₄

2. mass of water = mass of sample - mass of anhydrous salemass of water = 7.834 - 0.647 = 7.19 gpercent water in hydrate = 7.19/7.834 * 100 = 91.74%

> b takes place in the gas phase in an isothermal tubular reactor. the feed is one mole of a per one mole of c, an inert. the entering temperature and pressure are 427°c and 10 atm, respectively. the gas constant r = 0.08206 atm · l/mol · k.