At high temperatures, solid ammonium chloride decomposes into
gaseous ammonia and hydrogen chloride.
NH4Cl (s) ⇌ NH3 (g) + HCl (g)
a) An excess of ammonium chloride was introduced into an evacuated
container. After raising the temperature to 340 ° C, the pressure
was measured 1.013 bar. Calculate the equilibrium constant at this
temperature. (4p)
b) A container of volume 1.00 dm3 initially contained 0.0200 moles
of ammonia. What are the partial pressures for ammonia and hydrogen
chloride after an excess of ammonium chloride is introduced into
the container and the temperature is raised to 340 ° C?
The answer is a) K = 0,2565 b) P = 1,229 bar för NH3(g); P = 0,209 bar för HCl(g)
Answer :-
This question is solved by using the simple concept of equilibrium reaction and using the expression of equilibrium constant.
The answer is given in the image,
At high temperatures, solid ammonium chloride decomposes into gaseous ammonia and hydrogen chloride. NH4Cl (s) ⇌...
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