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A sample of solid ammonium chloride was placed in an evacuated chamber, and then heated causing it to decompose according to the following reaction: NH4Cl(s) NH3(g) + HCl(g) In a particular experiment the pressure of NH3(g) in the container was found to be 2.2 atm. Calculate the value of Kp for the decomposition of NH4Cl(s) at this temperature. Kp = SubmitShow Hints

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Answer:

Kp = 4.84

Explanation:

Considering the ICE table for the equilibrium as:

                     NH₄Cl (s)      ⇔         NH₃ (g) +      HCl (g)

t = o              

t = eq                                                 x                      x

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Moles at eq:                                      x                      x

       

Given the pressure of NH₃ at equilibrium = 2.2 atm

x = 2.2 atm

The expression for the equilibrium constant is:

[tex]K_p={P_{NH_3}P_{[HCl}}[/tex]  

So,

[tex]K_p={x^2}[/tex]  

x = 2.2 atm

Thus,  

[tex]K_p={2.2}^2[/tex]  

Thus, Kp = 4.84

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