1) I just want to check if this one is correct(adsbygoogle = window.adsbygoogle || []).push({});

reaction => CCl4(g) <==> C(s) = 2Cl2(g)

Kp= .76

find the initial partial pressure of CCl4 that will produce an equilibrium total pressure of 1.20 atm

p.total = p.CCl4 + p.Cl2

CCl4 <=> 2Cl2

i. press x 2x

change 1.20 - x 1.20 - 2x

kp = .76 = (p.Cl2^2)/(p.CCL4) = (1.2-2x)^2/(1.2-x)

x= .8557 or x= .1543

.8557 will not work so take x = .1543

p.CCl4 = 1.20- .1543 = 1.05 atm

the rub is that if I use x to find p.Cl2 I get .892 atm

1.05 + .892 =/= 1.2 ?

Q2.

Ok

constant temp =25 C constant volume

reaction; Nh4HS (g)<==> NH3(g) + H2S(g)

step 1; some NH4HS decomposed in an evacuated container to give a total pressure at equililbrium of .659 atm

step 2; extra NH3 is added. re-established equilibrium gives a partial pressure for NH3 of .750 atm

find Kp

I'm stuck on this one.

.

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# Two equilibrium problems

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