Consider the following equilibrium: Now suppose a reaction vessel is filled with

Question

Consider the following equilibrium: Now suppose a reaction vessel is filled with 8.38 atm of chlorine (C12) and 1.14 atm of nitrosyl chloride (NOCI) at 1157· Answer the following questions about this system: Under these conditions, will the pressure of NOCI tend to rise or se fall? O fall x Ino Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of NOCI will tend to rise, can that be changed to a tendency to fall by adding NO? Similarly if you said the pressure of NOCI will tend to fall, can that be changed to a tendency to rise by adding NO? yes If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO needed to reverse it. Round your answer to 2 significant digits. atm

Explanation / Answer

a)

get Q

Q = P-NOCl^2 / (PNO^2)(PCl2)

since there is no NO, the reaction must go reverse, in order ot increase NO pressure, so NOCl pressure must drop/fall

B)

yes, we can reverse this by adding NO, so Q = Kp

C)

this will be:

dG°= -RT*ln(Kp)

-41000 = -8.314*298*ln(Kp)

Kp = exp(41000 /(8.314*298))

Kp = 15378170.16

now..

Kp = Qp

15378170.16 = P-NOCl^2 / (PNO^2)(PCl2)

15378170.16 =1.14^2 / (PNO^2)*8.38

PNO^2 = (1.14^2)/(15378170.16 *8.38)

PNO = (1.00846*10^-8)^0.5

P-NO = 0.00010 atm must be added

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