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Consider the following equilibrium: ci2) and 2.39 atm of nitrosyl chloride NOCl at 595·℃ Answer the following questions Now suppose a reaction vessel is filled with 9.28 atm of chlorine about this system: O rise Under these conditions, will the pressure of NOCl tend to rise or fall? O fall ク is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of NoCl 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 no If you saild 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

Answer 1

1)

There is zero amount of NO present

Therefore the shift must go from left to right

NOCl will fall/decrease in order to increase NO

2)

Yes, rise by addition of NO

3)

K = [NO^2][Cl^2] /[NOCl]^2

∆G = -RTlnK

Arrange the equation for K,

∆G = -41 kj =41000 j

R = 8.314, Temperature = 595 +273=868

K = exp[-41000/(8.314×868)]

K = 0.003409

Then,

0.003409 = [NO^2][Cl^2] / [NOCl]^2,

Plug the values

0.003409 = [NO^2]×9.28/ (2.39)

Arrange the equation for NO and take the square root of both sides,

[NO] = √(0.003409×2.39) / 9.28)

[NO] = 0.02963 atm

[NO]=0.030 atm