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 9.10 atm of nitrosyl chloride (NOC1) and 6.50 atm of chlorine (C1, at 1003. °C. Answer the following questions about this system rise Under these conditions, will the pressure of NOCI tend to rise or fall? fall 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 thates be changed to a tendency to fall by adding NO2 Similarly, if you said the pressure of NOCl will tend to fall, can that be changed to a tendency to rise by adding NO? no 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)

clearly, there is 0 amount of NO present

therefore the shift must go from left to rigth

NOCl will fall/decrease in order to increase NO

b)

yes, via addition of NO

c)

K = [NO^2][Cl2] / [NOCl]^2

dG = -rT*lnK

K = exp(-41000/(8.314*(1003+273))

K = 0.020967

0.020967 = [NO^2][Cl2] / [NOCl]^2

0.020967 = [NO^2] * 6.50 / (9.10^2)

[NO] = sqrt(0.020967 *(9.10^2) / 6.50 )

[NO] = 0.5168 atm

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