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 2.33 atm of nitrogen monoxide (NO) and 6.82 atm of nitrosyl chloride (NOC) at 576. °C. Answer the following questions about this system 10 rise Under these conditions, will the pressure of NO tend to rise or fall? fall Is it possible to reverse this tendency by adding CI2? In other words, if you said the pressure of NO will tend to rise, can that be changed to a tendency to fall by adding Cl2? Similarly, if you said the pressure of NO will tend to fall, can that be changed to a tendency to rise by adding Cl2? yes no If you said the tendency can be reversed in the second question, calculate it. atm Round your answer to 2 significant digits

Explanation / Answer

under these conditions pressure of NO tend to rise

yes , it is possible to reverse the tendency by adding NO

DG0 = - RTlnk

-41*10^3 = -8.314*849.15lnkp

Kp = 332.8

Kp = pNOCl^2/pNO^2*pCl2

(332.8) = (6.82-x)^2/((x^2*(2.33-(x/2)))

x = 0.243

at equilibrium,

pNOCl = 6.82-0.243 = 6.577 atm

pNO = x = 0.243 atm

pCl2 = x/2 = 0.243/2 = 0.121 atm

minimum pressure required to reverse the process is above 0.12 atm

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