Consider the following equilibrium: AG5.4 kJ Now suppose a reaction vessel is fi

Question

Consider the following equilibrium: AG5.4 kJ Now suppose a reaction vessel is filled with 5.64 atm of dinitrogen tetroxide (N-04 at 30·°C. Answer the following questions about this system rise x 1 Under these conditions, will the pressure of N2O4 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 N2O4 will tend to rise, can that be changed to a tendency to fall by adding NO2? Similarly, if you said the pressure of i end to fall, can that be changed to a tendency to rise by adding NO,? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO2 needed to reverse it Round your answer to 2 significant digits O yes no atm

Explanation / Answer

     N2O4(g) <====> 2NO2(g)

pressure of N2O4 tend to fall

yes,

DG0 = -RTlnKp

5.4*10^3 = -8.314*303.15lnKp

   Kp = 0.117

   Kp = pNO2^2/pN2O4

0.117 = (2X)^2/(5.64-X)

X = 0.392

minimum pressure of NO2 required to reverse the process = 2*0.39 = 0.78 atm

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