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 6.87 atm of dinitrogen tetroxide (N204) at 736·°C. Answer the following questions about this system rise Under these conditions, will the pressure of N204 tend to rise or fal? fall Is it possible to reverse this tendency by adding NO2? In other words, if you said the pressure of N24 will tend to rise, can that be changed to a tendency to fall by adding NO2? Similarly, if you said the pressure of N,0, will tend to fall, can that be changed to a tendency to rise by adding NO2 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 yes no atm

Explanation / Answer

a)

there is no N2O4, therefore, NO must produce N2O4, there is increase/rise of N2O4

b)

yes, we can add enough n2O4 to counterbalance it

c)

dG = -rT*ln(k)=

K = exp(-dG/(RT))

K = exp(54000/8.314/(736+273)) = 624.61

now..

K = N2O4 / (NO)^2

624.61 = N2O4 / (6.87^2)

N2O4 = 624.61*(6.87^2)

N2O4 = 29479.65 atm

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