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Calculate the rate at which N2O4 is formed in the following reaction at the moment in time when NO2 is being consumed at a rate of 0.0521 M/s.

2NO2(g) <-> N2O4 (g)

I am not really sure how to go about this problem.

rate = k (N2O4)

d(NO2)/dt = -2 d(N2O4)/dt

This is what I have so far

  • Chemistry -

    Isn't the rate of appearance of N2O4 just 1/2 that of disappearance of NO2?

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