how do you get the answer for The reaction 2NO2 → 2O2 + N2 is a third order reaction with respect to NO2. If the rate of disappearance of NO2 is 25.0 mol/Ls when the concentration of NO2 is 0.10 mol/L, what is the new rate when the concentration of NO2 changes to 0.30mol/L.
Question
how do you get the answer for The reaction 2NO2 → 2O2 + N2 is a third order reaction with respect to NO2. If the rate of disappearance of NO2 is 25.0 mol/Ls when the concentration of NO2 is 0.10 mol/L, what is the new rate when the concentration of NO2 changes to 0.30mol/L.
Solution
The rate law for this reaction is Rate = k[NO2]^3 because it's a third order reaction with respect to NO2.
Given that the rate of disappearance of NO2 is 25.0 mol/Ls when the concentration of NO2 is 0.10 mol/L, we can find the rate constant (k) using the rate law:
25.0 mol/Ls = k(0.10 mol/L)^3 Solving for k gives k = 25000 L^2/mol^2s.
Now, we can find the new rate when the concentration of NO2 changes to 0.30 mol/L using the rate law and the value of k:
Rate = 25000 L^2/mol^2s * (0.30 mol/L)^3 = 675 mol/Ls.
So, the new rate of the reaction when the concentration of NO2 changes to 0.30 mol/L is 675 mol/Ls.
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