2N2O(g) → 2N2(g) + O2(g)
d[N2O]/dt = -5.8×10-4 M/s at a particular temperature and set of concentrations.
What are d[O2]/dt and d[N2]/dt?
d[O2]/dt =
d[N2]/dt =
What is the rate of the reaction?
my answer for the first one im getting -.00016 and the second one 2.9e-4
and i don't understand how to do the last part, do i add up all the values together?
To find d[O2]/dt and d[N2]/dt, you can use the stoichiometry of the reaction and the given rate for d[N2O]/dt.
From the balanced chemical equation, we see that the coefficients of N2O, N2, and O2 are 2, 2, and 1, respectively.
Using the stoichiometry, we can relate the rates:
d[O2]/dt = (1/2) * d[N2O]/dt
d[O2]/dt = (1/2) * (-5.8×10^(-4) M/s) = -2.9×10^(-4) M/s
d[N2]/dt = (2/2) * d[N2O]/dt
d[N2]/dt = (2/2) * (-5.8×10^(-4) M/s) = -5.8×10^(-4) M/s
Therefore, d[O2]/dt = -2.9×10^(-4) M/s and d[N2]/dt = -5.8×10^(-4) M/s.
To calculate the overall rate of the reaction, we can use any of the rate expressions since they should be equal due to the stoichiometry.
Rate = d[N2O]/dt = -5.8×10^(-4) M/s
So, the overall rate of the reaction is -5.8×10^(-4) M/s.