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 determine d[O2]/dt and d[N2]/dt, we need to use the stoichiometry of the reaction. According to the balanced chemical equation:

2N2O(g) → 2N2(g) + O2(g)

We can see that for every mole of N2O that reacts, 1 mole of O2 is produced and 2 moles of N2 are produced. Therefore, the rate of change of O2 concentration (d[O2]/dt) is half of the rate of change of N2O concentration (d[N2O]/dt) and the rate of change of N2 concentration (d[N2]/dt) is equal to the rate of change of N2O concentration (d[N2O]/dt).

Given d[N2O]/dt = -5.8×10^-4 M/s, we can calculate the values:

d[O2]/dt = (1/2) * d[N2O]/dt = (1/2) * (-5.8×10^-4 M/s)

d[O2]/dt = -2.9×10^-4 M/s

d[N2]/dt = d[N2O]/dt = -5.8×10^-4 M/s

For the last part, to determine the rate of the reaction, we add up the rates of change of all the species involved in the reaction. Since the stoichiometric coefficients are 2 for N2O and N2O, and 1 for O2, we can sum up their respective rates of change:

Rate of reaction = |d[N2O]/dt| + |d[N2]/dt| + |d[O2]/dt|

Rate of reaction = |-5.8×10^-4 M/s| + |-5.8×10^-4 M/s| + |-2.9×10^-4 M/s|

Rate of reaction = 14.5×10^-4 M/s

Therefore, the rate of the reaction is 14.5×10^-4 M/s or 1.45×10^-2 M/s.

To determine d[O2]/dt and d[N2]/dt, we can use the stoichiometric coefficients from the balanced equation:

2N2O(g) → 2N2(g) + O2(g)

Given that d[N2O]/dt = -5.8×10-4 M/s, we can use the stoichiometry to find the rates of change of O2 and N2.

According to the balanced equation, for every 2 moles of N2O reacted, 1 mole of O2 is produced. Therefore, the rate of change of O2 is half the rate of change of N2O:

d[O2]/dt = -5.8×10-4 M/s / 2 = -2.9×10-4 M/s

Similarly, for every 2 moles of N2O reacted, 2 moles of N2 are produced. Therefore, the rate of change of N2 is the same as the rate of change of N2O:

d[N2]/dt = -5.8×10-4 M/s

Now, to determine the overall rate of the reaction, we can use the rate expression coefficients from the balanced equation as well. In this case, the coefficients are equal:

Rate = -d[N2O]/dt = -d[O2]/dt = -d[N2]/dt = -5.8×10-4 M/s

So, the rate of the reaction is -5.8×10-4 M/s. Note that the negative sign indicates a decrease in concentration over time.