For the reaction: 2 N2O5 (g) → 4 NO2 (g) + O2 (g)
The experimental data for this reaction is :
t = 0.0 s [N2O5] = 0.80 M [NO2] = 0.0 M [O2] = 0.0 M
t = 20.0 s [N2O5] = 0.60 M [NO2] = 0.40 M [O2] = 0.10 M
What is the average rate of reaction during this time interval?
avg rate = #M/time
That will be in M/s, right?
And I think you're playing pretty fast and loose with those = signs
The average rate of this reaction is -1/2[delta(N2O5)/delta t] = -1/2[(0.60M - 0.80M)/(20s-0s)] = -1/2(-.20/20) = -1/2(-0.01) = + 0.005 M/s
To find the average rate of reaction during the given time interval, we need to calculate the change in the concentration of the reactant or product over that time interval.
In this case, we can choose either N2O5, NO2, or O2 to calculate the average rate of reaction. Let's choose N2O5.
The average rate of reaction is given by the formula:
Average rate = (Change in concentration of N2O5) / (Change in time)
First, we need to determine the change in concentration of N2O5. From the given data:
[N2O5] at t = 0.0 s = 0.80 M
[N2O5] at t = 20.0 s = 0.60 M
Change in concentration of N2O5 = [N2O5] at t = 20.0 s - [N2O5] at t = 0.0 s
= 0.60 M - 0.80 M
= -0.20 M
Next, we calculate the change in time:
Change in time = t = 20.0 s - 0.0 s
= 20.0 s
Now, we can calculate the average rate of reaction:
Average rate = (Change in concentration of N2O5) / (Change in time)
= (-0.20 M) / (20.0 s)
= -0.01 M/s
Therefore, the average rate of reaction during this time interval is -0.01 M/s.