Find the initial concentration of NO2 if the concentration after 2.00 min is 0.113. k = 0.331 1/(M * s)
2 NO2 (g) + N2 (g) --> 2 N2O (g) + O2 (g)
This is a second order reaction.
(1/A) - (1/Ao) = akt
Plug in 0.113 for A, 0.331 for k, 2 for a,and 2 for t then solv for Ao.
True, however, I keep getting a negative value which is not possible.
What is the unit for 0.113? Check the numbers in the post to make sure all are ok.
its concentration, so it should be mol/L
To find the initial concentration of NO2, we can use the given rate constant (k) and the concentration after a certain time.
The given reaction is:
2 NO2 (g) + N2 (g) --> 2 N2O (g) + O2 (g)
From the balanced equation, we can see that the stoichiometric coefficient of NO2 is 2.
We can use the integrated rate equation for a second-order reaction to relate the initial concentration (NO2ₒ) with the concentration at a given time (NO2t):
1/NO2t - 1/NO2ₒ = kt
Given:
NO2t = 0.113 M (concentration after 2.00 min)
k = 0.331 1/(M * s) (rate constant)
Now, we can substitute the given values into the equation to solve for NO2ₒ:
1/NO2t - 1/NO2ₒ = kt
1/0.113 - 1/NO2ₒ = 0.331 * 2.00
Solving this equation will give us the initial concentration of NO2.