This is an incomplete question, here is a complete question and an image is attached below.
The following diagrams represent mixtures of NO(g) and O₂(g). These two substances react as follows:
[tex]2NO(g)+O_2(g)\rightarrow 2NO_2(g)[/tex]
It has been determined experimentally that the rate is second order in NO and first order in O₂.
Based on this fact, which of the following mixtures will have the fastest initial rate?
The mixture (1). The mixture (2). The mixture (3).
Answer : The mixture 1 has the fastest initial rate.
Explanation :
The given chemical reaction is:
[tex]2NO(g)+O_2(g)\rightarrow 2NO_2(g)[/tex]
The rate law expression is:
[tex]Rate=k[NO]^2[O_2][/tex]
Now we have to determine the number of molecules of [tex]NO\text{ and }O_2[/tex]
In mixture 1 : There are 5 [tex]NO[/tex] and 4 [tex]O_2[/tex] molecules.
In mixture 2 : There are 7 [tex]NO[/tex] and 2 [tex]O_2[/tex] molecules.
In mixture 3 : There are 3 [tex]NO[/tex] and 5 [tex]O_2[/tex] molecules.
Now we have to determine the rate law expression for mixture 1, 2 and 3.
The rate law expression for mixture 1 is:
[tex]Rate=k[NO]^2[O_2][/tex]
[tex]Rate=k(5)^2\times (4)[/tex]
[tex]Rate=k(100)[/tex]
The rate law expression for mixture 2 is:
[tex]Rate=k[NO]^2[O_2][/tex]
[tex]Rate=k(7)^2\times (2)[/tex]
[tex]Rate=k(98)[/tex]
The rate law expression for mixture 3 is:
[tex]Rate=k[NO]^2[O_2][/tex]
[tex]Rate=k(3)^2\times (5)[/tex]
[tex]Rate=k(45)[/tex]
Hence, the mixture 1 has the fastest initial rate.
