Respuesta :
Answer : The rate order of [tex]Cl_2[/tex] is, 1
Explanation :
The given balanced reaction is,
[tex]2NO(g)+Cl_2(g)\rightarrow 2NOCl(g)[/tex]
As we know that rate is an experimentally determined value. So, we can not determine the rate law by looking at the reaction.
The general rate law expression will be,
[tex]R=k[NO]^x[Cl_2]^y[/tex]
where,
R = rate
k = rate constant
[tex][NO][/tex] and [tex][Cl_2][/tex] = concentration of NO and [tex]Cl_2[/tex] reactant
x and y are the order of the reaction of NO and [tex]Cl_2[/tex] reactant respectively.
To calculate the order with respect to [tex]Cl_2[/tex], we can compare the rates of two reactions in which the concentration of NO remains the same.
Now we have to compare the rates 2 and 3 experiment because in this NO concentration remains same and we get:
[tex]\frac{R_2}{R_3}=\frac{k[NO]^x[Cl_2]^y}{k[NO]^x[Cl_2]^y}[/tex]
[tex]\frac{0.08}{0.16}=\frac{k[0.8]^x[0.3]^y}{k[0.8]^x[0.6]^y}[/tex]
[tex]\frac{1}{2}=\frac{(0.3)^y}{(0.6)^y}[/tex]
[tex]\frac{1}{2}=(\frac{1}{2})^y[/tex]
[tex]y=1[/tex]
Therefore, the rate order of [tex]Cl_2[/tex] is, 1
