Mechanism with a slow initial step:
2NO(g)+Br2(g)--->2NOBr
-The experimentally determined rate law for this reaction is second order in NO and first order in Br2
Rate=K[NO]^2[Br2]Mechanism with a fast initial step:
Step1:NO+Br2<=>NOBr2 Fast Step
Step2: NOBr2+NO<=>2NOBr
Since it is a rate law with a slow initial we need to set up an equation like this:
Ina a dynamic equilibrium the forward reaction rate equals the reverse reaction rate.
[NOBr2]=K(1)/K(-1)[NO]^2[Br2]
Rate=K(2)*K(1)/K(-1)[NO][Br2][NO]=K[NO]^2[Br2]
"AP Chemistry Study Guide- Kinetics." AP Chemistry Study Guide- Kinetics. N.p., n.d. Web. 30 May 2014.
2NO(g)+Br2(g)--->2NOBr
-The experimentally determined rate law for this reaction is second order in NO and first order in Br2
Rate=K[NO]^2[Br2]Mechanism with a fast initial step:
Step1:NO+Br2<=>NOBr2 Fast Step
Step2: NOBr2+NO<=>2NOBr
Since it is a rate law with a slow initial we need to set up an equation like this:
Ina a dynamic equilibrium the forward reaction rate equals the reverse reaction rate.
[NOBr2]=K(1)/K(-1)[NO]^2[Br2]
Rate=K(2)*K(1)/K(-1)[NO][Br2][NO]=K[NO]^2[Br2]
"AP Chemistry Study Guide- Kinetics." AP Chemistry Study Guide- Kinetics. N.p., n.d. Web. 30 May 2014.
"Rate Law for a Mechanism with a Fast Initial Step." YouTube. YouTube, n.d. Web. 29 May 2014.
If the mechanism has a slow initial step the process is much simpler. All you do is take the reactants and put them into a rate law.
Na^++Cl^-=NaCl
Rate law=K[Na+][Cl]
Na^++Cl^-=NaCl
Rate law=K[Na+][Cl]