What is the rate law for the overall reaction?
consider the following mechanism step 1: A--)B + C (slow) step 2: C +D --->E (fast) overall A +D ---->B +E what is the rate law for the overall reaction? HELP!
What is the rate law for the overall reaction for this mechanism?
We need to get rid of CD in the slow step. C+D=CD therefore, we rewrite the elementary reaction as, CD+D→CD^2(slow) C+D+D→CD^2(slow) C+2D→CD^2(slow) Rate=k[C][D]²
Determine the rate law for the overall reaction?
Consider the following mechanism. Step 1: 2A ↔ B + C (equilibrium) Step 2: B + D → E (slow) Overall: 2A + D → C + E Determine the rate law for the overall reaction (where the overall rate constant is represented as k). Can you show me how to do this?
Determine the rate law for the overall reaction?
C is an intermediate it ought to be included in the rate equation, especially if this is the rate limiting step in the mechanism. BUT, if the reaction is zero order with regards to C, then it isn't included. A + C + D--> C + E + B A +D --> B + E is the overall reaction. the rate of the reaction is dictated by the slow step rate = k[C][D] the Kc for this reaction = [E] / [D][C] to determine [C], we rearrange the equation: [C] = [E] / Kc[D] substitute this into the rate equation that you have determined your rate equation: rate = k[C][D] rate = k {[E] / Kc[D]} x [D] rate = k1[E]
Determine the rate law for the overall reaction (where the overall rate constant is represented as k).?
The rate law is determined by the slow step of the mechanism. Because the first step of this mechanism is the slow step, you can directly write the rate law for the reaction as: Rate = k[A][B]
Determine the rate law for the overall reaction (where the overall rate constant is represented as k).?
Ready? Usually stoichiometry of a reaction (# of moles, etc.) determines the rate law, but not in this case. For overall reaction, you look at the slow step (a.k.a. rate limiting transition state). The rate law for the slow step is: rate=k [C] [D] Since [C] is an intermediate, we need to substitute it using equilibrium step. We know equilibrium means rate of forward reaction = rate of reverse reaction. so, k[A] = k[B] [C] <------- shows equilibrium. Then solve for [C] to get: k[A]/k[B]= [C]. Now, you simply substitute in the initial rate equation you got from the slow step to get: rate= k(slow) {k[A]/[B]} x [D] So, your answer my friend is rate= k{ [A] [D] } / [B].
PLEASE HELP Determine the rate law for the overall reaction (where the overall rate constant is represented as?
When looking at the elementary steps of a reaction the overall rate of the reaction is equal to the slow step (aka the rate determining step). For this reaction that would be step 1. The rate expressed in step 1 (bimolecular) is rate=k[A]^2 Since there are no intermediates, this also represents the overall equation and is the final answer.