steady state approximation rate law for this reaction:
k1
Br2 <--> 2Br
k-1 (this refers to reverse of Br2 to 2Br)
k2
2Br + H2 ----> 2HBr
steady state approximation rate law for this reaction: k1 Br2 <--> 2Br k-1 (this refers to...
Derive using steady state approximation for both H ans Br atoms. H2(g) + Br2(g) -> 2HBr(g)
Consider the reaction mechanism: k A+B= X k-1 X+A_K2C+D Using the steady-state approximation, show that an effective rate equation for [C] is rate=d[C]/dt = -keff[A] [B]. What is keff in terms of ki, k-1, k2, [A], and [B]? A kzkz[A][B]/(k-1[B]+k2) B kık2[B]/(k-1[B]+k2) C kzkz/(k-1+k2[A]) D kık2/k-1 E ki
find k1, kN/kS and k-1/ks the values are: Steady-state approximation, competition experiments. The solvolysis of 2-octylmethane- sulfonate (RX) in aqueous solutions containing azide ions yields a mixture of alcohol and azide 35 Two mechanisms should be considered: ROH H+ X ROH H+ X H20 H2O IR versus RX kNIN3) kNIN3] RN3 X RN Derive the steady-state rate law for each, and the expression for the product ratio, ORN3MROHI, in terms of the rate constants and IN3 J. Use the following...
2.4 Using the steady state approximation derive the rate expression for the formation of C in the reaction 2A + B (g) → 2C(9) on the basis of the following proposed mechanism ki ZA K-1 X + B K2 20 To what expression does the rate expression reduce if the second reaction is slow, the initial equilibrium established very rapidly. (8)
Step 1: NO(g) + O2(g) ---> NO2(g) + O(g) rate= k1 Step 2: NO(g) + ) --> NO2 (g) rate = k2 suppose that k1<<k2, That is the first step is much slower than the second. Write the balanced chem equation for the overall chemical rxn Write the experimentally observable rate law for the overall reaction. (no reaction concentrations) rate=k() Express the rate constant k for the overall reaction in terms of k1, k2 and (if necessary) the rate constant...
6. Use the steady state approximation to derive a rate law for d[D/dt with the following mechanism A+B +C Step 1) Step 2) 7. a) What is the rate law for the mechanism in question (6) if the second step is the rate-limiting step? b) Express the activation energy for the overall reaction in terms of the activation energies for each step in the mechanism from part (a)
The reaction 2A + B → C occurs by the following 2 step mechanism: A + B ------(k1)------> AB AB ------(-k1) ------> A+B AB + A ----- (k2)------> C Apply the steady-state approximation for the reaction intermediate concentration to obtain the overall rate law from this mechanism: a) k1 [A][B] b) k1k2[A][B]/((-k1) - k2[A]) c) k1k2[A]^2[B]/((-k1)+k2[A])
For the following reaction, Kp = 2.8 ✕ 104 at 1630 K. H2(g) + Br2(g) equilibrium reaction arrow 2 HBr(g) What is the value of Kp for the following reactions at 1630 K? (a) HBr(g) equilibrium reaction arrow 1/2 H2(g) + 1/2 Br2(g) (b) 2HBr(g) equilibrium reaction arrow H2(g) + Br2(g) (c) 1/2H2(g) + 1/2 Br2(g) equilibrium reaction arrow HBr(g)
For the reaction H2(g) + Br2(g) → 2HBr(g) Kp = 3.6 x 104 at 1494 K. What is the value of Kp for the following reaction at 1494 K? 42 H2(g) + / Br2(g) HBr(g) K". p Submit
QUestion about Steady-State Approximation! THank you for answering. find the rate law for the production of NOZE 2NO3 + Fz2NO3F ( NO 2 + Ez teh y NO2F2 I Nozz ke NO2F+F 1 Ft NO2 kz NOF o please explain whole solving process ③ in the last sequence, =ck [F] [NO2] + kz [NO2Fz] which is correct? and why? ... and [F] [NO]