mechanism 1 overall reaction is 2NO + Cl2 --> 2NOCl NO + Cl2 = NOCl2     fast equilibrium NOCl2 + NO--->  2NOCl     slow rate law for mechanism 1 is rate=k[no2]^2[cl2] mechanism 2 Cl2 --> 2Cl     slow Cl + NO --> NOCl     fast rate law for this mechansim 2 is rate=k[cl2] i noticed that when the mechanism has a fast reaction at equilibrium, the rate law includes reactants form both fast and slow, whereas when the reaction has fast reactions not at equilibrium, the rate law is only the reactants from the slow step (rate determining step) why is the rate law different when the fast reaction is at equilibrium vs when the mechansim has a fast reaction not at equilibrium?

For the rate expression below, determine the exponents x and y for the following data. Rate = k [A] [B]Y Trial [A] M 1 2 3 4 0.10 Hint 0.20 0.10 0.30 x=1, y=0 x=0, y=1 Ox=1, y=2 x= 1, y=1 x=2, y=1 [B] M 0.20 0.20 0.10 Initial rate 4.6x10-2 9.2x10-² 2.3x10-2 0.30 1.4x10-1

For the following reaction: 2N2O5(g) ---> 4 NO2(g) + O2(g) The rate law is first order with respect to N2O5 and has a rate constant of 4.82 x 10-3 sec-1 .  Calculate the rate of reaction when the [N2O5] = 0.25M.

Based on the data below. Graphically determine the rate law for the reaction, and extract the rate constant and initial concentrations.    2 A -----> B Time [A] 5 11.4730407 10 7.6906092 15 5.15516951 20 3.45561346 25 2.31636698 30 1.55270722 35 1.04081077

The rate constant for the second order reaction 2 NO2 - 2 NO + O2 is 0.24 M's. If a 1.38 M sample of NO2 reacts for 47.7 seconds, what concentration of NO2 wil remain? Report your answer to two decimal places. |Al = - kt +|Alo InJAl = - kt + InlAlo TAI = kt + TAlo

What are the correct units for the rate constant in a zeroth order overall reaction rate? O M-1s1 O Ms1 s1 O None of these are correct.

None

Please make sure that the answer that I get is correct thank you so much

The integrated rate laws for zero-, first-, and second-order reaction may be arranged such that they resemble the equation for a straight line, y = mz +b. • Part A Order Integrated Rate Law Graph Slope [A] =- kt + [A]Jo -kt + In[A]o In[A] vs. t + = kt + TAT [A] vs. t -k The reactant concentration in a zero-order reaction was 7.00x102 M after 170 s and 3.00x102 M after 380 s. What is the rate constant for this reaction? 1 In[A] = -k Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash. 1 - vs t JA 2 • View Available Hint(s) ? koih = Value Units Submit Prevlous Anawera Part B Complete previous part(s) • Part C The reactant concentration in a first-order reaction was 6.60x102 Mafter 30.0 s and 7.70x10 Mafter 100 s. What is the rate constant for this reaction? Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a…