Identify any intermediate species + write the rate law for each step. *I'm confused on how to identify intermediate species and why the rate law for 2 = k2[Cl]2   Answers: Cl(g) and COCl(g) are intermediate species. The rate laws are k1[Cl2], k2[Cl]2, k3[Cl][CO], and k4[COCl][Cl2], respectively

Initial rate: 1.6 •10^-7mol/L•s K=6.4 •10^-9L/mol•s Rate law: k[HI]^2 Can you please show me the steps.

The rate law for the reaction NO2(g) + O2(g) is given by rate = - k[NO₂] NO(g) + 03 (g) If the following is the mechanism for the reaction, which of the following statements correctly describe the reaction? Check all that apply. NO2(g) NO(g) + O(g) - O(g) + O2(g) 03 (g) The reaction is 2nd order overall. The first step is the slow step. Doubling NO, would quadruple the rate. Cutting O, in half would decrease the rate by a factor of 2. The molecularity of the first step is 1. Both steps are termolecular. None of the above

Consider this reaction: 2SO3 (g) →2SO₂(g) + O₂(g) At a certain temperature it obeys this rate law. rate = (0.894 M¹-s¹) [S0₂] Suppose a vessel contains SO3 at a concentration of 0.390 M. Calculate the concentration of SO3 in the vessel 8.60 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M Explanation Check 0 10 Q Search a Ⓒ2023 McGraw Hill LLC. All Rights Reserved. Terms of Use O Privacy Center

3. Consider the reaction below: 2NO (g) + Cl,(g)'n 2NOCI (g) A mechanism involving these steps has been proposed for the reaction: Step 1: NO (g) + Cl,(g)'n NOCI, (g) Step 2: NOCI, (g) + NO(g)'n 2NOCI (g) The rate law for the reaction is given by rate = k[NO][Cl]. (a) What is the reaction intermediate? (b) Which is the rate-determining step? (c) Is the rate-determining step unimolecular, bimolecular, or termolecular? Why?

Click in the answer box to activate the palette. Enter the general form of the rate law for the following process. Represent the order as  n, n', and so forth.  Complete the equation using brackets, [], to represent concentration.  2Cu(g) + O2(g) → 2CuO(g)

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The exponents in a rate law describe the effects of the reactant concentrations on the reaction rate and define the reaction order. Consider a reaction for which the rate law is: rate = k[A]m[B]n If m is 1, the reaction is first order with respect to A. If the exponent is 2, the reaction is second order with respect to A. If n is 1, the reaction is first order in B. If m or n is zero, the reaction is zero order in A or B. If m = 1 and n = 1, the overall order of the reaction is second. (m + n = 1 + 1 = 2). 1. What is the difference between a reaction rate and a reaction's rate constant? 2. What does it mean if a reaction is zero order with respect to a reactant?  3. Doubling the concentration of a reactant increases the rate of a reaction four times. What is the order of the reaction with respect to that reactant? 4. Doubling the concentration of a reactant increases the rate of a reaction four times. Tripling the concentration of a different reactant increases the rate of a reaction…

The reaction 2 NO(g) + O2(g) --> 2 NO2(g) proceeds through the following mechanism: 2 NO(g) --> N2O2(g)N2O2(g) + O2(g) --> 2 NO2(g) (a) The second step of this mechanism is rate-determining (slow). What is the rate law for this reaction? Rate = k [NO] [O2] Rate = k [NO]2 [O2]     Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 (b) What would the rate law be if the first step of this mechanism were rate-determining? Rate = k [NO] [O2] Rate = k [NO]2 [O2]     Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 Rate = k [NO]