Example: For the following reaction 2H2 (g) + 2NO(g) → N2 (g) + 2H2O(g) the experimentally determined rate law is rate = k [H2][NOJ? For each of the following two mechanisms, state whether it is possible or not possible for it to describe the overall reaction. Show all of your work Mechanism I Mechanism II H2(g) + NO(g) → H;O(g) + N(g) (slow) H2 (g) + 2NO(g) → H¿O(g) + N¿O(g) (slow) N(g) + NO(g) → N2 (g) + O(g) (fast) N2O(g) + H2 (g) → N2 (g) + H2O(g) (fast) O(g) + H2 (g) → H¿O(g) (fast)

Consider the following multistep reaction: C+D = CD (fast) CD+D →CD2 (slow) CD2 +D→CD3 (fast) C+ 3D →CD3 (overall) Based on this mechanism, determine the rate law for the overall reaction. Express your answer in standard MasteringChemistry format. For example, if the rate law is k[C]° [D]? type k* [C]^3* [D]^2. • View Available Hint(s)

Suppose the reduction of nitric oxide proceeds by the following mechanism: step elementary reaction rate constant 1 H, (g) + 2NO (g) → N,0 (g)+ H,0 (g) k1 H, (g) + N,0 (g) → N2 (g) + H20 (g) k2 Suppose also k, « k,. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. rate = k|| Note: your answer should not contain the concentrations of any intermediates.

rate constant 1 H₂(g) + 2NO(g) N₂O(g) + H₂O(g) k₁ 2 H₂(g) + N₂O(g) → N₂(g) + H₂O(g) k₂ Suppose also k₁«k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k1, K₂, and (if necessary) the rate constants k-1 and k-2 for the reverse of the two elementary reactions in the mechanism. step elementary reaction t k = A 00 X

A possible mechanism for the reaction described by: CO(g) + Cl2(g) → COCl2(g) 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.

A possible mechanism for the next decomposition reaction is             A(g) ⇄ 2B(g) + C        (fast equilibrium)             C + A(g) → 2B(g)      (slow) What is a rate law that is consistent with this mechanism?

The rate law for: Cl2(g) + CHCl3(g) → HCl(g) + CCl4(g) is rate = k [Cl2]1/2 [CHCl3]3/4  The units for the rate constant are: M−1sec−1 M−1/4sec−1 sec−1 M−3/4sec−1 M−2sec−1

O KINETICS AND EQUILIBRIUM Writing the rate law implied by a simple mechanism H₂(g) + ICI(g) - 1 HI(g) + HCl(g) k₁ 2 HI(g) + ICl(g) 1₂(g) + HCl(g) k₂ Suppose also k₁«k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k₁, K₂, and (if necessary) the rate constants k.₁ and k-2 for the reverse of the two elementary reactions in the mechanism. Explanation Check rate = k0 = 0 k = JUL 16 L tv W MacBook Air ローロ 00 X 0- © 2023 McGraw Hill LLC. All Rights Reserved. Terms of 70

The reaction 2H2(g) + 2NO(g) ----> 2H2O(g) + N2(g) is a first-order in H2 and second order in NO. What is the rate law

A: Consider the following reaction: N2H5+  +  4 Fe(CN)63-  -->  N2(g)  +  5 H+  +  4 Fe(CN)64- Based on just this information, which species concentration(s) could most likely be in the rate law?  (Check ALL correct answers.) Group of answer choices Fe(CN)64- Fe(CN)63- N2H5+ N2(g) H+   B: Consider the following reaction: 2 C19H16O --> C38H32O2,  also written as: 2 Monomer --> Dimer Given the following kinetics plot, what is the rate order with respect to Monomer disappearance?   Group of answer choices 2nd 3rd Zero 1st