The reaction 2A + B - C has the following proposed mechanism Step 1: A + B2D (fast equilibrium) Step 2: D + B → E slow Step 3: E +A- C +B fast The rate law consistent with this mechanism is: Rate = k[A][B}? Rate = k[AJ[B}? Rate = k[A][B] Rate = k[A}°[B]

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The reaction A + B » C + D rate = k[A][B]? has an initial rate of 0.0640 M/s. What will the initial rate be if [A] is halved and [B] is tripled? initial rate: M/s What will the initial rate be if [A] is tripled and [B] is halved? initial rate: M/s

The reaction described by H, (g) + 1,(g) → 2 HI(g) has an experimentally determined rate law of rate = k [H2][I2] Some proposed mechanisms for this reaction are: Mechanism A (1) H, (g) + L,(g) 2 HI(g) (one-step reaction) Mechanism B (1) 1,(g) =2 1(g) (fast, equilibrium) k_1 (2) H, (g) + 2 I(g) –→ 2 HI(g) (slow) Mechanism C (1) I, (g) = 2 I(g) (fast, equilibrium) k_ k, (2) I(g) + H, (g) –→ HI(g)+H(g) (slow) (3) H(g)+I(g) → HI(g) (fast) Which of these mechanisms are consistent with the observed rate law? O mechanism A O mechanism B O mechanism C In 1967, J. H. Sullivan showed that this reaction was dramatically catalyzed by light when the energy of the light was sufficient to break the I-I bond in an I, molecule. Which mechanism or mechanisms are consistent with both the rate law and this additional observation? O mechanism B O mechanism C O mechanism A

The reaction C 4 H 8 (g) longrightarrow2C 2 H 4 (g) has an activation energy of 262kJ / m * o * l . At 600.0 K, the rate constant, k, is 6.1 * 10 ^ - 8 * s ^ - 1 What is the value of the rate constant at 800.0 K? k=

For the interconversion between A and B as shown below, which of the following describes how the equilibrium constant (K) is related to the rate constants k1 and k -1 and to the amounts of A and B present at equilibrium? k1 A В k.1 OK = kj[A] and K = kj[B] k[B] K = kj[A] [B] K and K || [A] k1 [B] [A] K and K %3D k-1 k[A] K = kj[B]

A) In the proposed reaction mechanism below, the intermediate product is: A).  NO(g) B).  N2O2(g) C).  H2(g) D).  N2O(g)   B) The rate expression for a particular reaction is rate = k[A][B]^2. If the initial concentration of B is increased from 0.10M to 0.30M, the initial rate will increase by which of the following factors  A) 2 B) 3 C) 6 D) 9

Please don't provide hand writtin solution....

Consider the overall reaction 2A + B ⇌ 2C(g) with proposed mechanism for this reaction: A + B ⇌ C + D (slow) A+D ⇌ C (fast)What is the rate law for this proposed mechanism?

A mechanism was developed to explain the kinetics of the reaction;OCl– + H2O <-------> HOCl + OH– (fast equilibrium)I– + HOCl --------> HOI + Cl– (slow)OH– + HOI ------------> H2O + OI– (fast)Does the rate expression of this mechanism support or refute the data?Is there a catalyst for this reaction? Identify itIs/are there a reaction intermediate(s)? Identify it