If you have a reaction A + B --> C, and the rate equation is Rate = k [A], what can you infer about the mechanism of the reaction?

The rate law for the reaction 2A → B  is second order in A. The following figure represents samples with different concentrations of A; the red spheres represent molecules of A. In which sample will the reaction proceed most rapidly?

6) For the reaction 3A + 2B2C + D + E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: Rate (M/s) 1.9 x 108 [A] (M) [B] (M) 1.0 x 10¹2 1.0 x 10¹1 9.5 x 108 5.0 x 10¹2 1.0 x 1011 3 5.7 x 108 1.0 x 10¹2 3.0 x 10¹1 a) Write the rate law for this reaction. rate=[A]*[B]Y 3 3.0 x 10" 1.0 x10¹2 y = ²/ 5.0×10 1.0x1010 X = = 1 1.0x10" 1.0 ×1010 5 3=1 b) What is the overall order of the reaction? c) Calculate the rate law constant, k (including units). x = = 1.0x10" 1.0 x 10" 1 lom C²

The reaction described by H, (g) + L,(g) 2 HI(g) has an experimentally determined rate law of rate = k [H2] [I2] Some proposed mechanisms for this reaction are: Mechanism A k1 (1) H,(g) + L,(g) → 2 HI(g) (one-step reaction) Mechanism B k1 =2 I(g) k_1 (1) L(g) ; (fast, equilibrium) k2 (2) H, (g) + 2 I(g) 2 HI(g) (slow) Mechanism C k1 = 2 I(g) (fast, equilibrium) (1) k2 (2) I(g) + H, (g) HI(g) + H(g) (slow) (3) H(g) + I(g) → HI(g) (fast) Question Sourc

Using the data in the table, determine the rate constant of the reaction and select the appropriate units. k = A + 2B → C + D Trial [A] (M) [B] (M) Rate (M/s) 1 0.260 0.260 2 0.260 0.520 3 0.520 0.260 Units 0.0199 0.0199 0.0796

You are studying the reaction A₂(g)+B₂(g) →2AB(g) to determine its rate law. Assuming that you have a valid exper-imental procedure for obtaining [A₂] and [B₂] at various times,explain how you determine (a) the initial rate, (b) the reaction orders, and (c) the rate constant.

You and your lab partner are studying the rate of a reaction, A + B --> C. You make measurements of the initial rate under the following conditions: (b) For a reaction of the form, A + B + C --> reaction from the choices below. (a) Which of the following reactant concentrations could you use for experiment 3 in order to determine the rate law, assuming that the rate law is of the form, Rate = k [A] [B]Y? Choose all correct possibilities. O [A] = 0.2 and [B] = 1.0 O [A] = 0.4 and [B] = 1.0 O [A] = 0.8 and [B] = 0.5 O [A] = 0.6 and [B] = 0.5 O [A] = 0.2 and [B] = 1.5 O [A] = 0.4 and [B] = 0.5 O [A] = 0.4 and [B] = 1.5 O [A] = 1.0 and [B] = 0.5 O Rate = K[A][B][C] O Rate = K[A][C] O Rate = K[A]²[C] T O Rate = k[A][C]² O Rate = K[A]²[C]² O Rate = K[A]³ [c] O Rate = K[A][C]³ the following Experiment [A] (M) [B] (M) Rate (M/s) 0.5 0.5 The rate will be the original rate multiplied by a factor of 0.2 0.4 (c) By what factor will the rate of the reaction described in part (b) above change if the…

What is the effective rate constant [in units that combine M and min] for the reaction with rate law v = k[A][B]2 where k = 0.54 M -2 min-1 if the initial concentration of B is 3.7 molar and that of A is 0.032 molar?

Given the following data, determine the rate constant of the reaction 2NO(g) + Cl2(g) –→ 2NOCI(g) Experiment [NO] (M) |Ck] (M) Rate (M/s) 0.0300 0.0100 3.4 x 104 0.0150 0.0100 8.5 x 10-5 3 0.0150 0.0400 3.4 x 104

Hydrogen peroxide decomposes spontaneously to yield water and oxygen gas according to the reaction equation 2H,0, (aq) — 2н,00) + 0,(8) The activation energy for this reaction is 75 kJ-mol-1. In the presence of a metal catalyst, the activation energy is lowered to 49 kJ-mol-1. At what temperature would the non-catalyzed reaction need to be run to have a rate equal to that of the metal-catalyzed reaction at 25 °C? T = K