A + B → Products
[A] [B] Initial Rate (M/s)
2.0 6.0 0.95
4.0 6.0 1.9
2.0 18.0 8.55
What is the overall reaction order?
22. The rate law for the chemical reaction shown below has been determined experimentally: Rate = k[O3][CI]. What is the overall order of the reaction? 03(g) + Cl(g) → O2(g) + ClO(g) a. 3 b. 5 d. 2 8. The following data were obtained for the hypothetical reaction A+B → products. [A]o (M) 4.0 2.0 4.0 [B]. (M) 6.0 6.0 3.0 Initial Rate (M/s) 1.60 0.80 0.40 What is the overall order of this reaction? a. 3 b. 12 c....
Please write in the number that represents the order. Only use a decimal if necessary. The overall order of a reaction with a rate constant of k = 3.0 x 10-5 M-0.5 s-1 is ._______________ The overall order of a reaction with a rate constant of k = 2.0 x 10-3 M-2 s-1 is ._________________ The overall order of a reaction with a rate constant of k = 6.0 x 10-4 M-1 s-1 is .________________ The overall order of a reaction with a...
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: Experiment [A] (M) [B] (M) Rate (M/s) 1 1.7 2.0 2 3.4 2.0 (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]x [B]y? Choose all correct possibilities. [A]...
24. 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: Experiment [A] (M) [B] (M) Rate (M/s) 1 2.0 1.4 2 4.0 1.4 (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]x [B]y? Choose all correct possibilities....
1) Block A started on the left, and block B on the right. The two moved towards the middle and collided.The image above depicts the result of the two blocks colliding. A) What is the total initial momentum of the blocks? B) What is the total final momentum of the blocks? C) What is the total initial kinetic energy of the blocks? D) What is the total final kinetic energy of the blocks? 2) What type of collision is this?...
March 4, 2020 5. The reaction of 'butyl-bromide (CH3)3CBr with water is represented by the equation: (CH3),CBr + H2O → (CH3)3COH + HBr The following data were obtained from three experiments: Experiment 1 Experiment 2 Experiment 3 Initial [(CH3)3CBr mol L-1 5.0 x 10-2 5.0 x 10-2 1.0 x 10-1 Initial [H0] mol L 2.0 x 10-2 4.0 x 102 | 4.0 x 10-2 Initial rate mol L-'min 2.0 x 10-6 2.0 x 10-6 4.0 x 10-6 a) What is...
The rate of a certain reaction is given by the following rate law: rate=k [N_]*[0] Use this information to answer the questions below. What is the reaction order in N2? What is the reaction order in O3? What is overall reaction order? At a certain concentration of N2 and O3, the initial rate of reaction is 2.0 x 105 M/s. What would the initial rate of the reaction be if the concentration of N2 were halved? Round your answer to...
just answers please, thanks a bunch Shown below are the initial conditions for four separate experiments for the reaction A+B2-> C. What is the rate equation for this reaction? Relative initial rate = Orate-k[A] Orate-k[B2] rate=k[A][B,12 o'rate-k[A]2[B2]2 Orate-k[A]2B2] In the reaction: N2 + 3H2 ->2NH3 the reactant Hy is consumed at a rate of 6.0 mol L-?min 1. What is the corresponding rate of the consumption of N2? O 6.0 mol L-4 min-1 O 12 mol L-1 min-1 10:3.0 mol...
The reaction, A → products, is known to be zeroth order with respect to the concentration of A and zeroth order overall. The rate constant for the reaction is 0.0750 M·hr-1 at a certain temperature. If the initial concentration of A is 0.875 M. What will be the concentration of A after 10.0 hr? Answer M How long would it take for 80.0% of the starting material (A) to undergo reaction? Answer hr The reaction, A → products, is known...
Consider the reaction A + B ? products From the following data obtained at a certain temperature, determine the rate law, the order of the reaction, and calculate the rate constant k. Experiment 1: [A] = 1.50 M; [B] = 1.50 M; Initial Rate = 3.20 x 10-1 M/s Experiment 2: [A] = 1.50 M; [B] = 2.50 M; Initial Rate = 3.20 x 10-1 M/s Experiment 3: [A] = 3.00 M; [B] = 1.50 M; Initial Rate = 6.40...