Using the experiments and calculate the order with respect to A and B. Then calculate complete rate law.
A + 2B-30 Experiment Number [A] (M) [B] (M) Initial Rate (M/s) 1 0.112 0.58 0.87...
1-2. Rate data were obtained for the following reaction A (g) + 2B (g) -C(8) Experiment Initial (Al Initial [B] 1 Initial Rate, Ms 0.15 0.10 0.45 2 0.30 0.10 0.9 3 0.15 0.20 1.8 1. What is the rate law of the above reaction? This question is for the test taker to work out independently, any help from others including online service is prohibited. rate = K[A][B]^2 O rate = K[A](B) rate = k[A]^2[B] rate = K[A] O rate...
12 of 15 Use the table below to calculate the initial reaction rate of the following reaction: 2AB+C [A]/M t/s 0.100 0.045 O 0.006 M/S -0.006 M/S -0.012 M/s 0.012 M/s 13 of 15 Use the table below to determine the rate law for the reaction A-2B: Initial rate/Ms Experiment Initial [A]/M 1 0.010 0.020 0.040 0.0010 0.0040 0.0160 2 3 1 rate=k O rate=k[A] O rate=k[A]2 O rate=k[A][B]2
The experimental data below were obtained. Experiment # [A] (M) [B] (M) Initial Rate (M/s) 1 1.80 3.54 4.52 2 1.80 7.08 4.52 3 5.40 3.54 40.68 What is the rate law for this reaction?
1. For the reaction, A + 2B + C +2D, some measurements of the initial rate of reaction at varying concentration gave the following data. run # [A] [B] rate, moll's eman 19 1 0.100 0.200 0.000360 20.150 0.200 0.000540 3 0.150 0.250 0.001055 012 noite a. the rate law is therefore: rate = k[A[B] b. the rate law is therefore: rate = k[A][B]', UX physHouten c. the rate law is therefore: rate = K[A[B] d. the rate law is...
Based on the data below, calculate the rate constant, k, for the reaction A + 2B --> C + D, if the rate law is rate = k[A]2[B]0. Experiment [A] M [B] M Initial Rate (M / s) 1 0.110 0.150 0.145 2 0.220 0.150 0.581 3 0.220 0.450 0.581
Experiment Initial [A] Initial [B] Initial [C] Initial Rate of Reaction 1 0.1 M 0.1 M 0.2 M 4 x 10^(-4) M/min 2 0.3 M 0.2 M 0.2 M 1.2 x 10^(-3) M/min 3 0.1 M 0.3 M 0.2 M 4 x 10^(-4) M/min 4 0.3 M 0.4 M 0.6 M 3.6 x 10^(-3) The method of initial rates is used to determine the rate law for reactants A, B, and C. This data was obtained at 25 degrees C....
The reaction 2A + 2B → M + N has the rate law: Rate = k[A]2. At 25°C, k = 0.0311 L mol-1 s-1. If the initial concentrations of A and B are 0.321 M and 0.499 M, respectively. What will be the concentrations of A and B after 30.0 minutes?
For this question, consider the reaction A-->B with a rate constant k=7.17x10^-4 m/s. A.)In one experiment, the half life for A is determined to be 15.00 minutes. What was the initial concentration of A? B.) In a different experiment, it takes 15.00 minutes for the concentration of A to decrease by 28%. What was the initial concentration of A in this trial? ate dete ate law for this rance of pros Name: TA Name: Student ID: Section number: Aneta 10For...
Given the following initial rate data, write the rate law expression. Experiment [A]o, M [B]o, M Initial rate, M/s 1 5.1 × 10-4 0.35 × 10-4 3.4 × 10-8 2 5.1 × 10-4 0.70 × 10-4 6.8 × 10-8 3 5.1 × 10-4 0.18 × 10-4 1.7 × 10-8 4 1.0 × 10-3 0.35 × 10-4 6.8 × 10-8 5 1.5 × 10-3 0.35 × 10-4 10.2 × 10-8 A. k [A] [B] B. k [A]2 [B]2 C. k [A]2...
2 ICl + H2----->I2 + 2 HCl Experiment [ICl]o, M [H2]o, M Initial Rate, M s-1 1 0.129 8.70×10-2 1.67×10-3 2 0.258 8.70×10-2 3.34×10-3 3 0.129 0.174 6.68×10-3 4 0.258 0.174 1.34×10-2 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = ____________ From these data,...