From an experiment, it had been determined that the hypothetical reaction A + 2B → 2C +D follows the rate law dA := K[AF [B} dt Three new experiments were performed by keeping the concentration [B] = 0.10 M constant. The new experiment led to the following data Experiment Concentration [A] -d[A]/dt (mol/s) 1 0.05 6.02 × 10-3 2 0.1 1.20 x 10-2 3 0.2 2.41 × 10-2 Determine the order of this reaction and calculate the reaction rate constant.

From an experiment, it had been determined that the hypothetical reaction A + 2B → 2C +D follows the rate law dA := K[AF [B} dt Three new experiments were performed by keeping the concentration [B] = 0.10 M constant. The new experiment led to the following data Experiment Concentration [A] -d[A]/dt (mol/s) 1 0.05 6.02 × 10-3 2 0.1 1.20 x 10-2 3 0.2 2.41 × 10-2 Determine the order of this reaction and calculate the reaction rate constant.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Give handwritten answer of all parts
Part B Constanta, @gic US UIC Taic an O IncicacUGHT. rate = If the rate constant for this reaction at 1000 K is 6.0 x 104 M-²s¹, what is the reaction rate when [NO] 2.30×10-2 M and [H₂] = 1.30×10-2 M? Express your answer using two significant figures. 10 ΑΣΦ L Xª Xb a √x Vx rate= [H₂] [NO]² f t C IXI 0 ? X-10" 8 M/s
Using the data in the table, determine the rate constant of the following reaction and select the appropriate units. A+B → C + D Trial rate= I 2 3 [A] (M) 0.250 0.250 0.450 Step 2: What is the rate law in terms of k, [A], and [B]? [B] (M) 0.200 0.520 0.200 Rate (M/s) 0.0138 0.0933 0.0248
Analyze the following set of data and determine: An expression for the rate law for the reaction • A value for the rate constant with appropriate units The reaction in question is: 2A + B + 2C 1 23 EXPERIMENT INITIAL [A] (mol/L) 0.20 0.20 0.20 0.60 4 -> INITIAL [B] (mol/L) 0.10 0.30 0.10 0.30 3D INITIAL INITIAL [C] RATE (mol/L) (mol/L's) 0.10 4.0 X10-4 0.20 1.2 X 109 0.30 4.0 X 10 -4 0.40 3.6 X 10°
Consider the reaction described by the equation С,Н, Br, (aq) + 31 (аq) — C,H,(g) + 2 Br¯(aq) + I, (aq) 4 The rate law is rate = k[C,H,Br, ][I¯] where k = 0.00483 M-1. s-1. What are the missing entries in the table? Run [C,H,Br, lo (M) | [I¯]o (M) Initial rate of formation of C,H, (M-s ) 4 1 0.299 0.00173 2 0.299 y 0.000864 3 0.299 0.299
3. An experiment was carried out to determine the rate law for the following reaction: 19152 2NO( )+0( ) → 2NO( ) Where the rate law is: par Rate = k[NO] [0] The experiment was repeated three times and the following data recorded: Experiment # Initial [NO] (M) Initial [0] (M) Rate (M/s) 1 ullo2 M0.015 0.015 2 0.030 0.015 3 0.015 0.030 of in Determine the value of x in the rate law (order of reaction with respect to NO) by comparing experiments 1 and 2 in Equation 13 reaction with respect to O₂) by comparing experiments 1 and 3 in equation 13. 0.048 0.192 0.096
Using the data in the table, determine the rate constant of the Trial [A] (M) | [B] (M) | Rate (M/s) reaction and select the appropriate units. 0.250 0.260 0.0234 A + 2B → C + D 0.250 0.520 0.0234 3 0.500 0.260 0.0936 Units k = M.s-1 M-²s¬1 M-ls-1
6
Consider the reaction 5Br (aq) + BrO, (aq) + 6H+ (aq)→3B12 (aq) + 3H20(1) The average rate of consumption of Br is 1.36x104 M/s over the first two minutes. What is the average rate of formation of Br2 during the same time interval? Express your answer with the appropriate units. • View Available Hint(s) HẢ |] ? Rate of formation of Br2 Value Units %3D
A+ B+ 2C - 2D+ 3E where the rate law is A[A] k[A][B]* Rate = - %3D At An experiment is carried out where [A], = 1.0 x 10-2 M, [B, = 6.0 M, and [C, = 2.0 M. The reaction is started, and after 8.0 seconds, the concentration of A is 3.8 x 10-3 M. a. Calculate the value of k for this reaction. k%3= L mols 1 b. Calculate the half-life for this experiment. Half-life = c. Calculate the concentration of A after 17.0 seconds. Concentration= M d. Calculate the concentration of C after 17 seconds. Concentration=