A student collected pressure measurements at 298 K over 120 seconds and plotted the data as the following reaction occured: 2H2O2(aq) → 2H2O(g) + O2(g) The slope of the best-fit line was determined to be 1.231 torr/s. What is the rate of the reaction (M/s)? A. 2.57 x 103 M/s B. 0.08206 M/s С. 1.231 M/s D. 6.62 x 10-5 M/s

A student collected pressure measurements at 298 K over 120 seconds and plotted the data as the following reaction occured: 2H2O2(aq) → 2H2O(g) + O2(g) The slope of the best-fit line was determined to be 1.231 torr/s. What is the rate of the reaction (M/s)? A. 2.57 x 103 M/s B. 0.08206 M/s С. 1.231 M/s D. 6.62 x 10-5 M/s

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

Here is the following reaction at 25.0 °C Hg(OH)2 (aq) + CaCl2 (aq) →2HgCl (s) + Ca(OH)2 (aq) experiment [Hg(OH)2] (M) [CaCl2] (M) Initial rate (M/s) 1 0.022 0.0022 5.0 ×10-4 2 0.085 0.0022 7.5 ×10-3 3 0.022 0.50 5.0×10-4 Determine the overall order of the reaction.
The data given in the table below is for the following reaction (run at 25°C): 2 NO + O, 2(g) → 2 (g) 2(g) Initial Concentration (M) Initial rate Experiment NO 0, Mol/(L · s) 1 0.0010 0.0010 7 x 10-6 2 0.0010 0.0020 14 x 106 3 0.0010 0.0030 21 x 10-6 4 0.0020 0.0030 84 x 10-6 5 0.0030 0.0030 189 x 106 1. Determine the orders of the reaction with respect to NO and O, (show all work): NO
[References] The reaction I (ag) + OCI (aq) → IO¯(aq) + Cl¯(aq) was studied, and the following data were obtained: I], (mol/L) [OCI"], (mol/L) Initial Rate (mol/L · s) 0.12 0.16 7.80 x 10-2 0.060 0.16 3.90 x 10-2 0.030 0.080 9.80 x 10-3 0.24 0.080 7.80 x 10- What is the rate law? (Use k for the rate constant.) Rate Calculate the value of the rate constant. k = L/mol · s Calculate the initial rate for an experiment where both I and OcI are initially present at 0.16 mol/L. Rate = mol/L · s
Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of ·0.0040Ms−1:2HI(g)→H2(g)+I2(g) Suppose a 300.mL ⁢ flask is charged under these conditions with 500.mmol of hydrogen iodide. After how much time is there only 250.mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.
The following data were obtained for the gas-phase decomposition of dinitrogen pentoxide,
A reaction between substances A and B has been found to give the following data: 3A +2B 2C+D Al (mol/L) (mol/Rate of appearance of C 10 x 102 10 x 102 30 2.0 x 102 30 mol / L-hr) 0.300 x 100 810x 10 3 24 x 10-5 1.20 x 10-8 30 x 10-5 10 0 x 102 1.0 3.0 x 10- Using the above data, determine: a) the order of the reaction with respect to A and B - b) the rate law, and - c) calculate the specific rate constant
I need help with this problem. I don't know how to start it.
The reaction rate of CO and NO2 in the reaction CO(g) + NO2(g) → CO2(g) + NO(g) is measured using the initial rates method. The results are tabulated below. [CO] (mol/L) NO2 (mol/L) -([CO]/Δt (mol/L·s) 8.00 10-4 5.50 10-4 8.40 10-8 8.00 10-4 7.78 10-4 1.68 10-7 1.60 10-3 5.50 10-4 1.68 10-7 Determine the rate expression and calculate the rate constant for the reaction.
mm
The following data was collected over four different experiments. for this reaction: aA + bB → CC Experiment [A] M [B] M 1 0.200 0.200 2 0.200 0.400 3 0.400 0.200 4 0.300 0.100 The initial rate of the first reaction was 0.650 mol/L min. The second reaction was 2 times that rate, the third reaction was 8 times the rate of the first reaction, and the fourth reaction was 1.7 times the rate of the first reaction. Determine the value for the constant k. Your Answer: 2031.25
7. A study of the hypothetical reaction 2A + B C+D gave these results: Initial Rate (emol Ls) Initial Concentration (mal/) Experiment 181 1. 0.10 0.050 6.0 x 10 2. 0.20 0.050 1.2 x 10 3 0.30 0.050 1.8 x 10 2 4. 0.20 0.150 1.1 x 10-1 a) What is the rate law for this reaction? b) Calculate the rate constant k and express it in appropriate units.
Consider the following reaction mechanism: Step 1: A3(g) → A2(g) + A(g) Step 2: A3(g) + A(g) → 2A2(g) What is the role of A(g) and what is the overall balanced equation? Periodic Table and Datasheet O A(g) is an intermediate; 2A3(g) + A(g) → 3A2(g) + A(g) O A(g) is a catalyst; 2A3(g) + A(g)→ 3A2(g) + A(g) O A(g) is an intermediate; 2A3(g) –→3A2(g) O A(g) is a catalyst; 2A3(g) → 3A2(g)