The progress of a reaction is tracked by following the concentration of one reactant as it is consumed. The table gives the concentration of that reactant at several times.Time (s)[R] (mol/L)5.00 × 10-34.32 × 10-33.66 × 10-33.03 × 10-32.44 x 10-³1.90 x 10-³1.39 × 10-3010.522.335.751.169.391.6120.4160.9230.3299.6-49.27 x 1075.26 x 10-41.99 x 10-47.54 x 10-5a Use graphing software to plot the data as [R] versus time, and determine the average rate for the first 15 s and the average rate from t = 100 to t = 125 s. Enter the rates as positivevalues.Rate (from t = 0 tot = 15 s) =Rate (from t = 100 to t = 125 s) =M/sM/sPreviousNext

To find the average rate of the reaction between the time mentioned in the question.Concept Average…

The progress of a reaction is tracked by following the concentration of one reactant as it is consumed. The table gives the concentration of that reactant at several times. Time (s) [R] (mol/L) 5.00 × 10-3 4.32 x 10-3 3.66 x 10-3 0 10.5 22.3 35.7 51.1 69.3 91.6 120.4 160.9 230.3 299.6 3.03 x 10-3 X 2.44 x 10-3 1.90 x 10-3 1.39 x 10-3 9.27 x 10-4 5.26 x 10-4 1.99 x 10-4 7.54 x 10-5 a Use graphing software to plot the data as [R] versus time, and determine the average rate for the first 15 s and the average rate from t = 100 to t= 125 s. Enter the rates as positive values. Rate (from t=0 to t= 15 s) = Rate (from t= 100 tot = 125 s) = M/s M/S Previous Next

The progress of a reaction is tracked by following the concentration of one reactant as it is consumed. The table gives the concentration of that reactant at several times. Time (s) [R] (mol/L) 5.00 × 10-3 4.32 x 10-3 3.66 x 10-3 0 10.5 22.3 35.7 51.1 69.3 91.6 120.4 160.9 230.3 299.6 3.03 x 10-3 X 2.44 x 10-3 1.90 x 10-3 1.39 x 10-3 9.27 x 10-4 5.26 x 10-4 1.99 x 10-4 7.54 x 10-5 a Use graphing software to plot the data as [R] versus time, and determine the average rate for the first 15 s and the average rate from t = 100 to t= 125 s. Enter the rates as positive values. Rate (from t=0 to t= 15 s) = Rate (from t= 100 tot = 125 s) = M/s M/S Previous Next

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

A flask is charged with 0.140 mol of A and allowed to react to form B according to the following hypothetical gas-phase reaction. A(g) → B(g) The following data are collected. Os 0 40 S 0.072 80 s 0.025 120 s 0.014 (a) Calculate the number of moles of B at each time in the table. 160 s 0.013 0 - 40 s 0.0018 40 - 80 s 0.000625 80 - 120 s 0.00035 120 - 160 mol/s 0.000325 times (s) mol mol x mol x mol moles of A X mol mol/s mol/s 0 (b) Calculate the average rate of disappearance of A for each 40 s interval, in units of mol/s. mol/s 40 mol/s 80 120 0.140 0.068 0.043 0.029 160 0.016
Which of these are factors that impact rate of reaction? temperature reactant concentration presence of a catalyst O reactant particle size
Restate the collision theory in your own words. Apply the concepts of collision theory to determine if the rate of reaction between zinc metal and hydrochloric acid will either increase or decrease under the following conditions: Decreasing the temperature of the hydrochloric acid Increasing the concentration of the hydrochloric acid Adding a catalyst to the reaction
Which of the following will lower the activation energy for a reaction? Group of answer choices raising the temperature of the reaction. increasing the concentrations of reactants. increasing the surface area of the reactants. adding a suitable catalyst.
Select all of the following that are required for a chemical reaction to occur according to the collision model: molecules must collide molecular collisions must be properly oriented to allow new bonds to form to create products molecular collisions must meet or exceed a minimal energy threshold (energy of activation) collisions of molecules of the same chemical species will not yield a chemical reaction
22. Based on the reaction rate data shown in Table 1, plot a properly labelled graph of Concentration vs. Time in the space provided. Draw a curve to connect the points. Table 1: Reaction rate Time (s) 0 1 2 3 4 5 6 7 8 9 10 Concentration (mol/L) 0 0.15 0.20 0.30 0.50 0.80 0.90 0.95 0.98 0.99 1.00 This curve should ascend over time. Conc vs 0.10 6.9 0.8 0.7 0.6 G.S 6.4 0.3 0.2 O. I • time 10 (mol/L) Concentration 4. Timeros 8 12 23. a) Based on the reaction rate data in Table 1, determine the average rate of chemical production between 2 s and 7 s. b) On the above graph, draw a line segment to represent the details in this question. Note: Show all calculations, follow the rules of significant figures, and box your final answer.
topic: molecular collision reactions A student reacts ground chalk, CaCO3(s), with HCl(aq) in an open beaker at room temperature. Explain, using collision theory, what happens to the rate of the reaction as the reaction proceeds to completion.
For the following reaction 5 experiments have been run and the data collected is in the following table: 4 HBr(g) + O2(g)--->2 Br2(g) + 2 H2O(g) Experiment [HBr], M [O2 ], M Rate, M/s (aka mol/L.s) 1 0.120 0.490 0.0267 2 0.142 0.120 0.00190 3 0.120 0.630 0.0442 4 0.230 0.630 0.0846 5 0.630 0.863 0.435 a)Write the rate expression. b) Calculate the rate constant, k c) If the concentration of HBr and O2 are 1.5 x 10-3 M and 3.25 x 10-3 respectively, what is the rate of the reaction?
3) Which of the following is NOT true about a catalyst? A.It may be homogeneous B. It speeds up the reverse reaction C. It is consumed D. It speeds up the forward reaction E. it may be heterogeneous
The following reaction occurs in your car's exhaust system catalytic converter:Heat + 2CO + O2 + Pt → 2CO2 + PtWhat is the catalyst?
The following represents the effect of time on the concentration during a reaction. The upper line represents a reactant concentration and the lower line the concentration of a product. Which of the following statements is not correct? Concentration B C Time → O Between points A and D the reactant concentration is decreasing. O Between points B and C the product concentration is increasing. At point D the rate of the forward and reverse reactions are the same. O At point C the rate of product breakdown equals that of reactant consumption.
For the reaction of A B, which of the following statements about the rates of forward and reverse reactions is true at time z? Concentraton vs time Time W X y Z The rate of forward reaction is greater. The rate of reverse reaction is greater. The rates of forward and reverse reactions are equal. The relative rates of reaction cannot be determined from the graph. Concentration [B] [A]