2. Consider the following reaction: Time b) What is the rate law? 0 1000 2000 3000 4000 5000 A B [A] (M) 0.475 0.350 0.277 0.230 0.196 0.171 a) Determine the order of the reaction by graphing the data appropriately. You may create graphs by hand using the graph paper provided or by using Excel or Google Sheets (be sure to include an image of your graph). Explain your answer. c) What is the rate constant? Provide appropriate units.

2. Consider the following reaction: Time b) What is the rate law? 0 1000 2000 3000 4000 5000 A B [A] (M) 0.475 0.350 0.277 0.230 0.196 0.171 a) Determine the order of the reaction by graphing the data appropriately. You may create graphs by hand using the graph paper provided or by using Excel or Google Sheets (be sure to include an image of your graph). Explain your answer. c) What is the rate constant? Provide appropriate units.

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

[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
7. The rate of the reaction NO,(g) + CO(g) → NO(g) + CO,(g) depends only on the concentration of nitrogen dioxide below 225°C. At a temperature below 225°C, the following data were collected: Time (s) [NO,] (mol/L) 0.500 1.20 X 103 3.00 X 103 0.444 0.381 4.50 X 103 0.340 9.00 X 103 0.250 1.80 X 104 0.174 Determine the rate law, the integrated rate law, and the value of the rate constant. Calculate [NO2] at 2.70 × 10* s after the start of the reaction.
For the reaction A → products, concentration and time data were collected. t (s) [A] (M) Enter these data into the graphing tool to determine the reaction order. 0.0 0.900 25.0 0.609 50.0 0.461 75.0 0.370 Graphing Tool Clear All Data [A] vs. t In[A] vs. t 1/[A] vs. t [A] In[A] 1/[A] Add Row 10 total rows What is the reaction order? 1 Calculate the concentration of A after 127 s. 1/[A]
The rate of the reaction NO2+ CO - NO + CO2 depends only on the concentration of nitrogen dioxide, NO2. The following data were collected. time (s) [NO] (M) 0.500 1.20 x 10 0.444 3.00 x 10 0.381 4.50 x 10 0.340 9.00 x 10 0.257 1.80 x 10 0.174 When entering values in scientific notation follow this format: 6.022 x 1023 would be 6.022e23 (no spaces) 1. Using graphical analysis (Google Sheet et) determine the overall reaction order. (0.1.2) Be sure to upload a screenshot copy of the the Google sheet for question 2 in the next question box. 2 Determine the value of the rate constant for the reaction (do not round answer). 3. Calculate the [NO2l, at 2:40 x 10 s. (show answer to 3 places after the decimal) 182 4. Determine the t, for the reaction. (round answer to the whole number)
Given the following rate and concentration data, determine the rate law for the reaction A + B ---> products [A]0 (M) [B]0 (M) initial rate (M/s) 0.10 0.10 4.22 X 10^-6 0.20 0.10 8.44 X 10^-6 0.20 0.40 3.38 X 10^-6 the rate constant k= rate=
Consider the following reaction: Cl2O (g) + CO (g) → Cl2 (g) + CO2 (g) Initial rate of the reaction was measured at multiple different concentrations of CO, which created the following data: [CO] (M) Initial Rate (M/s) 0.10 0.0020 0.20 0.0040 0.40 0.0080 From this data, we can see that the reaction order with respect to CO is __________. Consider the following reaction: Cl2O (g) + CO (g) → Cl2 (g) + CO2 (g) Initial rate of the reaction was measured at multiple different concentrations of CO, which created the following data: From this data, we can see that the reaction order with respect to CO is __________. a. 1st Order b. 3rd Order c. 2nd Order d. 0th Order
Consider this reaction: A + B → C + D Expt. [A] (M) [B] (M) Initial Rate (M/s) 1 0.100 0.100 0.152 2 0.100 0.200 0.152 3 0.200 0.200 0.305 What is the overall reaction order for this reaction?
Consider this reaction: 2HI (g) → H₂ (g) + 1₂ (g) At a certain temperature it obeys this rate law. rate = (0.00315 M¹-s¯¹) [HI] ² S olo Suppose a vessel contains HI at a concentration of 1.16M. Calculate the concentration of HI in the vessel 970. seconds later. You may assume no other reaction is important. Ar Round your answer to 2 significant digits. M x10 X Ś ?
The following initial rate data was obtained for the reaction between oxygen and nitric oxide. 2 NO(g) + O₂(g) → 2 NO2(g) [0₂] (M) [NO] (M) Rate (M s-¹) 0.0100 0.0150 0.0150 0.0100 0.0100 0.0200 10.0 22.5 45.0 J What is the rate law for this reaction under these conditions? Rate = k [0₂]2 [NO]² Rate = k [0₂] [NO]² Rate = k [0₂]²2 [NO] Rate = k [0₂] [NO] G
At a certain temperature the rate of this reaction is second order in SO, with a rate constant of 4.02 M 's': 2S0, (g) → 2S0, (g) +0,(g) Suppose a vessel contains SO , at a concentration of 0.790 M. Calculate how long it takes for the concentration of SO, to decrease to 0.103 M. You may assume no other reaction is important. Round your answer to 2 significant digits.
Consider the initial-rate data at a certain temperature in the table for the reaction described by 2 NO, (g) + 0, (g) N,0,(g) + 0,(g) [NO2], (M) [03]o (M) Initial rate (M 0.650 0.800 3.25 x 10 1.10 0.800 5.50 x 10* 1.76 1.40 15.40 x 10 Determine the value and units of the rate constant, k. k = Units;
Very confused with this rate law