1. In the Rates of Chemical Reactions lab you measured the experimental rate of the followingreaction:S208 +212 +2 SO4²Given a graph of moles S₂Og 2 consumed versus time (s) with a best fit linear line and a totalvolume of 325 mL for the reaction, explain how would you determine the rate of reaction?2. The initial rates listed in the following table were determined for the reaction:H2PO3 (aq) + OH (aq) →HPO3²¯ (aq) + H2O (1)TrialInitial [H₂PO3¯], (M) Initial [OH], (M)Initial Rate of Consumption (M/s)10.0250.0300.43220.1000.0301.72830.1000.0150.864a) What is the rate law?b) What is the value of the rate constant, k?c) What is the initial rate when the initial concentrations of both reactants are 0.12 M?3. The following experimental data was obtained for the bromination of acetone at 30°C.21 +2 H+H2O2 → I2 + 2 H₂OTrialInitial [I] (M)Initial [H+]Initial [H2O2] (M)Rate (M/sec)(M)10.0010.0050.0012.0 x 10420.0020.0050.0014.0 x 10+30.0060.0020.0014.8 x 10+40.0060.0040.0019.6 x 10+50.0010.0010.0014.0 x 10-560.0010.0010.0024.0 x 10-5a) Determine the order with respect to each reactant.b) Determine the overall order of reaction.c) Write the rate law for the reaction.d) Find the value of the rate constant, k. 4. The tabulated data shows the concentration of AB versus time for the following reaction:AB A+BUsing the following data and graph paper. Complete the following questions below:Time, s[AB], M00.1001000.09712000.09443000.09174000.08905000.08656000.08407000.08168000.07939000.077010000.074811000.072712000.070613000.068614000.066615000.0647a. Determine the order for the following reaction.b. Determine the rate constant, k.

"Since you have asked multiple questions, as per the answering guidelines, we will answer the first…

1. In the Rates of Chemical Reactions lab you measured the experimental rate of the following reaction: S208 +212 +2 SO4 Given a graph of moles S₂Og 2- consumed versus time (s) with a best fit linear line and a total volume of 325 mL for the reaction, explain how would you determine the rate of reaction?

1. In the Rates of Chemical Reactions lab you measured the experimental rate of the following reaction: S208 +212 +2 SO4 Given a graph of moles S₂Og 2- consumed versus time (s) with a best fit linear line and a total volume of 325 mL for the reaction, explain how would you determine the rate of reaction?

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

Time, s C3H8], M 0.0 0.26 10.0 0.18 20.0 0.14 30.0 0.10 . 40.0 0.064 .50.0 0.052 M
Question 23 The rate law for a reaction is determined to be rate=k[AJIB}*[C]. If the reaction has an overall order of 9, what is the value of exponent for B? (the answer should be entered as a single digit number; do not enter units; examples include 0 and 1 and 2 and 3 and etc.) K Questa A Moving to another question will save this response. B88 . 43C & %23 4 5 6. 8 3 I o P Q E R T Y tab A S F G K caps lock V B alt alt control option command command option
Consider the reaction in aqueous solution: 3r+ S20g? - 15 + 2 so,2 Under a given set of conditions, the concentration of 13 changes from 0.0 M to 9.3 10 Min 30 seconds Calculate A(SOyat (in molil-s) for this time interval O 97 104 moUL s O 93- 105 molLs O 8.6 10-5 mol/L s O 97x10 mol/L s O 62- 104 molL s
(Can I get the answer in not more than 45 mins please? or asap. Thank you!)
The data below were collected for the following reaction: CH3CI(g) + 3 Cl2(g) CCI4(g) + 3 HCI(g) [CH3CI] / mol L-1 Initial Rate / mol L-1 s-1 Trial [Cl2] / mol L-1 1 0.050 0.050 0.0142 2 0.100 0.050 0.0290 3 0.200 0.200 0.115 What is the order of the reaction with respect to Cl2?
1. At elevated temperatures, nitrous oxide decomposes according to the equation2N2O(g)⟶2N2(g)+O2(g) Time (min) 0 60 90 300 600 [N2O] 0.250 0.228 0.216 0.128 0.0630 Given the following data, determine whether the reaction is zeroth, first, or second order. a) first b) second c) zeroth
The data for the reaction given NOCI (g) The following experimental data was measured for the reaction. Use the Method of Initial Rates to determine the rate law equation for this reaction 1 2 3 NO (g) + 1/2 Cl2₂ (g) [NO] [Cl₂] Initial Rate Experiment (mol.L-¹) (mol.L-¹) (mol.L-¹ s¯¹) 1.4x10-6 2.8x10-6 5.6x10-6 0.250 0.250 0.500 0.250 0.500 0.250 → 1. Determine the order of the reaction with respect to NO oxide 2. Determine the order of the reaction with respect to Cl₂ 3. What is the overall order of this reaction? 5. Calculate the value of the rate constant, k → 4. Select the correct rate law (rate equation) for this reaction: Rate =
How would you find the rate law for this question?
Chem q 5
I need help with all parts please
60 QUESTION 13 The following graphs can be used for the questions that follow: 00 B0 00 Seris 1 02 time(min) D2 -D4 y = -0.0358x + 0.1058 Liner (Serive t) -18 time(min) The decomposition reaction of NO 2 is important in atmospheric chemistry. The reaction 2NO 2(g) → 2NO(g) + O 2(g) is second order with respect to NO 2. How can the rate constant be determined? A plot of 1/[NO2] versus time will be linear with a slope of -k. A plot of 1/[NO2] versus time will be linear with a slope of k. A plot of [NO2] versus time will be linear with a slope of -k. A plot of In[NO2] versus time will be linear with a slope of -k. Click Save and Submit to save and submit. Click Save All Answers to save all answers. MacBook Air DD F8 F3 F4 F5 F1 %23 24 2 4. 7.
[A] vs Time In[A] vs Time O 1/[A] vs Time Least Squares Plot The reaction A → C was performed and the concentration vs. time data below collected. time, s [A], mol/L 0.7983 0.1898 0.1077 0.07517 0.05774 0.04687 0.03944 0.03405 0.02995 [A] 0 reaction order = Check Submit Answer 1 Time, s 2 3 Try Another Version Complete the rate law for the reaction by filling in the values for the rate constant and reaction order. Rate = K[A]* rate constant (without units) = Next> (1 of 1) Show Approach 2 item att 5 6 Hide Hint 7 8 A least squares line gives the best straight- line fit through any set of points but to get the right answer you need to figure out which plot gives the straight line.