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) Consider the following reaction and data: ??(?) + ??(?) ⟶ ?(?)
Determine the rate law for this reaction
Calculate the rate constant
![Experiment #
[A] (mol L)
[B] (mol L1)
Initial Rate (mol L1 s)
1
0.033
0.033
4.44 x 105
2
0.033
0.066
8.89 x 10-5
3
0.066
0.033
1.78 x 10-4](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa3f7f1ae-6435-43dd-a988-21c9df34ccce%2F853ba82a-86a7-4617-a4bc-b7e1a48ff28a%2Ftnv97zg_processed.png&w=3840&q=75)
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- In(a。-x) Slope=-0.0527 Intercept= -4.20 Calculate the initial concentration of the reactant O 0.15 M O Cannot be determined O 0.53 M O 0.24 M 0.42 M timeCalculation Tables Table 4- Logarithms [l]o (M) -log[I]o -log(rate) [H2O2]o (M) 0.0100 -log[H2O2]o 2.00 Experiment # Rate (M/s) 1 2.63 x10-6 5.58 0.0200 1.70 5.18 x 106 0.0100 0.0400 0.0600 8.01 x 10-6 1.62 x 105 0.0100 4 0.0200 0.0600 3.21 x 105 0.0400 0.0600 Table 5- Rate Constants Experiment [H2OzJo(M) [H2O2]om Initial rate k # (M/s) 2.63 x10-6 1 0.0100 0.0200 2 0.0100 0.0400 5.18 x 10-6 0.0100 0.0600 8.01 x 106 4 0.0200 0.0600 1.62 x 105 5 0.0400 0.0600 3.21 x 105 Value of m (2 significant figures): Value of n (2 significant figures): verage value of k (3 significant figures):Match the rates to the correct expression.
- A+B+CD Exp. Initial A (mol/dm³) Initial B (mol/dm³) Init. Rate of Formation of D (mol/dm³ min-¹) 1 0.10 0.10 3.0 x 10-4 2 0.30 0.30 9.0 x 10-4 3 0.10 0.30 3.0 x 10-4 4 0.20 0.40 6.0 x 10-4 5 0.10 0.10 1.2 x 10-3 The student concluded that the rate equation should be: rate = K[A] [B][C]² ii) Using the data for experiment 4, calculate the value of the rate constant, k, using the correct rate equation, making sure that you include the correct units. Initial C (mol/dm³) 0.10 0.10 0.10 0.10 0.20What is the rate? lodine chloride reacts with hydrogen to produce iodine and hydrogen chloride. 2ICI + H2 --> 2HCI Trial ICI(mol/L) H2(mol/L) Initial rate mol/Ls 5.84 x 107 0.0015 8.76 x 10-7 0.0030 1.17 x 106 0.0060 0.20 2. .0.40 0.20 Include UnitsBe sure to answer all parts. For the following general reaction, rate -AJAJ and k-1.3 x 102 M.s. A+B 2C Use this information to fill in the missing table entries. Experiment JA] (M) BỊ (M) Initial rate (Mis) 1 0.013 0.250 2.20 x 10 2 0.026 0.250 3 0.500 2.20 x 10 1) Initial reaction rate in experiment 2: <10 M/s (Enter your answer in scientific notation.) 2) Initial concentration of A in experiment 3:
- 2. Compare the value you calculated with the actual value (-601.8 kJ/mol). Show your determination of percent error. Use the standard equation for this: actual value - experimental value %error = x 100% |actual value| ragraph* and which the & 3 4 7 81. Using the experimental data below: NO2(g) + SO2(g) → 1 2 3 NO(g) + SO3(g) Trial # Initial Initial Initial Rate [SO₂] [NO₂] (mol L-¹¹) 0.246 0.004 9.38 x 10-2 0.246 0.012 9.38 x 10-² 0.492 0.012 3.752 x 10-¹ a. Determine the rate law including the rate constant and exponents for each reactant b. What is the overall order of this reaction?flask is charged with 0.100 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. times (s) 0 40 80 120 160 moles of A 0.100 0.065 0.042 0.030 0.023 (a) Calculate the number of moles of B at each time in the table. 0 s mol 40 s mol 80 s mol 120 s mol 160 s mol (b) Calculate the average rate of disappearance of A for each 40 s interval, in units of mol/s. 0-40 s mol/s 40 - 80 s mol/s 80 - 120 s mol/s 120 - 160 mol/s mol/s
- ew K History Bookmarks DZL Rate Laws Expe X Profiles Tab Determination c X 1 Homework 2 ttempt 1 Listen Window my.edu/d21/le/content/408344/viewContent/17004406/View Help Your Answer: Rates Law Expe X D21 4. CLASS SLIDE X 3 What is the rate constant for a reaction based on the following experimental information? Expt Rate (M/s) [A] (mol/L) [B] (mol/L) 1 0.5170 0.700 0.648 2 1.4912 1.189 0.648 1.2205 1.529 D21 Activity Assignr X 0.700 Report your answer to THREE significant figures. A ALEKS-Isabell x ETrial [A] (M) [B] (M) Rate (M/s) 1 0.10 0.20 5.777 2 0.45 0.20 0.6052 3 0.10 0.37 19.77 A) Determine the exponent in the rate law for reactant B using the data above B) Determine the exponent in the rate law for reactant A. C) Determine the UNITS on k (i.e., NOT the numeric value – just the units). D) Determine the numeric value of the rate constant and write it in the top box. Then right the FULL rate law equation in the bottom box.I-(aq) + OCI-(aq) 10-(aq) + Cl-(aq) The above reaction was studied (at a particular temperature) and the following data were obtained: [1-10 [OCI-]0 Initial Rate (mol/L) (mol/L) (mol L-1s-1) 0.360 0.100 8.42\times 10-20.045 0.100 1.05\times 10-20.090 0.200 4.21\times 10-20.180 0.200 8.42\times 10-2 Which of the following expressions for the rate law are completely consistent with the above experimental data, d[Cl-]/dt = kl OCI-][-] d[10-]/dt = k[OCI-]3 k[OCI][I] = d[OCI-]/dt-d[-]/dt = k[-]2[OC]d[1]/dt = k[-][OC] 1 pts Tries 0/5 Calculate the rate constant (k). (Units required.)