Nitric acid is a key industrial ch A ALEKS - Ciapha Dorley Learn A www-awn.aleks.com/alekscgi/x/Isl.exe/lo_u-IgNsIkr7j8P3jH-IQs_dp5pR4E P Course Home Login | Student Veri... E- Connect Apps M SIMnet Assignme... O KINETICS AND EQUILIBRIUM Using a rate law The rate of a certain reaction is given by the following rate law: *[H,][L] rate= k Use this information to answer the questions below. What is the reaction order in H,? What is the reaction orderin 1,? What is overall reaction order? At a certain concentration of H, and I,, the initial rate of reaction is 97.0 M/s. What would the initial rate of the reaction be if the concentration of H, were doubled? Be sure your answer has the correct number of significant digits. The rate of the reaction is measured to be 7.0 x 10-M/s when (H2] = 0.94 M and [I,] = 0.88 M. Calculate the value of the rate constant. Be sure your answer has the correct Inumber of significant digits,

Nitric acid is a key industrial ch A ALEKS - Ciapha Dorley Learn A www-awn.aleks.com/alekscgi/x/Isl.exe/lo_u-IgNsIkr7j8P3jH-IQs_dp5pR4E P Course Home Login | Student Veri... E- Connect Apps M SIMnet Assignme... O KINETICS AND EQUILIBRIUM Using a rate law The rate of a certain reaction is given by the following rate law: *[H,][L] rate= k Use this information to answer the questions below. What is the reaction order in H,? What is the reaction orderin 1,? What is overall reaction order? At a certain concentration of H, and I,, the initial rate of reaction is 97.0 M/s. What would the initial rate of the reaction be if the concentration of H, were doubled? Be sure your answer has the correct number of significant digits. The rate of the reaction is measured to be 7.0 x 10-M/s when (H2] = 0.94 M and [I,] = 0.88 M. Calculate the value of the rate constant. Be sure your answer has the correct Inumber of significant digits,

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...

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Consider the following 2-step reaction mechanism, consisting of elementary steps: k1 2 XO2g) k-1 Step 1: X2O4(g) k2 Step 2: X2O4(g) + Br2७) Br2(g) + 2 XO2Br(g) a) Complete the following (if none exist, write 'none'). The reaction intermediate(s) is/are... i) The reaction catalysts(s) is/are.. b) Without assuming the relative reaction rates of Step 1 or Step 2, determine the rate law that is predicted by this mechanism. If Step 2 is a fast reaction (and Step 1 was a slow equilibrium), determine the overall reaction order.
tab lock atrol D esc Question 14 Based on the initial-rate data below, which is the magnitude (units omitted) for the specific-rate constant for this reaction? Rate (M/s) 1.3 x 10-7 5.2 x 10-7 1.0 x 10-6 [HgCl2] (M) [C2042-] (M) 0.10 0.10 0.10 0.20 0.20 0.20 O 5.2 x 10-6 O 1.3 x 104 O 1.3 x 10-5 O 2.0 x 10-7 Question 15 ! An chemical reaction has specific-rate constant 1.10 x 104 s¹ at 470 C. How many hours are required for a 0.335 M solution to decrea to 0.051 M? 1 O A B Ā N @ 2 W S X 2 option command w # E D DS 4 C R TI % 5 V 2 T G > A 6 MacBook Pro CO B Y 4) & 7 H U N 00 8 J - M ( 9 K O ) O < H 5 L P command
average cycle time with the doubled KBrO3 concentration is 40 and average cycle time with initial KBrO3 concentration is 74.
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C blackboard.sc.edu Content Blackboard Lea... > Recitation W3... J Late Model Ca... rate = k[N₂01² Question 3 Worksheet 13.6 #2 X Consider the two-step mechanism below that has been proposed for the reaction of nitrous oxide to form nitrogen and oxygen gas to answer the following questi Step 1: N₂0 (g) → N2 (9) + O (g) (slow) (fast) Step 2: N₂O(g) + O (g) → N2 (g) + O2 (9) Net: 2 N₂O (g) → 2 N2 (9) + O2 (9) Part B: Based on the proposed rate law for the net overall reaction, what is the overall order of the reaction? Selected Answer: 1/2 order Worksheet 13.6 #2 Consider the two-step mechanism below that has been proposed for the reaction of nitrous oxide to form nitrogen and oxygen gas to answer the following questi Step 1: N₂O (g) → N₂ (g) + O (9) (slow) (fast) Step 2: N₂O(g) + O (g) → N₂ (9) + 02 (9) Net: 2 N₂0 (g) → 2 N2 (9) + 02 (9) Part C: What intermediates/catalysts are present in this mechanism? Selected Answer: N₂O is a catalyst; there are no intermediates Wednesday, April 6,…
By using collision theory calculate the activation energy of a reaction having two reactants A and B and the product is C. The value of the universal rate constant is 8.314J/mol*K.When the reaction is happening at different temperatures 350K and 700K , the ratio of rate constant is 5. (Gpt/ai wrong answer not allowed)
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General Chemistry II- Ara Sinavi 13 According to the data given below calculate k and t1/2. For the hypothetical aqueous reaction: A B, the concentration change of A was monitored and several derived data were tabulated and two different plots were obtained. Based on these given plots and data: time(min) [A] (M) In[A] V [A] -0.2 0.65 -0.43 1.5 --0.4 10 0.51 -0.67 2.0 -0.6 S -0.8 20 0.42 -0.87 2.4 -1.0 30 0.36 -1.02 2.8 Карat
Captain Marvelibrium discovered a figure with data frorh an experiment left by Le Châtelier Flipdime. Consider the following data where A andB are mixed at initial concentrations indicated. Upon reacting the concentrations change a can be read from the plot. The reaction is A(g) + B(g) = C(g). C Time (s) Based on figure, calculate the value for Ke for the reaction. Submit Answer Tries 0/99 This discussion is closed. Send Feedback MAR 10 étv МacВос Air 000 esc F1 F2 F3 F4 F5 F6 #3 $4 3. 4 CO AB 3. Concentration (mol.dm-3)
t- Assignme... Connect P Course Home E Login | Student Veri... Bb Logout MyProgrammingLab Im O KINETICS AND EQUILIBRIUM Deducing a rate law from initial reaction rate data Some measurements of the initial rate of a certain reaction are given in the table below. [-] [H.] , initial rate of reaction 1.75 M 0.767 M 16.0 M/s 7.77 M 0.767 M 71.0 M/ s 1.75 M 0.136 M 2.84 M/ s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k D k = ]
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