[References]Use the References to access important values if needed for this question.The following initial rate data are for the reaction of UO, with hydrogen ion in aqueous solution:4+2 UO, + 4 H-U* +U0,2* + 2 H20Experiment[UO,], M[H*],, MInitial Rate, M s14.15x1030.3449.66×104218.30x10-30.3443.86x1034.15x1030.6881.93x103148.30x1030.6887.73x103Complete the rate law for this reaction in the box below.Use the form k[A]" B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n.Rate =From these data, the rate constant isM21Submit AnswerTry Another Version10 item attempts remainingPreviousNext63°F RainingDELL3.

From given Rate law and Rate constant have been solved below

[References] Use the References to access important values if needed for this question. The following initial rate data are for the reaction of UO, with hydrogen ion in aqueous solution: 2 UO, +4 H*-u* + UO,2+ +2 H,0 Experiment [UO,1, M [H'], M Initial Rate, M s 4.15x103 S.30x103 4.15x103 0.344 9.66x104 0.344 3.86x10-3 3 0.688 1.93x103 S.30x10-3 0.688 7.73x10-3 Complete the rate law for this reaction in the box below. Use the form kJA]" B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is

[References] Use the References to access important values if needed for this question. The following initial rate data are for the reaction of UO, with hydrogen ion in aqueous solution: 2 UO, +4 H-u + UO,2+ +2 H,0 Experiment [UO,1, M [H'], M Initial Rate, M s 4.15x103 S.30x103 4.15x103 0.344 9.66x104 0.344 3.86x10-3 3 0.688 1.93x103 S.30x10-3 0.688 7.73x10-3 Complete the rate law for this reaction in the box below. Use the form kJA]" B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is

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

The following initial rate data are for the reaction of ICI with hydrogen: 2 ICI + Hz I, + 2 HCI Experiment [ICI], M [Ha]o, M Initial Rate, M s-1 1.58×10-2 3.16x10-2 6.29x10-2 0.126 1 0.254 0.188 2 0.508 0.188 3 l0.254 0.375 4 0.508 0.375 Complete the rate law for this reaction in the box below, Use the form k[A]"[B]", where '1' is understood for m orn and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is
X Cut AaBbCcl AaBbCcDc AaBbCcD AaBbCcE AaB AaBb CcC Aa8be T No Spac. Heading 2 Calibri (Body) | AA Aa. E , 刻T Copy Paste Subtle Title Subtitle BIU abc x, x A - y- A- Heading 1 T Normal Format Painter Paragraph Styles Font Clipboard I 10 11 6. From the data variation of the reaction rate of the following temperatures: 1500 T (K) k (M1 second ) 500 1000 5,49 x 106 9,86 x 108 5,09 x 10° Specify: a. Amount of Activation Energy (Ea) b. Magnitude of the pre-exponential factor (A)
ess important values if needed for this question. For the decomposition of hydrogen lodide on a gold surface at 150 °C 2 HI(g) → H₂(g)+ 12 (9) the average rate of disappearance of HI over the time period from t=0s to t=2610s is found to be 1.20 x 10 M-s¹. The average rate of formation of I₂ over the same time period is M-s Submit Answer Retry Entire Group 9 more group attempts remaining
A + 2B C + 2D ->> In another experiment at 25 °C, the rate of formation of C is 3.0 x 10-4 M/sec when 0.30 moles of B is reacted with an unknown quantity of A. Rate = 0.0067 M-2S-¹ [A][B]² How many moles of A are reacted in this trial? moles A = [?] Do not include units in your answer. Moles of A Enter
4. The following data were obtained for the follwing chemical reaction: 2A + 3B ---> 2C + D Initial [A] Initial [B] Initial Rate of Formation Trial # (mmol/L) (mmol/L) of D (mmol/L*s) 1 4.0 6.0 1.60 2 2.0 6.0 0.80 3 4.0 3.0 0.40 (a) Determine the rate law equation for this reaction. Show your reasoning. (b) Find the rate constant, k, with units.
The reaction 2 N205(g) → 4 NO2(g) + O2(g) was studied and the rate of change of the concentration of O2 was found to be 3.65 mol L 15-1. Calculate the reaction rate (in mol L1s1). Reaction rate = i mol L-1s-1. eTextbook and Media Save for Later Attempts: 0 of 3 used Submit Answer
T[C] K [ cm³/mol-s] The rxn is a decomposition reaction of HI. 2HI → H₂ + 1₂ In this rxn, the ff data were gathered. 508 1.059x10-1 427 3.1x10-3 393 5.88x10-4 356 8.09x10-5 Solve for the complete rate eq. for this reaction [ i.e. r = f(T) f(C) ] 283 9.42x10-7
6. The oxidation of Br¯ by Br03 in acidic solution (H*) is described by the equation 5 Br (aq) + Br03 (aq) + 6 H* (aq) З Вrz (aq) + 3 H,0() Initial [Br ] (M) Initial [BrO3] (M) Initial [H*] (M) Initial Reaction Rate (M/s) 4.2 x 10-3 8.4 x 10-3 1.055 x 10-3 4.2 x 10-3 Experiment 1 0.404 0.250 0.100 2 0.808 0.250 0.100 3 0.404 0.125 0.250 0.100 4 0.404 0.050 (a) What is the reaction order with respect to each reactant? (b) Write the rate law. (e) What are the units of the rate constant (k)? [Hint: The units of the rate constant should match the overall reaction order
Use the following data table to answer the following questions. Experiment Concn. of A (M) Concn. of B (M) Initial rate (M/s) 1 0.10 0.010 1.2e-3 2 0.10 0.040 4.8e-3 3 0.20 0.010 2.4e-3 d. The rate constant of the reaction is e. The rate of reaction when concentration of A and B are 0.15M and 0.075M is
* 97% 7:58 PM Wed Feb 12 х Unanswered •1 attempt left • Due on Feb 13 Rate law of a reaction is experimentally determined as Rate = k [A]^2 [B]^0 [C] The unit of k is sec/M 1/M^3-sec 1/M^2-secc. 1/M^4-sec M^3/sec Submit
[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.
The following initial rate data are for the reaction of ICl with hydrogen: 2 ICI + Hz Iz + 2 HCI Experiment [ICI],, M [H2]o, M Initial Rate, Ms 1 0.205 6.75x102 1.77x103 0.410 6.75x102 3.53x103 2. 3 0.205 0.135 7.06x10-3 0.410 0.135 1.41×10 2 4 Complete the rate law for this reaction in the box below. Use the form k[A]"[B]" , where 'l' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or Rate = Common Greek(upper) Greek(lower) Arrows Other From these data, the rate constant is X, Ox Aa (s) (1) (g) (aq)