storyBookmarksWindowHelpe prod01-cnow-owl.cengagenow.comBb ContentX OWLV2 | Online teaching and leaParaphrasing .ewriting ToolCar note CAU EMAIL CANVAS Pirate Ship MYJSCCBLACKBOARD Vacancies | A. BirminghamNew NCOER C.e Measures[References)Use the References to access important values'needed for this question.The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution:NH, + NO, -N2 + 2 H,0ExperimentNH,o, MNO,1,, MInitial Rate, Msl10.7140.1553.32x10-56.64x1056.65x10-520.7140.3101.430.15541.430.3101.33×104Complete the rate law for this reaction in the box below.Use the form kJAJ"|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 nRate =otptFrom these data, the rate constant isM'sptIptSubmit AnswerTry Another Version3 item attempts remaining(Pr10tvMacBook Air80DDF2F3F4F5F6F7F8F9F10#3$&*46.78

We will use this question by using data given and then dividing one by one.

Use the References to access important values if needed for this question. The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution: NH, + NO, N2 + 2 H,O Experiment INH,Jo, M [NO,lo, M Initial Rate, Ms 3.32x105 6.64x105 6.65x105 1.33x104 1 0.714 0.155 2 0.714 0.310 1.43 0.155 4 1.43 0.310 Complete the rate law for this reaction in the box below, Use the form k[AJ"|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 ot Rate = ot pt From these data, the rate constant is M's pt pt Submit Answer Try Another Version 3 item attempts remaining

Use the References to access important values if needed for this question. The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution: NH, + NO, N2 + 2 H,O Experiment INH,Jo, M [NO,lo, M Initial Rate, Ms 3.32x105 6.64x105 6.65x105 1.33x104 1 0.714 0.155 2 0.714 0.310 1.43 0.155 4 1.43 0.310 Complete the rate law for this reaction in the box below, Use the form k[AJ"|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 ot Rate = ot pt From these data, the rate constant is M's pt pt Submit Answer Try Another Version 3 item attempts remaining

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 complex reaction: P + 2Q → Products whose initial rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: Trial [P](M) [Q](M) Rate(M/s) 1 0.100 0.050 2.25 × 10−3 2 0.100 0.150 6.75 × 10−3 3 0.200 0.050 9.00 × 10−3 A) Write the rate law for this reaction. Use k to represent the rate constant. B) Solve for k in the above rate law (express your answer to three significant figures), and select the units for k.
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[03mol/L Initial Rate mol/L.s S02 m 7/1ou 0.118 0.25 0.40 0.25 0.20 0.118 0.75 0.20 1.062 Q1 Consider the following reactions SO2+03 → SO3 +O2. A rate study of this reaction was conducted at 298 K. The data that were obtained are shown in the table (a) What is the order of reactions for S02 (b) What is the order of reactions for 03 (c) Write the rate law (d) Determine the value and units of the rate constant, k
The rate of a certain reaction was studied at various T(K) k (s-1) temperatures. The table shows temperature (T) and rate 400 0.000108 constant (k) data collected during the experiments. Plot the 420 0.000626 data to answer the questions. 440 0.00310 What is the value of the activation energy, E, for 460 0.0134 this reaction? 480 0.0511 500 0.175 520 0.547 E, = kJ - mol- 1108.79 540 1.57 560 4.18 Incorrect 580 10.4 What is the value of the pre-exponential factor (sometimes called the frequency factor), A, for this reaction? A = 140 6.79 x10 Incorrect
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1. In the Rates of Chemical Reactions lab you measured the experimental rate of the following reaction: S208 +212 +2 SO4² 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? 2. The initial rates listed in the following table were determined for the reaction: H2PO3 (aq) + OH (aq) →HPO3²¯ (aq) + H2O (1) Trial Initial [H₂PO3¯], (M) Initial [OH], (M) Initial Rate of Consumption (M/s) 1 0.025 0.030 0.432 2 0.100 0.030 1.728 3 0.100 0.015 0.864 a) 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 H₂O Trial Initial [I] (M) Initial [H+] Initial [H2O2] (M) Rate (M/sec) (M) 1 0.001 0.005 0.001 2.0 x 104 2 0.002 0.005 0.001 4.0 x 10+ 3 0.006 0.002 0.001…
3. The following results were obtained by monitoring the reaction + 1e+1/2 H,Oo) 1/2 I(a0)+ H,O (bo) rate l'o'Hl 0.020 0.020 3.3 x 105 0.040 0.020 6.6 x 105 0.020 9.0 x 10-5 0.040 0.040 1.3 x 104 Determine the order of the reaction with respect to I' and H,O, and also determine the value for the rate constant, k
The following initial reaction rates have been measured for the following reaction NO2(g) + O3(g) -> NO3(g) + O2(g) Experiment: Initial Concentration (M) initial rate of the reaction O3 NO2 1 0.7 0.21 6.3 2 1.39 0.21 12.5 3 0.7 0.38 11.4 4 0.18 0.66 X a) Determine the order of and write the rate law of the reaction b) determine the value of K for the reaction. c) Find X
Values if needed for this question. The following initial rate data are for the reaction of mercury(II) chloride with oxalate ion: 2 HgCl2 + 2 CI + Hg,Cl2 + 2 CO2 Experiment [HgCl2]o, M [C,0,?], M Initial Rate, M sl 1 0.415 0.180 1.23x104 0.830 0.180 2.45x104 4.91×10-4 9.81×104 3 0.415 0.360 4 0.830 0.360 Complete 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 power not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is M2s1 Submit Answer Try Another Version 2 item attempts remaining
Find the rate constant (M-1 s-1) for the reaction
Consider the reaction between nitric oxide and hydrogen 2NO + H2 → N20 + H20 Initial Rate of Disappearance of NO Experiment Initial [NO], M Initial [H2], M (mol/L sec) 1 6.4 x 10-3 2.2 x 10-3 2.0 x 10-5 2 12.8 x 10-3 2.2 x 10-3 8.0 x 10-5 6.4 x 10-3 4.4 x 10-3 4.0 x 10-5 What is the rate law for this reaction? a. Rate = k[NO] b. Rate = k[NO]? c. Rate = k[NO]²[H2] d. Rate = k[No][H2]
Need the following questions answered The reaction of interest: O2 (g) + 2 NO (g) → 2 NO2 (g) Expt. [O2] (M) [NO] (M) Initial Rate (M/s) 1 0.0110 0.0130 0.00321 2 0.0220 0.0130 0.00640 3 0.0110 0.0260 0.01280 4 0.0330 0.0130 0.00960 5 0.0110 0.0390 0.02880 What is the reaction order for oxygen? What is the reaction order for nitrogen monooxide? What is the overall reaction order? What is the rate law for this reaction? What is the specific rate constant (k) for this reaction? Write the rate law for this reaction that includes the numerical value of the specific rate constant: