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...

See similar textbooks

Similar questions

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.
[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
Label the reaction profiles below as exothermic or endothermic and use them to calculate the activation energy of the forward and reverse reactions and the value of AH for the reaction. This is a reaction of profile of an 250 exothermic/endothermic reaction 200 PE 150 (kJ) Eaf = ...... 100 Ea, = 50 AH = Reaction pathway 100 This is a reaction of profile of an 80 exothermic/endothermic reaction 60 PE (kJ) A+B 40 Ear = C+D 20 Ear = ΔΗ Progress of the reaction
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
Based on the initial rates given below, determine the rate constant, k for the following reaction. NH," (aq) + NO2- (aq) → N2 (g) + 2H½O (1I) Rate (Ms-') 2.50 x 10-3 5.00 x 10-3 1.25 x 10-3 Experiment 1 Experiment 2 Experiment 3 NH4" (M) 0.500 NO2 (M) 0.500 0.500 1.000 0.500 0.250 O 0.04 M-1 s-1 0.01 M-1 s-1 0.04 M s-1 O 0.01 M s-1
The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution: NH4+NO₂ → N₂ + 2 H₂O Experiment [NH4+]o, M [NO₂ ]o, M Initial Rate, M. s-1 0.0358 1.45 x 10-6 0.0715 0.0358 0.0715 1 2 3 4 Rate = 0.128 0.128 0.255 0.255 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 zero power do not appear. Don't enter 1 for m or n. k = 2.89 x 10-6 2.88 x 10-6 5.76 x 10-6 M-1.s-1
The following data were collected for a certain reaction of the type A +B → products. Determine the specific rate constant for this reaction. [A]o, mol L-1 [B]o, mol L-1 Initial rate, mol L-1 s-1 Run i 0.200 0.300 2.44 x 10-2 ii 0.200 0.450 2.44 x 10-2 i 0.300 0.450 5.49 x 10-2 O A. 0.610 L mol s-1 B. 0.960 L mol1 s-1 C. 0.271 L mol-1 s-1 D. 0.407 L mol-1 s-1 O E. 0.120 L mol-1 s-1
23 II. An experiment followed the decomposition. of nitregen dioxide to nitregen monoxide & oxygen gas. Given the following data, what order is the reaction for nitrogen dioxide? Given an initial concentration of nitrogen dioxide of 0.0400 M, what's the concentration of this reactant after a half hour? show all grapers & calcs to determine answers. (sec) Time |[NO₂] (M) 0.0 50.0 100.0 200.0 300.0 0.01000 0.00787 0.00649 0.00481 0.00380 M G 2 XX 6.5 Hoa X019 201 2(x) = 2 (1.86) (3 (9)
Match the quantities that yield straight lines for the given types of reactions molarity vs. time zero order rate equations inverse molarity vs. time secondorder rate equations In molarity vs. time firstorder rate equations inverse molarity vs. inverse time not a straight line for any type & へへ

* 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
7. Use the following data to determine the rate law for the reaction 2NO+H,N,0 + H20. Exp No. (NO] (M) (CI) (M) Rate (M/min 0.021 0.065 1.46 0.021 0.260 1.46 0.042 0.065 5.84 Select one