QUESTIONThe rate law for the following reaction is rate = k[F][CIO₂]. What is the value of k basedon the given data?ANSWERO4.16 × 103 M'sF,(g) +2 CIO(g)-2 FCIO,(g)Trial [F] (M) [CIO,] (M) Initial rate (M/s)10.0500.0250.13020.0500.0500.26030.2000.0250.5200.160 MS10.0550 M¹s104 M'sОI DON'T KNOW YET

Answered: QUESTION The rate law for the following…

Chemistry

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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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doubleonship of rate = kIX?[YLIfthe concentration of X is tripled and the concentration of Y doubled, the reaction rate would be increased by a factor o1: a) 6 b) 9 с) 12 d) 18 e) 36 f) 4 g) 3 h) 24
Current Attempt in Progress The reaction 2A + 2B M+Nhas the rate law: Rate = k[A]?. At 25°C, k = 0.0376 L mol1s1. If the initial concentrations of A and B are 0.387 M and O.459 M, respectively Your answer is correct. (a) What is the half-life of the reaction? 68.7 seconds Hint Your answer is incorrect. (b) What will be the concentrations of A and B after 30.0 minutes? [A] = i ! M [B] = i M Hint
Question 18 of 25 -/1 E At least three possible reaction mechanisms exist for the reaction of hydrogen with halogens, H+X-2HX Determine the rate law predicted by each of them: (a) H + X - 2HX (bimolecular, direct) (b) X, X+x (slow) X+H2 HX+H (fast) H+X HX (fast) (c) X X+X (fast reversitle) *+H HX+H (slow) H+X HX (fast) In case of first order type 1 (a) Rate = [X:1 (b) Rate [H:1 (X: i (e) Rate = k2 (H2) [X21 Save forLater Attempts: 0 of 2 used Submit Answer
2. Consider the reaction A+2B C whose rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: [v] (M) (M) (M/s) [B] Rate Trial 1 0.10 0.050 6.0x10-4 0.10 0.100 1.2x10-3 3 0.20 0.050 2.4x10-3 Part B Provide
Current Attempt in Progress The following reaction is investigated to determine its rate law: 2NO(g) + 2H2(g) → N2(g) + 2H2O(g) Experiments yielded the following results: Initial Concentrations (mol L-1) Initial Rate of Formation of N, (mol L-s-) [NO) [H,1 0.40 x 10-4 0.30 x 10-4 1.0 x 10- 0.80 x 10-4 0.30 x 10-4 4.0 x 10- 0,80 x 10-4 0.60 x 10-4 8.0 x 10- What is the rate law for the reaction? O rate = k [NO][H2]² O rate = k [NO]?[H2] O rate = k (NO]?[H2]? O rate = k (NO][H2] What is the value of the rate constant? k= i x 105 O L mol 1s1 O s-1 O L³mol 3s1 O mol L1s-1 O L² mol-2s 1
Consider the following complex reaction: A + 2B → C whose initial rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: Trial [A](M) [B](M) Rate(M/s) 1 0.400 0.050 9.60 × 10−3 2 0.400 0.100 1.92 × 10−2 3 0.800 0.050 3.84 × 10−2 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. Include units for k.
Question 3 of 8 Submit What are the units for the rate constant of a reaction with the rate law, Rate = k[A][B]? %3D A) s-1 B) M s-1 С) М-1 s-1 D) M-2 s-1 E) s M-1
Use the previous example for the chemical reaction 2 HgCl₂(aq) + C₂O4²-(aq)→ 2 Cl(aq) + 2 CO₂ (g) + Hg₂Cl₂ (s) The following initial rates of reactions were determined for the reactant concentrations given: Experiment #[HgCl₂] 0.100 0.100 0.050 1 2 3 [C₂O4²-] 0.20 0.40 1.2 x 10-4 0.40 6.2 x 10-5 Initial rate (M/sec) 3.1 x 10-5 (a) Find the order of the reaction with respect to HgCl2₂. (b)Find the order of the reaction with respect to C₂04² (c)Write the rate law for this reaction. (d)Calculate the value for the rate constant based on the data for experiment #1 and provide the proper units.
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Consider the following complex reaction: 2NO2(g) + O3(g) → N2O5(g) + O2(g) whose initial rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: Trial [NO2](M) [O3] (M) Rate (M/s) 1 0.20 0.40 0.25 2 0.40 0.40 0.50 3 0.40 1.20 1.50 What is the rate law for this reaction? Write the value for k to two significant figures in the first box. Select the units for k and concentration terms in the second box.

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