The following initial rate data are for the reaction of mercury(II) chloride with oxalate ion:\[ 2 \text{HgCl}_2 + \text{C}_2\text{O}_4^{2-} \rightarrow 2 \text{Cl}^- + \text{Hg}_2\text{Cl}_2 + 2 \text{CO}_2 \]| Experiment | [HgCl₂]₀, M | [C₂O₄²⁻]₀, M | Initial Rate, M s⁻¹ ||------------|-------------|---------------|----------------------|| 1 | 8.53×10⁻² | 0.378 | 1.26×10⁻⁴ || 2 | 0.171 | 0.378 | 2.52×10⁻⁴ || 3 | 8.53×10⁻² | 0.756 | 5.02×10⁻⁴ || 4 | 0.171 | 0.756 | 1.01×10⁻³ |Complete the rate law for this reaction in the box below. Use the form k[A]^m[B]^n, 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 \_\_\_\_\_\_ M⁻²s⁻¹.

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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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(c) A reaction between substances R and S was second order with respect to R and second order with respect to S. S-or x 8.1 0.3 At a given temperature, the initial rate of reaction was 1.20 x 10-3 mol dm-3 s-1 when the initial concentration of R was 1.00 x 10-2 mol dm-3 and the initial concentration of S was 2.45 x 10-2 mol dm-3 acom ton Scor 0.8 Calculate a value for the rate constant, k, for the reaction at this temperature. Give the units for k rose ni to nollbeen to stist leitini ert worla of SeldsT otalama) (B) S eldsT amb tom \\ els fallinl Ot *8.1 Inomheqx3
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5. Consider the table of initial rates for the reaction: 2CIO2 + 20H1- CIO31- + CIO21- + H2O Trial [CIO2] [OH] Initial Ratess 1 0.012 0.012 2.07 x 10-4 0.024 0.012 8.28 x 10-4 3. 0.012 0.024 4.14 x 10-4 4 0.024 0.024 1.66 x 10-3 Order with respect to [CIO2): Order with respect to [OH]: Rate law of this reaction: Value and units for the rate constant:
The following initial rate data are for the reduction of nitric oxide with hydrogen: ... 2 NO + 2 HzN2 + 2 H2O Experiment NO],, M [H]o, M Initial Rate, M s 8.66x10-2 1 0.370 0.408 2 0.740 0.370 0.740 0.408 0.816 0.346 0.173 0.693 3 0.816 From these data, what is the rate constant in M?s1 (A) 2.55 B) 1.55 (c) 3.55 D) 4.55
[A] vs Time In[A] vs Time 1/[A] vs Time O Least Squares Plot Time, s The reaction A - C was performed and the concentration vs. time data below collected. time, s 2 3 4 5 7 8 [A], mol/L 0.9540 0.5864 0.3605 0.2216 0.1362 0.08371 0.05145 0.03163 0.01944 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) = reaction order = [v]uj
For the reaction: BrO3-(aq) + 5Br (aq) + 8H*(aq) → 3Br2(/) + H201) The initial rate of the reaction has been measured at the reactant concentration show: Trial [BrO;] (mol/L) 1 [H'] [Br ] Initial rat (mol/L) (mol/L) (mol/L-s) 0.10 0.10 0.10 8.0 0.20 0.10 0.10 16 0.10 0.20 0.10 16 4 0.10 0.10 0.20 32 The value for k will be: A L/mol.s Ouestion 13 (1 23
(50,00 Puanlar) 1- Decomposition reaction of ozone (03) in water follows second-order kinetics with a rate constant of 70 M-1sec-1. Assuming that the initial concentration of ozone in water is 1x10-4 M. how many seconds are required for the concentration of ozone to reach 2.5x10-5 M? 015022 92.6 b) 116.9 c) 174.6 265.3 428.6 Boş bırak
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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
Assume that the reaction: 2A + 3B --> 2C is first order in both reactants A and B. Calculate the value of the reaction rate constant if the initial rate is .10 M/s when initial [A] is .15M and the initial [B] is .12M Group of answer choices .18 5.6 37 .67
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