**Data for the Decomposition of Hydrogen Peroxide****Reaction:**\[ \text{H}_2\text{O}_2(aq) \rightarrow \text{H}_2\text{O}(l) + \frac{1}{2} \text{O}_2(g) \]**Conditions:**- The data is for the decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C.**Table: Concentration of Hydrogen Peroxide Over Time**| [H₂O₂], M | Time, min ||-----------|------------|| 1.27×10⁻² | 0 || 6.35×10⁻³ | 7.95 || 3.18×10⁻³ | 15.9 || 1.59×10⁻³ | 23.9 |**Notes:**- It is not necessary to graph these data for analysis.**Calculations:**1. **Half-Life:** - The half-life observed for this reaction is ______ min.2. **Reaction Order and Rate Constant:** - Based on these data, the rate constant for this ______ order reaction is ______ min⁻¹.**Instructions:**- Use the provided data to determine the half-life and the rate constant for the reaction.- Submit your answers or retry if needed. ---In a study of the decomposition of ammonia on a tungsten surface at 1100°C, the following data were obtained:\[\text{NH}_3 \rightarrow \frac{1}{2} \text{N}_2 + \frac{3}{2} \text{H}_2\]| [NH₃], M | Seconds ||--------------|---------|| 1.35×10⁻² | 0 || 6.75×10⁻³ | 442 || 3.38×10⁻³ | 663 || 1.69×10⁻³ | 774 |**Hint:** It is not necessary to graph these data.1. The observed half-life for this reaction when the starting concentration is 1.35×10⁻² M is \_\_\_\_ s and when the starting concentration is 6.75×10⁻³ M is \_\_\_\_ s.2. The average rate of disappearance of NH₃ from t = 0 s to t = 442 s is \_\_\_\_ M s⁻¹.3. The average rate of disappearance of NH₃ from t = 442 s to t = 663 s is \_\_\_\_ M s⁻¹.4. Based on these data, the rate constant for this [ ] order reaction is \_\_\_\_ M s⁻¹.**Buttons:**- Submit Answer- Retry Entire Group*Navigation:*- Previous- Next---

Since there are multiple questions, we will answer only the first one. If you require the answers to the other question, please post it separately again.Also this can be confirmed graphically as : We can determine the order of the reaction easily by graphs. This can be done by plotting graphs of time versus concentration of reactant, [A]. If the time vs [H2O2] gives a straight line it will be zero order reaction. If the time vs ln[H2O2] gives a straight line it will be first order reaction. If the time vs 1/[ H2O2] gives a straight line it will be second order reaction. Since, time vs ln[H2O2] gives a perfect straight line. Therefore, the reaction is first order.Answer: The half-life observed for this reaction is 7.95 min The rate constant for this 1(first) order reaction is 0.0913 min-1

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Chemistry

The following data are for the decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C. H2O2(aq) –→ H2O(1) + ½ O2(g) - [H,02 ], M 1.27x10-2 6.35×103 7.95 3.18×10-3 15.9 1.59x103 23.9 time, min Hint: It is not necessary to graph these data. (1) The half life observed for this reaction is min . (2) Based on these data, the rate constant for this order reaction is min ! <>

The following data are for the decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C. H2O2(aq) –→ H2O(1) + ½ O2(g) - [H,02 ], M 1.27x10-2 6.35×103 7.95 3.18×10-3 15.9 1.59x103 23.9 time, min Hint: It is not necessary to graph these data. (1) The half life observed for this reaction is min . (2) Based on these data, the rate constant for this order reaction is min ! <>

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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The general rate law for the reaction is given by rate = k[NH4+]x[NO2-]y. Determine the order with respect to each reactant (i.e. solve for x and y). X = Y = Then determine the value of the rate constant, k (provide your answer to two significant figures). Rate constant, k = x 10 --
Question 9 In the reaction below, using the following data, determine the rate law for the following reaction: NH,° (aq) + NO,"(aq) → N;(g) +2 H,O) Experiment [NHI (M) [NO2] (M) Rate (M/s) 0.2500 0.2500 1.250 x 10-3 0.5000 0.2500 2.500 x 10 -3 0.2500 0.1250 3.125 x 10 -4 Oa. K[NH4 J[NO2 Ob.K[NH4 J[NO27/2 OC. KINH47²INO2 Od. KINH4 INO2 O e. KINH41/2[NO27 MacBook Air SC 吕口 F3 888 F4 F1 F2 F5 F6 F7 F8 F9 F10 F11 23 2$ & 2 3 4 5 7 8 TY Q E R
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The formation reaction of hydroiodic acid was studied by Max Bodenstein in 1897. The results found by him are given in the following table where "T" is the temperature in Kelvin and k₁ and k₂ are respectively the rate constants for the forward and reverse reaction, given in cm³/mol.s. k2 T (K) k1 300 2.04 x 10-16 2.24 x 10-19 500 2.14 x 10-4 1.66 x 10-6 700 3.02 x 10¹ 5.50 x 10-1 Determine the order of the reaction: Answer: n=2.
Consider the reaction data. A⟶productsA⟶products ? (?) ? (?−1) 275 0..370 875 0.675 What two points should be plotted to graphically determine the activation energy of this reaction? To avoid rounding errors, use at least three significant figures in all values. X1= Y1= X2= Y2= Determine the rise, run, and slope of the line formed by these points. rise= run= slope= What is the activation energy of this reaction? Ea= ? J/mol
The decomposition of a single compound at 330 K has a rate constant of 2.52 x 10-3 M-1 s-1. If the initial concentration of the reactant is 0.504 M, what is the concentration of the reactant after 26.30 seconds? (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 12.3 and 120. and -123)
The data given in the table below is for the following reaction (run at 25°C): 2 NO + O, 2(g) → 2 (g) 2(g) Initial Concentration (M) Initial rate Experiment NO 0, Mol/(L · s) 1 0.0010 0.0010 7 x 10-6 2 0.0010 0.0020 14 x 106 3 0.0010 0.0030 21 x 10-6 4 0.0020 0.0030 84 x 10-6 5 0.0030 0.0030 189 x 106 1. Determine the orders of the reaction with respect to NO and O, (show all work): NO
Chemistry 2. The following experimental data are obtained for the decomposition of nitrogen dioxide: 2 NO2(g) → 2 NO(g) + O2(g) ⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯ Time, s [NO2], M ln[NO2], [NO2]-1, M-1 ⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯ 0 10.0 x 10-3 -4.605 1.00 x 102 60 6.83 x 10-3 -4.986 1.46 x 102 120 5.18 x 10-3 -5.263 1.93 x 102 180 4.18 x 10-3 -5.477 2.39 x 102 240 3.50 x 10-3 -5.655 2.86 x 102 300 3.01 x 10-3 -5.806 3.32 x 102 ⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯ Plot a graph of ln[NO2] versus t and 1/[NO2] versus t. Determine the decomposition of NO2 follows a first order or second order rate law with respect to [NO2].
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Consider this reaction: H,CO, (ag) – H,0 (aq) + CO, (ag) At a certain temperature it obeys this rate law. rate = (9.70 x 10-4s)H,co,] Suppose a vessel contains H,CO, at a concentration of 0.470 M. Calculate the concentration of H,CO, in the vessel 680. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. x10
The reaction rate of CO and NO2 in the reaction CO(g) + NO2(g) → CO2(g) + NO(g) is measured using the initial rates method. The results are tabulated below. [CO] (mol/L) NO2 (mol/L) -([CO]/Δt (mol/L·s) 8.00 10-4 5.50 10-4 8.40 10-8 8.00 10-4 7.78 10-4 1.68 10-7 1.60 10-3 5.50 10-4 1.68 10-7 Determine the rate expression and calculate the rate constant for the reaction.