PROBLEM-SOLVING:The following data shows the decomposition of hydrogen peroxide, H202 in an aqueous solution over time.TimeConcentration(hr)(mg/mL)0.0990100.0497150.0249200.0125On a Regular graphing paperConstruct the C vs t plot on a, indicate the proper labels. Take a snapshot of your work.On a Short Bond paper1. Determine the order of reaction2. Calculate1. Slope of the line2. Rate constant3. Half-lifeShelf-lifeLO

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Answered: The following data shows the…

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 tabulated data shows the concentration of N2O5 versus time for the reaction: N2O5=NO3+NO2 Time, s [N2O5], M 0 1.0 25 .822 50 .677 75 .557 100 .458 125 .377 150 .310 175 .255 200 .210 Determine the order of the reaction.
For the following reaction, the rate that the H2 is being consumed is 6.2 x 10-3 M/s. N2 (g) + 3 H2(g) --> 2NH3(g)Determine the rate of formation of (NH3) for this reaction at the same time. Select one: a. 4.1 x 10-3 M/s b. - 4.1 x 10-3 M/s c. 9.3 x 10-3 M/s d. -9.3x 10-3 M/s e. 1.3 x 10-2 M/s
Consider the following gas-phase reaction. A(g) + 2B(g) → C(g) Use the data set to determine the order of the reaction in A, the order in B, the overall order and the rate law, including the value of the rate constant. Initial concentration A (mol L-1) Initial concentration B (mol L-1) Initial Rate (mol L-1 s-1) 0.12 0.32 3.60 x 10-4 0.12 0.64 3.60 x 10-4 0.24 0.32 7.20 x 10-4 Use the rate law that you have found to determine the initial rate of the reaction if the initial concentrations are [A] = 0.33 mol L-1 and [B] = 0.46 mol L-1. How is the rate of appearance of C related to the rate of disappearance of B?
22. Use half-life trends from the data provided to determine the reaction order for the decomposition A(g) → Products(s). Time (min) Pressure (atm) reaction: 17 42 55 68 90 119 177 0.83 0.66 0.51 0.46 0.42 0.36 0.31 0.23 b. first second d. third c. a. zero own
Can someone please help with question 5
Some measurements of the initial rate of a certain reaction are given in the table below. [₂] [H₂] initial rate of reaction 0.912M 2.49 M 18.0M/s 0.374M 2.49 M 0.912M 11.2 M Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k 3.03 M/s 364. M/s k = ☐ x10 ロ・ロ X
100 80 60 40 20 AB+ C ABC Progress of Reaction A + BC The answers for the above question is exact. You must determine what each dash is worth to determine the scale. If the line looks a bit off that is because it is. All answers will be on a dash. The activation energy for the forward reaction is enthalpy change for the forward reaction is the reverse reaction is The reverse reaction is The activation energy for the reverse reaction is The The enthalpy change for thermic. . The forward reaction is thermic. The chemicals that forms the activated complex is . The requirement besides energy that must be met before a collision between two reactant particles is considered effective is the correct
A kinetics experiment was conducted based on the reaction: 2NO + H2 - N20 + H20 Use the following data from the experiment to determine the rate law for the reaction. Expt. # Initial rate 1.46 M/min INO]. [H:]0 1 0.021 0.065 2 0.021 0.260 1.46 M/min 3 0.042 0.065 5.84 M/min rate = k[NO] 2[H 2) 2 rate = k[NO] rate = k[NO] 2[H 2] rate = k[NO][H 2] rate = k[NO] 2
8. Smelling salt decomposes spontaneously at room temperature by the equation below. A student places a 10.00-g sample into a 1-liter sealed rigid vessel. What measurements should the student make to determine the rate of this reaction?(NH4)2CO3(s)→2NH3(g)+H2O(g)+CO2(g) a. change in mass and temperature b. temperature and time c. change in mass and time d. change in pressure and time
A student follows the Determining the Rate Law for the Crystal Violet-Hydroxide lon Reaction procedure. The stock concentration of sodium hydroxide used in trial 1 is 0.021 M. The stock concentration of sodium hydroxide used in trial 2 is 0.010 M. Given the data below, what is the hydroxide ion concentration (M) in the trial 1 reaction mixture? Give your answer to four decimal places. Volume NaOH Volume Crystal Violet (mL) (mL) Trial 1 5.00 5.00 Trial 2 5.00 5.00
17. SHOW ALL YOUR WORK OGiven the following data, determine the order of the reaction with respect to NO(g). 2 NO(g) + Cl2(g)→ 2 NOCI(g) Experiment 1 [C2] (M) 0.0100 [NO] (M) Rate (M/s) 3.4 x 104 1.36 x 103 3.4 x 104 0.0300 0.0150 0.0150 0.0100 3 0.0400
n

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