Be sure to answer all parts.Benzoyl peroxide, the substance most widely used against acne, has a half-life of 9.8 × 10³ days whenrefrigerated. How long will it take to lose 2% of its potency (98% remaining)? Assume that this is afirst-order reaction. Give your answer in scientific notation.×10 (select)days

Answered: Image /qna-images/answer/8c1390f3-f8f3-4d7c-ad9e-4590a0a4a724.jpg

Answered: Be sure to answer all parts. Benzoyl…

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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A chemical engineer is studying the rate of this reaction. 2H₂PO4 (aq)→ P₂O5 (aq) + 3H₂O (aq) He fills a reaction vessel with H3PO4 and measures its concentration as the reaction proceeds. Here's a graph of his data: (w) ['od³H] 0.5 0 0.2 0.4 0.6 t (s) 0.8
A chemical engineer is studying the rate of this reaction. NH,OH (aq) NH, (aq)+H,O (aq) He fills a reaction vessel with NH,OH and measures its concentration as the reaction proceeds. Here's a graph of his data: 0.2 0.15 0.1 0.05 4 t(s) (s) (w)[HO'HN]
Given the experimental data below, what is the average value for the rate constant, k, for this reaction? You will first need to calculate the value for m in the rate law to answer this question. 2 SO3(g) → 2 SO2(g) + O2(g) Trial SO3 Concentration (M) Initial Rate (M/s) 1 0.225 4.09 × 10–6 2 0.675 1.66 x 10-5 general form of the rate law: rate = k [SO3]"
A substance undergoes first-order decomposition. After 28 min at 500°C, only 12.5% of the original sample remains. What is the half-life of the decomposition? Round your answer to 2 decimal places.
Write the relative reaction rates for the following reaction: A + 2B → C
A city's water supply is contaminated with a toxin at a concentration of 0.63 mg/L. Fortunately, this toxin decomposes to a safe mixture of products by first-order kinetics with a rate constant of 0.27 day1. How long will it take for half of the toxin to decompose? 2.3 days 2.6 days 0.27 days 0.17 days 0.38 days
Choose all of the following that are true. Raising the temperature of a reaction will have no effect on the reaction rate. The units of the rate constant are independent of the overall reaction order. For a zero order reactant, tripling the concentration will have no effect on the rate. The plot of ln[A] vs time results in a straight line when a reaction is second order. Rates of reaction can be positive or negative. Activation energy is the maximum energy needed to initiate a chemical reaction.
The generic reaction shown below follows second-order kinetics. 3 A + 2 B → products The half-life of A is 65.0 seconds when the initial concentration of A is 0.858 M. Determine the value of the rate constant for this reaction. Round your answer to 3 significant figures. You do not need to enter a unit.
Given the initial rate data for the reaction below, determine the rate law for this reaction. 4A + 7B ⟶ 4C + 6D [A], M [B], M Δ[C]/Δt (initial), M/s 0.050 0.050 1.04 0.150 0.050 3.12 0.050 0.250 26.0 a ) None of the other answer options are correct. b) rate = 8320 M-2 s-1 [A]2 [B]1 c) rate = 6.66 x 107 M-5 s-1 [A]5 [B]1 d) rate = 2.13 x 1014 M-10 s-1 [A]4 [B]7 e) rate = 8320 M-2 s-1 [A]1 [B]2 Please explain your reasoning and show your work.
Determine the reaction-rate law and the value of the rate constant. 2 NO(g) + Br2(g) → 2 NOBr(g) Answer: rate of reaction = (1.30 × 10–3 M–2 . min–1)[NO]2[Br2] I need steps, I don't know how to get the exponent for NO as 2, i keep getting it as a first order reaction.
At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.0654 s 2NH₂(g) →1 → N₂(g) + 3H₂(g) Suppose a vessel contains NH3 at a concentration of 0.680M. Calculate the concentration of NH3 in the vessel 9.20 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M 0.0 X S
Consider the reaction below. The reaction starts with an initial concentration [A] of 3.50x10-2 M and is tracked over time. The rate of change is then plotted versus time; the graph is initially nonlinear, but becomes linear when 1/[A] is plotted versus time. The slope of the graph was determined to be +1.80x10-2 L/mol s.aA → bB 1. Calculate the half life for this reaction.2. How much time (in seconds) is required for the concentration of A to decrease to 4.00x10-3 M?

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