Question 1 (a) Distinguish between the differential rate law and the integrated ratelaw. Which of these is often called just the "rate law"? What is half-life offirst order reaction?(b) The rate of the reaction;O(g) + NO2 (g) NO(g) + O2(g) was studied at a certain tem-perature.1) In one experiment, NO2 was in large excess, at a concentration of 1.0x 1013 molecules/cm3 with the following data collected:Time (s)(atoms/cm)5.0 x 101.0 x 10-1.9 x 102.0 x 106.8 x 103.0 x 10-2.5 x 10What is the order of the reaction with respect to oxygen atoms?ii). The reaction is known to be first order with respect to NO2. De-termine the11alue of tanstant

Answered: Image /qna-images/answer/beb7e4d2-df88-4b25-b09a-0de233550966.jpg

Answered: Question 1 (a) Distinguish between the…

Question 1 (a) Distinguish between the differential rate law and the integrated rate law. Which of these is often called just the "rate law"? What is half-life of first order reaction?

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...

See similar textbooks

Similar questions

Determine the rate constant (with appropriate unit) and reaction orders of the reaction of A + B à C using the following data. Then write the full differential rate law of this reaction. Include any calculations using Word’s equation editor. [A] (M) [B] (M) Initial Rate (M/s) 0.0064 0.0055 0.0347 0.0128 0.0055 0.0694 0.0128 0.0110 0.2776
The reaction rate (k) for a zeroth order decomposition reaction is 0.050. If the initial concentration oka reactant is 1.71 mol/L, how much time (sec) is needed to reduce the concentration to 5% of the original concentration? Report seconds in digits (i.e., no decimal places) without units. Your Answer:
A reaction mechanism is defined as the sequence of reaction steps that define the pathway from reactants to products. Each step in a mechanism is an elementary reaction, which describes a single molecular event of usually one or two molecules interacting. Part A The rate law for an overall reaction is the rate law for the slowest step in the mechanism, which is directly related to the stoichiometric coefficients of the reactants. What is the rate law for the following mechanism in terms of the overall rate constant k? Step 1: Step 2: B+ C C ( fast) + D (slow) A +B The exception to this rule occurs when the slowest step contains intermediates. In these cases, the slowest step is usually preceded by an equilibrium step, which can be used to substitute for the intermediates in the overall rate law. Express your answer in terms of k and the necessary concentrations (e.g., k*[A]^3* [D]). • View Available Hint(s) Hνα ΑΣφ ? rate =
The answer is circled I just need help with what the work is suppose to look like.
At a certain temperature the rate of this reaction is first order in NH, with a rate constant of 1.83 s 2NH, (g) - N2 (g) +3H, (g) Suppose a vessel contains NH, at a concentration of 1.42M. Calculate the concentration of NH, in the vessel 0.710 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. | M Submit Assignmer Continue O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center| Accessibilit 43,203 FEB 18 CH.9 PF ASSESS MacBook Air FIO F9 D00 D00 F4 F7 F8 吕口 F3 esc F5 F6 F1 F2 3)
Suppose a 350. mL flask is charged under these conditions with 100. mmol of hydrogen iodide. After how much time is there only 50.0 mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.
only answer question 8 answer
Please don't provide handwritten solution ....
Question 17 of 19 Submit What is the rate law for the proposed mechanism? A) rate = k[H2][NO] H2(g) + 2NO(g) → N20(g) + H2O(g) B) rate = k[Hzl°[NO] Step 1 (slow) C) rate = k[H2][NO]? N20(g) + H2(g) N2(g) + H2O(g) Step 2 (fast) D) rate = k[H2l°[NO]? E) rate = k[H2][N2O]
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.
Substance A can react to form products. The concentration of Substance A versus time for the reaction is plotted below in three ways, including linear trend lines for each plot. A → products a) Write the rate law for the reaction (including the value and units of the rate constant). Explain how you got your answer. b) Determine the concentration of A after 220 seconds have passed.  Use 3 significant figures. c) Determine the half-life of the reaction after 220 seconds have passed.  Use 3 significant figures.
1) 2 H,Oz (aq) → 2 H2O (l) + Oz (g) Time (s) 0 10 20 30 40 50 60 70 80 [H₂O₂] (M) 1.00 0.75 0.55 0.40 0.30 0.22 0.18 0.12 0.10 Use the experimental data for the above reaction to answer. a) What is the average rate of disappearance of H₂O₂ between 30 and 40 seconds? b) What is the average rate of reaction between 50 and 70 seconds? c) What is the average rate of formation of O₂ between 40 and 60 seconds?