The decomposition of N, O, can be described by the equation 2N,0,(soln) 4 NO, (soln) + 0,(g) Consider the data in the table for the reaction at 45 °C in carbon tetrachloride solution. t(s) [N,0,1 (M) 2.194 175 1.965 506 1.596 795 1.331 Given the data, calculate the average rate of reaction for each successive time interval.

The decomposition of N, O, can be described by the equation 2N,0,(soln) 4 NO, (soln) + 0,(g) Consider the data in the table for the reaction at 45 °C in carbon tetrachloride solution. t(s) [N,0,1 (M) 2.194 175 1.965 506 1.596 795 1.331 Given the data, calculate the average rate of reaction for each successive time interval.

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

Ozone decomposes to oxygen gas. 2O3(g) → 3O2(g) A proposed mechanism for this decomposition is O3 K1⇌ k O2+O (fast, equilibrium) O3+O → 2O2 (slow) What is the rate law derived from this mechanism?
The rate constant at a given temperature for the reaction A →→ 2 B is 0.0145 s¯¹. What is the concentration of B (in molarity) after 1.8 minutes if the initial concentration of A is 2.6 M? Enter your answer without units.
Deducing a rate law from the change in concentration over time A chemistry graduate student is studying the rate of this reaction: 2N,O5 (g) →2N,0, (g) + O, (g) He fills a reaction vessel with N,0, and measures its concentration as the reaction proceeds: alo [N,0,] time (seconds) Ar 0.0800M 0.10 0.0450M 0.20 0.0253 M 0.30 0.0142M 0.40 0.00801 M Use this data to answer the following questions. Write the rate law for this reaction. rate = k Calculate the value of the rate constant k. k = Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol.
The following initial rate data was obtained for the reaction between oxygen and nitric oxide. 2 NO(g) + O₂(g) → 2 NO2(g) [0₂] (M) [NO] (M) Rate (M s-¹) 0.0100 0.0150 0.0150 0.0100 0.0100 0.0200 10.0 22.5 45.0 J What is the rate law for this reaction under these conditions? Rate = k [0₂]2 [NO]² Rate = k [0₂] [NO]² Rate = k [0₂]²2 [NO] Rate = k [0₂] [NO] G
Some measurements of the initial rate of a certain reaction are given in the table below. [N] N2 H, initial rate of reaction 1.89M |0.180M 0.848 M/s 1.89М |0.686M 12.3 M/s 0.689M| 0.180M 0.113 M/s 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 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k|| х10 k =
At a certain temperature the rate of this reaction is second order in SO, with a rate constant of 4.02 M 's': 2S0, (g) → 2S0, (g) +0,(g) Suppose a vessel contains SO , at a concentration of 0.790 M. Calculate how long it takes for the concentration of SO, to decrease to 0.103 M. You may assume no other reaction is important. Round your answer to 2 significant digits.
Determine the rate law and the value of k for the following reaction using the data provided. 2 NO(g) + O2(g) → 2 NO₂(g) [NO]i (M) [0₂]i (M) 0.030 0.030 0.060 A) Rate = 57 M-1s-1 [NO][0₂] B) Rate = 3.8 M-1/2-1[NO][0₂]¹/2 C) Rate = 3.1 x 105 M-³s-1 [NO]²[0₂]² D) Rate = 1.7 × 103 M-2s-1 [NO]²[0₂] E) Rate = 9.4 × 103 M-²s-1 [NO][0₂]² 0.0055 0.0110 0.0055 Initial Rate (M-1,-1) 8.55 × 10-3 1.71 × 10-2 3.42 × 10-2
Consider the reaction: 5Br−(aq) + BrO3-(aq) + 6H+(aq) → 3Br2(aq) + 3H2O(l)If the rate of consumption of Br− is 1.26x10-4 mol L−1 s−1, what is the rate of formation of Br2? Express your answer to three significant figures.
When designing a consumer product, it is desirable for it to have a two-year shelf life. Often this means that the active ingredient in the product should not decrease by more than 5% in two years. If the reaction is first order, and the rate constant is: k = 2.56 × 10-2 yr 1, determine the half-life of an active ingredient that has a shelf life of 2.00 years. The half-life of an active ingredient is i yr.
For A⟶products, time and concentration data were collected and plotted as shown. [A] (M) t (s) 0.750 00.0 0.596 30.0 0.473 60.0 0.376 90.0 Determine the reaction order, the rate constant, and the units of the rate constant. order= k= units
The following initial rate data are for the reaction for the formation of phosgene from carbon monoxide and chlorine: со + Clz → COCI2 Initial Rate, Ms-1 Experiment [CO]o, M [CIz]o, M 2.45 0.399 1.43x10-28 2 2.45 0.798 |2.85х10-28 3 4.90 0.399 2.85x10-28 4 4.90 0.798 5.71x10-28 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]^ , 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-1s-1.
Consider following reaction: 2 A2B5(g) → 4AB2(g) + B2(g) The rate constant is 0.129 s-1 at 298 K for this reaction. What is the percent of A2B5 left after the first 19.091 s? Report your answer with three decimals. Enter numbers only;