Most of the time, the rate of a reaction depends onthe concentration of the reactant. In the case ofsecond-order reactions, the rate is proportional tothe square of the concentration of the reactant.Select the image to explore the simulation, whichwill help you to understand how second-orderreactions are identified by the nature of their plots.You can also observe the rate law for differentreactions.ptime, 10ⒸP[M] vs timeOPHTOP2.52H1-H₂Rate law: KEHI-64-10ml) 500 KInitial rac-16-10SurtIn the simulation, you can select one of the threedifferent kinds of plots. You may use the Start,Stop, and Reset buttons to observe thecorresponding changes in the plot for differentkinds of reactions. You can also select six differentreactions using the drop-down menu and observethree different types of plots for each reaction.Part BConsider the second-order reaction:ΠΑΣΦ[HI] = 2.45-10²Submit[A]oPrevious Answers2HI(g) →H₂(g) + I2(g)Use the simulation to find the initial concentration [HI], and the rate constant / for the reaction. Whatwill be the concentration of HI after t = 7.67×1010 s ([HI]+) for a reaction starting under the conditionthe simulation?Express your answer in moles per liters to three significant figures.▸ View Available Hint(s)time, sslope - kReview | Constants | Periodic Ta[PMC ?* Incorrect; Try Again; 4 attempts remainingmolL

Answered: Image /qna-images/answer/2e7e6314-6bad-4b2d-9fe2-cc5508d24cd3.jpg

Consider the second-order reaction: 2HI(g) →H₂(g) +12(g) Use the simulation to find the initial concentration [HI], and the rate constant & for the reaction. What will be the concentration of HI after t = 7.67×10¹0 s ([HI]) for a reaction starting under the condition the simulation? Express your answer in moles per liters to three significant figures.

Consider the second-order reaction: 2HI(g) →H₂(g) +12(g) Use the simulation to find the initial concentration [HI], and the rate constant & for the reaction. What will be the concentration of HI after t = 7.67×10¹0 s ([HI]) for a reaction starting under the condition the simulation? Express your answer in moles per liters to three significant figures.

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

It has been found that DDT in the soil decomposes by a first-order reaction with a half-life of 12.0 years. How long would it take DDT in a soil sample to decompose from a concentration of 435 ppbm (parts per billion by mass) to 15 ppbm? | yr 1 2 3 4 5 6. C 7 8. 9. +/- х 100 CO
The reaction described by the equation 0,(g) + NO(g) → 0,(g) + NO,(g) has, at 310 K, the rate law rate of reaction = k[O,][NO] k = 3.0 × 106 M-!·s-! Given that [O,] = 4.0 × 10-4 M and [NO] = 2.0 × 10-³ M at t = 0, calculate the rate of the reaction at t = 0. %3D rate: M/s What is the overall order of this reaction? 3
Consider this reaction: 280; (g) → 2S0, (g) +0, (g) At a certain temperature it obeys this rate law. rate =(3.43 s")[so,] S SO Suppose a vessel contains SO, at a concentration of 0.590M. Calculate the concentration of SO, in the vessel 0.320 seconds later. You may assume no other 3 reaction is important. Round your answer to 2 significant digits. х10
The rate constant for a first order reaction is 0.54 s-1. If a 1.57 M sample reacts for 12 seconds, what concentration (in molarity) will remain?
18.) A generic reaction has the rate law rate = k[A]2[B]1. What is the value of the rate constant, k, if the rate = 0.517 M/s when the [A] = 0.413 M and [B] = 0.904 M? Do not include units. Your Answer:
The reaction so2cl2(g)→so2(g)+cl2(g) is first order. At 660 k it has a rate contsant of 4.5 X 10^-2 s^-1 Determine the concentration of SO2Cl2 at 15.2 seconds, if the initial concentration is 0.583 M.
Initial rate: 1.6 •10^-7mol/L•s K=6.4 •10^-9L/mol•s Rate law: k[HI]^2 Can you please show me the steps.
3. The following mechanism is proposed for the reaction of chlorine with chloroform: Cl, + CHCI, CCI, + HCI Cl, Step 1 fast equilibrium 2Cl CHCI, +CI » HCI +CCI, CCI, +Cl»cCI, Step 2 slow Step 3 fast a) Show that this mechanism gives the correct, overall balanced reaction equation. b) Write the rate law predicted by this mechanism.
At a certain temperature the rate of this reaction is second order in CICH₂CH₂Cl with a rate constant of 0.00455 M S -1 CICH₂CH₂Cl (g) → CH₂CHC1 (g) + HC1 (g) Suppose a vessel contains CICH₂CH₂Cl at a concentration of 1.11 M. Calculate the concentration of CICH₂CH₂Cl in the vessel 900. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.
Select all of the mechanisms that are plausible for the given reaction and its experimentally determined rate law. Overall Reaction: 2NO + Cl₂ → 2NOCl Experimentally Determined Rate Law: rate = k[NO][Cl₂] Step 1: NO + Cl2 ---> NOCl2 (slow) Step 2: NOCl2 + NO ---> 2NOCl (fast) Step 1: NO+ Cl2 ---> NOCl2 (slow) Step 2: NOCl2 ---> NOCl + Cl (fast) Step 3: NO+ Cl ---> NOCl (fast) Step 1: NO + NO ---> N2O2 (slow) Step 2: N2O2 + Cl2 ---> 2NOCl (fast) Step 1: NO + Cl2 ---> NOCl + Cl (slow) Step 2: NOCl + NO ---> NOCl2 (fast) Step 1: Cl2 ---> 2Cl (slow) Step 2: 2NO + 2Cl ---> 2NOCl (fast) Step 1: NO + Cl2 ---> NOCl+ Cl (slow) Step 2: Cl + NO ---> NOCl (fast)
The rate law for the reaction: NH4+ + NO₂ N₂ + 2H₂O is rate =k[NH4+][NO₂] It is found that the rate constant for this reaction is 3.05x10-4 M-1s-1. Calculate the rate of the reaction, including units, if [NH4*] is 0.265M and [NO₂] is 0.0803M. Attach File Browse Local Files
Please answer the question