t of the time, the rate of a reaction depends on thecentration of the reactant. In the case of second-orderctions, the rate is proportional to the square of thecentration of the reactant.ect the image to explore the simulation, which will help you toderstand how second-order reactions are identified by theture of their plots. You can also observe the rate law forferent reactions.[HI] moll0.510 15time, 10sPlot [HI] vs timeO Plot In[HI] vs. timeO Plot 1(HI) vs. time2.025concentration, moll2HIRate law: KHIk-64-10°1(mol-s) at 500 KInitial rate-1.6-10 moll-s)281-H₂+1₂StartIn the simulation, you can select one of the three different kinds ofplots. You may use the Start, Stop, and Reset buttons toobronie th tokinds ofkindsing thes forPart BConsider 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 = 5.45x10¹0s ([HI]) for a reaction starting under the condition in the simulation?Express your answer in moles per liters to three significant figures.View Available Hint(s)-Submit196) ΑΣΦΑPart C Complete previous part(s)Part D Complete previous part(s)?molL

Answered: Image /qna-images/answer/bec1fc35-48aa-4e54-a29d-49ee738df640.jpg

kinds of kinds 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=5.45x10¹0s ( [HI],) for a reaction starting under the condition in the simulation? Express your answer in moles per liters to three significant figures. ▸View Available Hint(s) 10 ΑΣΦΑ HI, - ? mol

kinds of kinds 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=5.45x10¹0s ( [HI],) for a reaction starting under the condition in the simulation? Express your answer in moles per liters to three significant figures. ▸View Available Hint(s) 10 ΑΣΦΑ HI, - ? mol

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

The reaction for the formation of phosgene from carbon monoxide and chlorine Co + Cl,COC1, is first order in CO and first order in Cl,. Complete the rate law for this reaction in the box below. Use the form k[A]"B]"... , where '1' is understood for m, n. (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate constant was determined to be 1.85×10-23 M's1. Using this value for the rate constant, the rate of the reaction when [CO] = 0.877 M and [Cl] = 0.119 |Ms!. M would be
D Other Bookmarks [References) Use the References to access important values if needed for this question. The reaction of nitrogen dioxide with fluorine 2 NO2 + F22 NO2F is first order in NO2 and first order in F2. Complete the rate law for this reaction in the box below. Use the form k[A]m[B]"..., where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate constant was determined to be 1.51x10-4 M-15-1 Using this value for the rate constant, the rate of the reaction when [NO2) = 1.95 M and [F2] = 2.97 M would be Ms-1, Submit Answer Try Another Wersion 2 item attempts remaining 7:15 PM 5/5/2022 SONY WEB K DISPLAY OFF One Touch Web Access Without Booting Up Delete F6 Num Lk Ser Lk Prt Sc Sys Ra Insert Pause F4 F7 BIG F12 F5 F8 F9 F10 F11 Break 1& Backspace - Home 6.
What is the total order for a reaction with rate law r= k[A][B]²[C] O A) 4 O B) 2 C) 1 D) 3
Consider the second-order reaction: 2HI(g)→H₂(g) + I2(g) Use the simulation to find the initial concentration [HI]o and the rate constant k for th reaction. What will be the concentration of HI after t = 7.46×1010 s (HI) for a reaction starting under the condition in the simulation? Express your answer in moles per liters to three significant figures. View Available Hint(s) [HI] 11 15. ΑΣΦ STEE ?
The reaction for the formation of phosgene from carbon monoxide and chlorine Co + Cl, → COC, is first order in CO and second order overall. Complete the rate law for this reaction in the box below. Use the form k[A]"B".. , where '1' is understood for m, n .. (don't enter 1) and concentrations taken to the zero power do not appear. Rate =
The reaction for the formation of phosgene from carbon monoxide and chlorine co + Ch → COCH is first order in CO and second order overall. Complete the rate law for this reaction in the box below. Use the form k[A]"B]"... , where '1' is understood for m, n .. (don't enter 1) and concentrations taken to the zero power do not appear. Rate =
Question Asked Sep 22, 2020 3 views The rate of a certain reaction was studied at various temperatures. The table shows temperature (?)(T) and rate constant (?)(k) data collected during the experiments. Plot the data to answer the questions. What is the value of the activation energy, ?aEa , for this reaction? ? (?)T (K) ? (?−1)k (s−1) 400400 0.0001080.000108 420420 0.0006260.000626 440440 0.003100.00310 460460 0.01340.0134 480480 0.05110.0511 500500 0.1750.175 520520 0.5470.547 540540 1.571.57 560560 4.184.18 580580 10.410.4 ?a=Ea= kJ⋅mol−1kJ⋅mol−1 What is the value of the pre‑exponential factor (sometimes called the frequency factor), ?A , for this reaction? ?=A= s−1 check_circle Expert Answer thumb_up thumb_down Step 1 Given- Table for temperature and rate constant values T (K) k (s−1) 400 0.000108 420 0.000626 440 0.00310 460 0.0134 480 0.0511 500 0.175 520 0.547 540 1.57 560…
Current Attempt in Progress The reaction of sucrose with water is first order with respect to sucrose. The rate constant under the conditions of the experiments is 6.17 x 104 s 1. Correct. Calculate the value of t1/2 for this reaction in minutes. t1/2 = 18.7 minutes. Hint Incorrect. How many minutes would it take for 0.937 parts of the sucrose to react? t = i minutes. Hint
The reduction of nitric oxide with hydrogen 2NO+2H₂ → N₂ + 2H₂O is second order in NO and first order in H₂. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m, n... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate of the reaction was determined to be 0.0608 M-s¹, when [NO] = 0.498 M and [H₂] = 0.137 M. From this experiment, the rate constant is M-². s-¹.
O d. the rate law is: rate = k [12][H₂014 e. the reaction fourth order overall QUESTION 3 Consider the following reaction for the formation of NO: N2(g) + O2(g) --> 2NO(g) the average rate of disappearance of N2 over the period from t = 0 tot = 0.100 s is found to be 5.00 x 10-1 mol/L-s. What is the rate of appearance of NO over the same period? O a. 5.00 x 10-1 mol/L-s O b. 1.00 mol/L-s O c. 5.00 mol/L-s O d. 2.50 x 10-1 mol/L-s O e. 10.0 mol/L-s QUESTION 4 Consider the following hypothetical reaction: Click Save and Submit to save and submit. Click Save All Answers to save all answers. 2.5 Save All Answe
Determine the overall rate law for the reaction CH3Br(aq) + OH (aq) → CH3OH(aq) + Br (aq). The data is given below Experiment [CH3B1] (M) [OH"] (M) Initial rate (M/s) k[CH3B1][OH¯]³ O k[CH3B1]°[OH73 1 0.12 0.12 5.2 x 10-5 O k[CH3B1]?[OH"7² 2 0.24 0.12 1.04 x 10-4 O k 3 0.12 0.06 6.5 x 10-6 O KỊCH3B1]°[OH"]) O k(CH3B1]?[OH"]
Don't provide handwitten solution please...