View PoliciesCurrent Attempt in ProgressConsider the reaction,CH3CI(g) + 3CI2(g) → CCI4(g) + 3HCI(g)(a) Express the rate of reaction with respect to each of the reactants and products.d[CH,C1]= -31 d[Cl,]_ d[cC,I1 ɖ[HCl]3%3Ddtdtdtdt(CH,CI] = [C1,1 = [cci,I = [HC1]O dICH,CI]1 d[Cl,] -dlcc,I1 ɖ[HCl]_dtdt3dtdt3d[Cl,]dtdtd[HCl]dtdt= -3= 3d[CH,C1](b) If the instantaneous rate of the reaction with respect to HCI is 0.035 M-s-1, what is the instantaneous rate of the reaction withrespect to CCI4?iM.s 1eTextbook and MediaGO TutorialSave for LaterAttempts: 0 of 15 usedSubmit AnswerA O S

Answered: Image /qna-images/answer/55822dc8-0d90-4207-8a29-6c24dbe13680.jpg

View Policies Current Attempt in Progress Consider the reaction, CH3CI(g) + 3Cl2lg) →CCI4(3) + 3HCI(g) (a) Express the rate of reaction with respect to each of the reactants and products. d[CH,C1] dt 1 d[Cl,]_ d[CCl,] _ 1 d[HCl] dt dt dt (CH,C1] = [Cl,1'= [cciI = [HC1] d[CH,C1] %3D 1 d[Cl] _ -d[CCı,I 1 ɖ[HCl]_ dt 3 dt dt dt dt d[Cl,] d[HCI] dt dt -3 d[CH,C1] = 3 d[CC1, dt (b) If the instantaneous rate of the reaction with respect to HCl is 0.035 M-s 1, what is the instantaneous rate of the reaction with respect to CCI4? i M:s 1 eTextbook and Media GO Tutorial Save for Later Attempts: 0 of 15 used Submit Answer

View Policies Current Attempt in Progress Consider the reaction, CH3CI(g) + 3Cl2lg) →CCI4(3) + 3HCI(g) (a) Express the rate of reaction with respect to each of the reactants and products. d[CH,C1] dt 1 d[Cl,]_ d[CCl,] _ 1 d[HCl] dt dt dt (CH,C1] = [Cl,1'= [cciI = [HC1] d[CH,C1] %3D 1 d[Cl] _ -d[CCı,I 1 ɖ[HCl]_ dt 3 dt dt dt dt d[Cl,] d[HCI] dt dt -3 d[CH,C1] = 3 d[CC1, dt (b) If the instantaneous rate of the reaction with respect to HCl is 0.035 M-s 1, what is the instantaneous rate of the reaction with respect to CCI4? i M:s 1 eTextbook and Media GO Tutorial Save for Later Attempts: 0 of 15 used Submit Answer

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter11: Rate Of Reaction

Section: Chapter Questions

Problem 9QAP: Experimental data are listed for the following hypothetical reaction: A+Bproducts (a) Plot these...

See similar textbooks

Similar questions

11.41 For a drug to be effective in treating an illness, its levels in the bloodstream must be maintained for a period of time. One way to measure the level of a drug in the body is to measure its rate of appearance in the urine. The rate of excretion of penicillin is first order, with a half-life of about 30 min. If a person receives an injection of 25 mg of penicillin at t = 0, how much penicillin remains in the body after 3 hours?
Consider the following hypothetical reaction: 2AB2(g)A2(g)+2B2(g)A 500.0-mL flask is filled with 0.384 mol of AB2. The appearance of A2 is monitored at timed intervals. Assume that temperature and volume are kept constant. The data obtained are shown in the table below. (a) Make a similar table for the disappearance of AB2. (b) What is the average rate of disappearance of AB2 over the second and third 10-minute intervals? (c) What is the average rate of appearance of A2 between t=30 and t=50?
What is the difference between average rate, initial rate, and instantaneous rate?
Experimental data are listed for the following hypothetical reaction: A+Bproducts (a) Plot these data as in Figure 11.3. (b) Draw a tangent to the curve to find the instantaneous rate at 60 seconds. (c) Find the average rate over the 20 to 80 second interval. (d) Compare the instantaneous rate at 60 seconds with the average rate over the 60-second interval.
At low temperatures, the rate law for the reaction CO(g)+NO2(g)CO2(g)+NO(g)is as follows: rate=(constant)[ NO2 ]2. Which of the following mechanisms is consistent with the rate law? (a) CO+NO2CO2+NO(b) 2NO2N2O4(fast) N2O4+2CO2CO2+2NO(slow) (c) 2NO2NO3+NO(slow) NO3+CONO2+CO2(fast) (d) 2NO22NO+O2(slow) O2+2CO2CO2(fast)
For a certain reaction, Ea is 135 kJ and H=45 kJ. In the presence of a catalyst, the activation energy is 39% of that for the uncatalyzed reaction. Draw a diagram similar to Figure 11.14 but instead of showing two activated complexes (two humps) show only one activated complex (i.e., only one hump) for the reaction. What is the activation energy of the uncatalyzed reverse reaction?
The rate of the reaction O(g)+NO2(g)NO(g)+O2(g) was studied at a certain temperature. a. In one experiment, NO2 was in large excess, at a concentration of 1.0 1013 molecules/cm3 with the following data collected: Time(s) [O](atoms/cm3) 0 5.0 109 1.0 102 1.9 109 2.0 102 6.8 108 3.0 102 2.5 108 What is the order of the reaction with respect to oxygen atoms? b. The reaction is known to be first order with respect to NO2 Determine the overall rate law and the value of the rate constant.
In the PhET Reactions under Options. (a) Leave the Initial Temperature at the default setting. Observe the reaction. Is the rate of reaction fast or slow? (b) Click Pause" and then Reset All, and then enter 15 molecules of A and 10 molecules of BC once again. Select Show Bonds" under Options. This time, increase the initial temperature until, on the graph, the total average energy line is completely above the potential energy curve. Describe what happens to the reaction.
Consider the following statements: In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get warmed up. After that, however, the rate of the reaction decreases because its rate is dependent on the concentrations of the reactants, and these are decreasing. Indicate everything that is correct in these statements, and indicate everything that is incorrect. Correct the incorrect statements and explain.
Nitrogen monoxide reacts with chlorine to form nitrosyl chloride. NO(g)+12Cl2(g)NOCl(g) The figure shows the increase in nitrosyl chloride concentration under appropriate experimental conditions. The concentration of nitrosyl chloride actually starts at zero, although this fact may be difficult to see in the figure. (a) Write an expression for the rate of reaction in terms of a changing concentration. (b) Calculate the average rate of reaction between 40 and 120 seconds. (c) Calculate the instantaneous rate of reaction after 80 seconds. (d) Calculate the instantaneous rate of consumption of chlorine 60 seconds after the start of the reaction.
The rate of the decomposition of hydrogen peroxide, H2O2, depends on the concentration of iodide ion present. The rate of decomposition was measured at constant temperature and pressure for various concentrations of H2O2and of KI. The data appear below. Determine the order of reaction for each substance, write the rate law, and evaluate the rate constant. Rate [H2OJ [Kll (mL min-’) (mol L ’) (mol L ’) 0.090 0.15 0.033 0.178 0.30 0.033 0.184 0.15 0.066
The plot below shows the number of collisions with a particular energy for two different temperatures. a. Which is greater, T2 or T1? How can you tell? b. What does this plot tell us about the temperature of the rate of a chemical reaction? Explain your answer.