REACTIONS OF VARIOUS ORDERS7. The kinetic study of decomposition of HI (g) at 700 K is as following:HI(g) -> 1/2 H₂(g) + 1/2 12(g)Time(s)0100200300400Donde[HI] (M)1.000.900.810.740.68ndCorderfirst order 2nIn[HI] 1/[HI](M¹)0-0.105-0.211-0.301-0.386What are the reaction order and the rate constant for the reaction?1.001.111.2351.351.47

7. The kinetic study of decomposition of HI (g) at 700 K is as following: HI(g) > 1/2 H₂(g) + 1/2 12(g) Donde Time 0 100 200 300 400 [HI] (M) 1.00 0.90 0.81 0.74 0.68 first order and order In[HI] 1/[HI](M¹) 0 -0.105 -0.211 -0.301 -0.386 What are the reaction order and the rate constant for the reaction? 1.00 1.11 1.235 1.35 1.47

7. The kinetic study of decomposition of HI (g) at 700 K is as following: HI(g) > 1/2 H₂(g) + 1/2 12(g) Donde Time 0 100 200 300 400 [HI] (M) 1.00 0.90 0.81 0.74 0.68 first order and order In[HI] 1/[HI](M¹) 0 -0.105 -0.211 -0.301 -0.386 What are the reaction order and the rate constant for the reaction? 1.00 1.11 1.235 1.35 1.47

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.35PAE: 11.35 For the reaction 2 NO(g) + 2 H?(g) — N,(g) + 2 H,O(g) at 1100°C, the following data have been...

See similar textbooks

Similar questions

11.35 For the reaction 2 NO(g) + 2 H?(g) — N,(g) + 2 H,O(g) at 1100°C, the following data have been obtained: [NOJ [HJ Rate = A(N2]/At (mol L~1) (mol L_1) (mol L-1 s_1) 5.0 X 10’1 0.32 0.012 1.0 X 10~’ 0.32 0.048 1.0 X 10"2 0.64 0.096 Derive a rate law for the reaction and determine the value of the rate constant.
In Chapter 3, we discussed the conversion of biomass into biofuels. One important area of research associated with biofuels is the identification and development of suitable catalysts to increase the rate at which fuels can be produced. Do a web search to find an article describing biofuel catalysts. Then, write one or two sentences describing the reactions being catalyzed, and identify the catalyst as homogeneous or heterogeneous.
For a first order gas phase reaction A products, k = 7.2 104s1 at 660. K and k = 1.7 102s1 at 720. K. If the initial pressure of A is 536 torr at 295C, how long will it take for the pressure of A to decrease to 268 torr?
One mechanism for the destruction of ozone in the upper atmosphere is a. Which species is a catalyst? b. Which species is an intermediate? c. Ea for the uncatalyzed reaction O3(g)+O(g)2O2(g) is 14.0 kJ. Ea. for the same reaction when catalyzed is 11.9 kJ. What is the ratio of the rate constant for the catalyzed reaction to that for the uncatalyzed reaction at 25C? Assume that the frequency factor A is the same for each reaction.
Can a reaction mechanism ever be proven correct? Can it be proven incorrect?
Azomethane decomposes into nitrogen and ethane at high temperatures according to the following equation: (CH3)2N2(g)N2(g)+C2H6(g)The rate of the reaction is followed by monitoring the disappearance of the purple color due to iodine. The following data are obtained at a certain temperature. (a) By plotting the data, show that the reaction is first-order. (b) From the graph, determine k. (c) Using k, find the time (in hours) that it takes to decrease the concentration to 0.100 M. (d) Calculate the rate of the reaction when [ (CH3)2N2 ]=0.415M.
For the reaction 5Br(aq)+BrO3(aq)+6 H+(aq)3Br2(aq)+3H2O It was found that at a particular instant, bromine was being formed at the rate of 0.029 mol/L s. At that instant, at what rate (a) are the hydrogen ions being consumed? (b) is water being formed? (c) are the bromide ions being consumed?