'Show all working explaining detailly each stepAnswer Qc(i), (ii) (iii) and (iv) Deine ihe folowing terme nd giye one suitable example in each case.Catalyst:a)Activation energy:Hydrogenationiv)Endothermic reactionAn experiment was carried out to investigate the effect of varying concentration ofhydrachloric acid on the rate of the reaction of the acid with 1g of iron fillings. The acid waspresent in excess The reaction times (1) required for the evolution of 15 cm of hydrogen(measured al one atmosphere and 300K were recorded and are shown in the table below.b)Time, (1/second.160Concentration of HCl moll0.250.350.500,701.0080402010Suggest why a large excess of hydrochloride acid was required.Consider the data in the table. Give a relationship between the time, t. and theconcentration of the hydrochloric acid.What is the order of the reaction with respect to hydrochioric acid.iv)The following are two possibilities for the rate equations, where n is the order of thereaction.Rate = K[H'T"Rate = K[CI]"How would you determine experimentally which of these is the correct expression......

(i) Catalyst - When the Chemical Reaction rate increases or decreases by help of any substance then…

Answered: LDetine ihe following terme nd give one…

LDetine ihe following terme nd give one suitable example in each case. Catalyst: a) Activation energy: Hydrogenation iv) Endothermic reaction

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter13: Chemical Kinetics

Section: Chapter Questions

Problem 13.23QE: Nitrogen monoxide reacts with chlorine to form nitrosyl chloride. NO(g)+12Cl2(g)NOCl(g) The figure...

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11.48 The following data were collected for the decomposition of NT),-: Time, f (min) [N2Os] (mol L-1) 0 0.200 5 0.171 10 0.146 15 0.125 20 0.106 25 0.0909 30 0.0777 35 0.0664 40 0.0570 Use appropriate graphs to determine the rate constant for this reaction. Find the half-life of the reaction.
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The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution. NH/(aq) + NO2-(aq) — N;(g) + 2 H,O(f) INH/I (mol L1) [NO21 (mol L-1, Rate = A[NJ/At (mol L-1 s’) 0.0092 0.098 3.33 X IO"7 0.0092 0.049 1.66 X 10‘7 0.0488 0.196 3.51 X 10"6 0.0249 0.196 1.80 X 10-6 Determine the rate law for this reaction and calculate the rate constant.
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.
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.