102-Manual.pdf C ars-chemia net Manual.pdf QUESTIONS FOR CHEMICAL KINETICS EXP N

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102-Manual.pdf C ars-chemia net Manual.pdf QUESTIONS FOR CHEMICAL KINETICS EXP NAME 1. The reaction 2 NO,al Cl 2 NOCl has been studied and found to be second order with respect to nitrogen monoxide andfirst order with respect to chlorine. a. What is the overall order for the reaction? b. How does the reaction rate change when the nitrogen monoxide concentration is halved and the chlorine concentration is doubled? Define terms (e.g., [NO] for initial concentration in experiment NO12 for initial concentration inexperiment 2,[NO]2 V2 [NOJ), set up the rate law ratios and show cancellations forExp2. Exp1 2. The initial rate of a reaction is found to increase by a factor of sixteen when the concentration of one reagent is doubled while all other reagent concentrations are held constant. What is the order of the reaction with respect to that one reagent? Define terms, set up the rate law ratios and show cancellations for Exp2. 3. At 593K a particular decomposition's rate constant had a value of 2.88x1o 4 and at 673K. the same reaction's rate constant was 1.94x1013. It was noticed that when the reactant's initial concentration was o.1250 M (with a 593K reaction temperature), the initial reaction rate was identical to the initial rate when the decomposition was run at 673K with an initial reactant concentration of o.o4816 M. Recall that rate laws have the form rate- k[AF and, showing work, determine the order ofthe decomposition reaction. 10:51 PM 5/4/2017

Explanation / Answer

1. a.)               2NO(g) + Cl2 (g) -------> 2NOCl (g)

                       Acoording to rate law : rate = k[NO]x[Cl2]y

                                                    x= 2 in NO and y = 1 in Cl2

                                                   order of reaction = x+y

                                                                           = 2+1 =3

                                               so its a third order reaction .

b. if the initial concentration of [NO]1 = x, intitial concentration of [Cl2]1 = y for experiment 1.

      Now the initial concentration of [NO]2 = 1/2 of [NO]1 for experment 2

                                                   [NO]2 = x/2,

and intitial concentration of [Cl2]2 = 2 [Cl2]1

                                         then [Cl2 ]2 = 2y for experiment 2

                                                 rate = k [NO]2[Cl2]

                               rate for experiment 1 rate =k x2.y

                                            rate for experiment 2 rate = k x2/22 . 2y

ratios of rate of experiment 2 and experiment 1 = ( k x2/22 . 2y)/(k x2.y)

                                                     exp2/ exp1 = 1/2

please raise another question for remaning part of the question as per chegg policy

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