Experiment 7: Rate Law for the Reaction of Crystal Violet and Hydroxide Prelab P

Question

Experiment 7: Rate Law for the Reaction of Crystal Violet and Hydroxide Prelab Practice Assignment Nitrous oxide, N2O, undergoe the following stoichiometry: s decomposition on a gold surface at 900 °C, obeying 1. 2N2O(g) >2N2()+02(8). The concentration of the reactant was monitored as a function of time In(N2O) vs. t gave the graph shown below. The trendline is printed on the box, with y In(N2O) and x t. The correlation coefficient is r--vR"--09995, for a nearly perfect . A graph of anticorrelation -2 y=-1.288 E 02x-2.291E+00 R1 9.990E-01 2.5 -3 -3.5 20 40 60 80 100 120 140 time (min) a. What is the reaction order according to the above results? b. What are the units of the rate constant? C. What is the numerical value of the rate constant? k = d. What is the half-life for the reaction? t1/2 e. What was the initial molarity of the reactant? (N2O)

Explanation / Answer

a) Since ln [N2O] V/s TIME gives straight line it is a first order reaction with rate equation

ln[N2O] = -kt + ln[N2O0]

b) rate constant = rate / (concentration)1

k = min-1

c) slope = -k = -1.288E-02

k = 0.0128 min-1

d) t(1/2)=0.693/k = 0.693 / 0.0128 = 54.14 min

e) intercept = ln[N2O0] = -2.291

[N2O0] = 0.1011 M

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