CALCULATIONS FOR PART 1-B: Table 1.2: The Effect of Concentration on the Rate of

Question

CALCULATIONS FOR PART 1-B: Table 1.2: The Effect of Concentration on the Rate of Reaction. Solution Concentration Average Run Solution(M) 1/IR InR Time (s) Stock 30.S -S.44-0.18 O.o 0.123 CALCULATIONS AND OBSERVATIONS FOR PART 2: 5) Complete the following table of observations: Table 1.3: The Relationship between Temperature and the Rate of Reaction. Molar concentration of solution E: 0-09 e5 TimeRun Rate Temperature (hh:mm:ss) Time Rate constant In k) 1/T (Ktart nd() 6:64t G. lwa 6:/6:So·yo 0. 0143 |-y-250.00337 3tS ocooBus 10.0250-3.67 o.oo328 53 | 32lo o wo86wb 2SD-3.67 | o.oo 30 NOTE: Rate = IRL / ine Co3

Explanation / Answer

R= K[A]n

taking ln

lnR= lnK+n lnA

so the plot of lnR vs lnA gives intercept of lnK and slope of order, n. The plot is not in good agreement showing low R2 value.

the plot is shown below

The slope is n= -1.87 and intercept lnK= 1.834 and K= 6.3

Rate constant

lnK= lnKo-Ea/RT

so a plot of ln K Vs 1/T shouod give a straight line whose slope is -Ea/R and intercept is lnKo.

the slope is Ea/R= 7.050 E= 7.050*8.314=58.6137 Joules/mole and lnKo= 944.6, The data needs to be verified.

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