in your textbook, it states that “…a 10 oC increase in temperature increases the

Question

in your textbook, it states that “…a 10 oC increase in temperature increases the rate of a typical
reaction by two or three times.” Is this the case for the decolorization of CV+? Show your work using 2 of the
average temperatures (from the data table) that differ by about 10 oC.

DATA SHEET PART A: Absolute value of the correlation factor for the graph of A vs. time Absolute value of the correlation factor for graph of InA vs. time Absolute value of the correlation factor for graph of 1/A vs. time Based on your correlation factor cv (p) is equal to the Order in Run 1: Slope of straight line 1332 c A3 2s Temp. (mean) 2.l o Rate constant, k" (give the units) PART B: Complete the following tables: Table -1 Run Tmean, OC Slope (m 2 Team "A" Co. 2 Team "B" 5.3 050244 3 Team "A" 5,3 G, no.050244 3 Team "B" Ll 1.5 Group mean

Explanation / Answer

Arrhenius equation-

lnK=-Ea/R(1/T) +lnA    K=rate constant,T=temperature,Ea=activation energy A=pre-exponential factor

For T=7.50 deg C ,K"=0.06516s-1

for T=17.7 deg C,K"=0.1391s-1

For 10 deg rise in temperature the ratio of rate constant,=0.1391/0.06516=2.13 or 2 (approx)

As reaction rate =K [A]^n where [A]=concentration of reactant,n=order of rxn with respect to A.

So reaction rate is directly proportional to rate constant K ,so it doubles with rate constant

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