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IMG_0004_NEW_0020

# IMG_0004_NEW_0020 - tAI(ii rntegrating ltl'itt"t...

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L\ T.DAY,S LE,CTURE: { .,REACTION KINETICS" The Integrated Rate Law First Order Rate Laws First Order Half Lives Second Order Rate Laws Second Order Half Lives The lntegrated Rate Law . Differential Rate Law How rate changes with concentration . lntegrated Rate Law How concentration changes with time First-order Rate Process . aA+Products e.g. 2N2O5 + 4NO2 + 02 . How does the concentration ofreactants decrease with time from its initial value? lm 2m 300 400 Time (sec) 0.08 z 0.06 .J f o-o+ = l"t Order lntegrated Rate Law aA + products Differential rate law: - ft *rlLa Rate = #=tln| (r) Rearranging,
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Unformatted text preview: tAI (ii) rntegrating,\ ltl 'itt "t J#=-!mt-3.m z ?4.00 hlAl = -frr+krlAlo = Equation for a straight line (y = mx + c) with: y=tn[Al, x=t, m---k, c=ln[A]o dk^ +=o LAI= DAJ" 3 1st Order lntegrated Rate Law O If f and [A]s are known then [A] can calculated for any time. O If ln[A] is plotted against t, the slope is -fr and intercept is ln[A]6 0.10 0.08 9 o.*- 0-M o-u2 0.00 1 Time (sec) 100 2m Time (sec) g Rearranging equation gives time dependence in terms of ratios of concentrations: ,,,[tn], ) = o, [tA],, 4 ln[A]:-h+ln[A]o C= hnh...
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