# Use Arrhenius equation k = A e Ea/RT to calculate rate of reaction and rate constant

2) Given that:

rate = k[N_{2}O_{5}]^{2}

A = 6 x 10^{23} L.mol^{-1}.s^{-1}

Ea = 250 kJ.mol^{-1}

R = 8.314 J.mol^{-1}.K^{-1}

Use the Arrhenius equation to calculate the rate constant (k) and hence a value for the rate of reaction when [N_{2}O_{5 }] = 0.32 mol.L^{-1} at a temperature of 320 ^{o}C.

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k = A e

^{Ea/RT}Ea and R should have the same energy units so that they cancel so convert Ea from Kj to J.

Ea = 250 x 10

^{3}J.mol-1 or (250 E3)Also temperature must be in Kelvin so 320C = 393 K.

Now plug in

k = 6 x 1023 mol/L sec x e

^{ (250 E3 / (8.314 J/mol K) x 593 K))}Once you have found the value for k you can plug into the rate law

Rate = k[N

_{2}O_{5}]^{2 }and find the Rate.spock

Sun, 2012-02-12 08:52