According to arrhenius equation
K = Koe-EA/RT
K = rate constant
T = temperature
EA = activation energy
for 2 different temperature ,the equation can be rearranged as:
ln(K2/K1) = EA/R[1/T1 - 1/T2]
ln{1.2 x 10-3/4.1 x 10-4 } = 10100J/mol / 8.314J/mol.K[1/593K - 1/T2]
T2 = 1246.48 K
b)
3oC = 273 + 3 = 276K
10 oC increment = 276 + 10 = 286K
ln(r2/r1) = EA/8.314J/mol.K[1/276K - 1/286K] given r2 = 10 r1
ln10 x 8.314 /[1/276K - 1/286K] = EA
151112.65 J/mol = 151.113 kJ/mol = EA
Please answer questions 1 and 2 on The rate constant for the reaction answered A +...
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