Reaction Kinetics : Half-Life and the Arrhenius Equation
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Knowing the rate constant is 3.46 X 10^-5 s^ at 298 and that energy activation is 1.60 x 10^5 J-mol ^-1. Determine the temperature at which the half life for the 1st order decomposition of dinitrogen pentoxide in carbon tetrachloride to dinitrogen tetroxide and oxygen is 2 hours.
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Solution Summary
Knowing the rate constant is 3.46 X 10^-5 s^ at 298 and that energy activation is 1.60 x 10^5 J-mol ^-1. Determine the temperature at which the half life for the 1st order decomposition of dinitrogen pentoxide in carbon tetrachloride to dinitrogen tetroxide and oxygen is 2 hours.
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half-life = ln(2)/k for a 1st order reaction so: ln(2)/3.46 X 10^-5 = 5.56 hours at 298
we want 2 hours: 2 x 60 x 60 = 7200 seconds
7200 = ln(2)/k
so we want k = 0.00009627 = 9.63 x 10^-5
A = 3.8357x10^23 worked ...
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