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The decomposition of benzene diazonium chloride (C6H5N2Cl, molar mass = 141 g/mol) at 50 degrees Celsius follows the first order kinetics rate law with the reaction equation: C6H5N2Cl-->C6H5Cl + N2, and has a half-life of 10.8 minutes. Exactly one liter of a solution of 10.0 g/L of benzene diazonium chloride is reacted and the generated nitrogen gas is trapped over water at 22.0 degrees Celsius under a barometric pressure of 743 Torr.
a) Calculate the volume of nitrogen gas that has been released by the reaction after 20.0 minutes
b) Calculate the volume of nitrogen gas that the reaction will release when it is complete, i.e. after infinite time

Solution Preview

half life = t1/2 = 10.8 min
mass left at time t,
m(t) = mo*exp(-k*t)
mo = initial mass = (10.0 g/lit)*1.00lit = 10 g = 10/141 mol
k = 0.69315/t1/2 = 0.69315/10.8 per min

a.) At t = 20 min,
m(20) = 10 *exp(-20*0.69315/10.8) ...

Solution Summary

The answers are given equationally.