The decomposition of formic acid (see below) is measured at several temperatures

Question

The decomposition of formic acid (see below) is measured at several temperatures. HCOOH(g) ? CO2(g) +H2(g) The temperature dependence of the first-order rate constant is: T(K) . . . . k(s-1) 800 ....0.00027 825 ....0.00049 850 ....0.00086 875 ....0.00143 900 ....0.00234 925 ....0.00372 1. Calculate the activation energy, in kJ/mol. 2. Calculate the pre-exponential term (in s -1). Use all data points and do a linear regression using calculator or Excel. Do not pick 2 data points. This is less accurate and assumes all data points are equally qood.

Explanation / Answer

ln k= ln k0- ?Ea/(RT) With y= ln k x= 1/ T one gets a line y=mx+b with m=?Ea/R and b= ln k0. -> ?Ea=R*m and k0= e^b The result is y= 15373.4(1/T) - 11.0091. The correlation is r=-0.999 and that is a straight line. ->?Ea= 127.81 KJ/mol and k0= 6.042*10^4 1/s

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