Question 5 Not answered Marked out of The decomposition of formic acid (see belo

Question

Question 5 Not answered Marked out of The decomposition of formic acid (see below) is measured at several termperatures HCOOH(g) CO2(g) + H2(g) The temperature dependence of the first-order rate constant is: 1.00 uestion 800 0.00027 825 8.88849 850 0.08086 875 .00143 900 .80234 925 0.00372 Calculate the activation energy, in k/mol. 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

Arrhenius equation

ln(K2/k1) = Ea/R[1/T1 - 1/T2]

k1 = 0.00027s-1 , T1 = 800 k

k2 = 0.00049s-1 , T2 = 825 k

Ea = ? kj/mol , R = 8.314*10^-3 j.k-1.mol-1

ln(0.00049/0.00027) = (x/(8.314*10^-3)((1/800)-(1/825))

Ea = activation energy = 130.8 kj/mol

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