The activation energy for the decomposition of hydrogen iodide is found to be 180 kJ mol–1 and the rate constant for this reaction is reported to be 0.24 mol–1 L min–1at 540 °C. What is k for this reaction at 30 °C?
ln(k2/k1) = Ea/R[1/T1 - 1/T2]
K1 = ? T1 = 30 c = 303 k
K2 = 0.24 T2 = 540 c = 813 k
Ea = 180 kj/mol , R = 8.314 j.k-1.mol-1
ln(0.24/k1) = (180*10^3/8.314)((1/303)-(1/813))
K1 = rate constant at 30 c = 8.2*10^-21
The activation energy for the decomposition of hydrogen iodide is found to be 180 kJ mol–1...
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