The activation energy for the decomposition of hydrogen iodide is found to be 180 kJ mol–1...
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?
Homework Answers
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
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