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?

Please show all workings

Solutions

Expert Solution

Ea = 180Kj/mole

= 180000J/mole

K1 =

K2 =0.24mole/min

T1 = 30C⁰ = 30+273 = 303K

T2 = 540⁰C = 540+273 = 813K

logK2/K1 = Ea/2.303R [1/T1 -1/T2]

log0.24/K1 = 180000/2.303*8.314 [1/303-1/813]

log0.24/K1 = 9400.88(0.0033-0.00123)

log0.24/K1 = 19.459

0.24/K1 = 10^19.459

0.24/K1 = 2.87*10^19

K1 = 0.24/2.87*10^19 = 8.36*10^-21mole/min

queen_honey_blossom answered 2 years ago

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