The decomposition of HI (Hydroiodic acid) to H2 + I2 at 508°C has a half-life of 135 min when the initial pressure of HI is 0.1 atm and 13.5 min when the pressure is 1 atm. (A) Show that this proves that the reaction is second order. (B) What is the value of the rate constant in L mol-1s-1? (C) What is the value of the rate constant in bar-1s-1? (D) What is the value of the rate constant in cm3s-1?
The question belongs to Chemical Engineering and it is about decomposition of hydroiodic acid to hydrogen and iodine at 508°C with a half time of 135 min. Questions like proving second order reaction, value of rate of constant in mole, bar and cm have been given.
Note: The solution is in handwritten format.
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