Decomposition of Hydroiodic Acid into Hydrogen and Iodine
$5.50$3.502226 reads
Question
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?
Summary
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.
Related Solutions
Calculate Concentration of Four Forms of HistidineCombusting Butane Gas And Calculating Composition Of Flue Gas StrDetermining Overall Mass Transfer Coefficient for Gas PhaseRedlich-Kwong Equation for Ideal Gas AssumptionCalculate Power Requirement For A PumpCalculate the Rate of Flow of Vapor and Liquid Composition of Met
Recently Uploaded Solutions
Write an Essay on the Importance of Public RelationsWrite an essay on the positive impact of shareholder power on bonWrite An Essay On What You Want From Work And How To Achieve ItWrite an essay/report on Marketing Mix OrientationWrite an interview structure about poultry litter convert to bio Write Article Reflection On The Article “Improving Teaching And
Most Downloaded Solutions