Question #191716

Hydrogen Iodide (HI) gas decomposes into gaseous hydrogen and iodine following the second-order kinetics with a rate constant of 0.031/M.s at 400ºC.

2HI(g) H2(g) + I2(g)

a.What is the half-life of the reaction if the initial concentration of HI is 0.045 M? Will the half-life be different if the initial concentration is 0.025 M? Justify your answer.

b.How much HI (in M) remains after 5.0 Minutes if the reaction started with 0.024 M HI?

c.How many minutes will it take for the concentration of HI to decrease from 0.045 M to 0.015 M?

Expert's answer

**A. **Half life of second order

Now when M

Half time seconds

Now when M

Half time seconds

Here half time changes as the half time is inversely proportional to the initial conc.

B. Now for the second order reaction we know that

** **

where t=5 minutes=300 seconds

Intial conc.=0.024 M

Rate constant=0.031

Now put in the equation

C. Again putting the values in the formula

seconds or minutes approximately..

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