1.

At elevated temperature, HI decomposes according to the chemical equations: 2HI(g) to H_(2)(g) + I_(2)(g) a)Determine (i) the order of reaction and (iii) Write the rate expression. b) Calculate the rate constant and give its units.

Answer»


Solution :From this data, it is QUITE evident that when (HI) is increased from 0.005 to 0.01 (made twice),
rate = `(30 xx 10^(-4))/(7.5 xx 10^(-4)) =4`
When (HI) is increased from 0.01 to 0.02 (made twice),
rate `= (12 xx 10^(-3))/(3 xx 10^(-3)) =4`
a) `therefore` ORDER of reaction=2
Rate expression, (r)=`k[HI]^(2)`
b) Calculation of rate constant:
For EXPT. (1), `k(0.005 mol L^(-1))^(2)=(7.5 xx 10^(-4)mol^(-1)s^(-1)`
`k=(7.5 xx 10^(-4) mol L^(-1)s^(-1))/(2.5 xx 10^(-5)mol^(2)L^(-2))=30 mol^(-1)Ls^(-1)`.


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