From given values, Let the rate is of first order
Integrated rate law for first order is:
ln [Ao]/[A] = kt
If after substituting different values, k remains constant for this, then reaction is of first order
So, ln (0.800 / 0.502) = k (10)
k = 0.0466
When ln (0.800 / 0.315) = k(20)
k = 0.0466
ln (0.800 / 0.198) = k(30)
k = 0.0465
ln (0.800 / 0.124) = k(40)
k = 0.0466
Which is almost constant
Hence rate Law = k [HI]
and k = 0.047 min-1
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