What will be the initial rate of a reaction if its rate constant is 10^-3 min^-1. and the concentration of
reactant is 0.2 mol dm^-3. How much of reactant will be converted into products in 200 min
a) 2 x 10^-4M min^-1, 18%
b) 10^-4M min^-1, 16%
c) 10^-3M min^-1, 18%
d) 10^-3M min^-1, 17%
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Answer:
Rate =K×[A]
=10−3×0.2=2×10−3moldm−3min−1
200=10−32.303log(0.2−x0.2)
0.244−1.22x=0.2
x=0.036moldm−3