Chemical Kinetics and Nuclear ChemistryHard
Question
Zn + 2 H+ → Zn2+ + H2
Half-life period is independent of concentration of zinc at constant pH. For the constant concentration of Zn, rate becomes 100 times when pH is decreased from 3 to 2. Hence ,
Half-life period is independent of concentration of zinc at constant pH. For the constant concentration of Zn, rate becomes 100 times when pH is decreased from 3 to 2. Hence ,
Options
A.
= k [Zn]0[H+]2
= k [Zn]0[H+]2B.
= k [Zn][H+]2
= k [Zn][H+]2C.rate is not affected if concentration of zinc is made four times and that of H+ ion is halved
D.rate becomes four times if concentration of H+ ion is doubled at constant Zn concentration
Solution
(B) Half life period independent of conc. of Zn than order W.R.T. Zn is 1st
Rate = k [Zn][H+]n we can write
by data
Given n = 2
Then Rate = k [Zn][H+]2
(C) Conc. of Zn four times and H+ ion is halved
Rate = k[4 × Zn]
Rate = k [Zn][H+]2
Rate remians and same.
(D) Similarly if conc. of H+ doubled and [Zn] constant
Then Rate2 = k [Zn] [2H+]2
Rate2 = 4 k [Zn] [H+]2
Rate2 = 4 x Rate1
Rate = k [Zn][H+]n we can write
by data
Given n = 2
Then Rate = k [Zn][H+]2
(C) Conc. of Zn four times and H+ ion is halved
Rate = k[4 × Zn]
Rate = k [Zn][H+]2
Rate remians and same.
(D) Similarly if conc. of H+ doubled and [Zn] constant
Then Rate2 = k [Zn] [2H+]2
Rate2 = 4 k [Zn] [H+]2
Rate2 = 4 x Rate1
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