Chemical Kinetics and Nuclear ChemistryHard

Question

For the reaction A (g) + 2B(g) → C(g) + D(g) = k [A] [B]2
Initial pressure of A and B are respectively 0.60 atm and 0.80 atm. At a time when pressure of C is 0.20 atm, rate of the reaction, relative to the initial value is :

Options

A.1/6
B.1/48
C.1/4
D.1/24

Solution

Initial Rate = k [A] [B]2
            Rate 1 = k [0.60] [0.80]2            .....(i)
            Rate 2 = k [At] [Bt]|2            .....(ii)
Given Rxn
                  A (g)     +   2 B (g)      →     C (g)     +     D (g)
              0.60 atm        0.80 atm          0           0        t = 0
         (0.60 – 0.2)       (0.80–0.40)          0.20           0.20 atm
             0.40 atm         0.40 atm          0.20 atm    0.20 atm    t = t
Put value of pressure of t = t in rate equation (II)
Rate 2 = k [.40] [.40]2


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