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 :
= 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
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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