Chemical Kinetics and Nuclear ChemistryMedium
Question
In a reaction, A + B → Product, rate is doubled when the concentration of B is doubled, and rateincreases by a factor of 8 when the concentrations of both the reactants (A and B) are doubled, ratelaw for the reaction can be written as:
Options
A.Rate = k[A]2 [B]
B.Rate = k[A] [B]2
C.Rate = k[A]2 [B]2
D.Rate = k[A] [B]
Solution
A + B → Product
r1 = [A]x [B]y
r2 = [A]x [2B]y = 2r1 = 2 × [A]x [B]y ⇒ 2y = 2 ⇒ y = 1
r3 = [2A]x [2B]y = 8r1 = 8 × [A]x [B]y
= 2x × 2y = 23 = 2x = 22
Rate = k [A]2 [B]
r1 = [A]x [B]y
r2 = [A]x [2B]y = 2r1 = 2 × [A]x [B]y ⇒ 2y = 2 ⇒ y = 1
r3 = [2A]x [2B]y = 8r1 = 8 × [A]x [B]y
= 2x × 2y = 23 = 2x = 22
Rate = k [A]2 [B]
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