Question
In a reaction, A+B → Product, rate is doubled when the concentration of B is doubled, and rate increases by a factor of 8 when the concentrations of both the reactants (A and B) are doubled. Rate law for the reaction can be written as
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Rate = k[A][B]2
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Rate = k[A]2[B]2
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Rate = k[A][B]
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Rate k[A]2[B]
Solution
D.
Rate k[A]2[B]
Let the order of reaction with respect to A and B is x and y respectively. so, the rate law can be given as,
R= k[A]x[B]y ......(i)
When the concentration of the only B is doubled, the rate is doubled, so
R1 = k[A]x[2B]y = 2R ....(ii)
If concentrations of both the reactants A and B are doubled, the rate increases by a factor of 8, so
R" = k[2A]x[2B]y = 8R (iii)
k2x2y[A]x[B]y = 8R (iv)
from equation (i) and (ii), we get
If concentrations of both the reactants A and B are doubled, the rate increases by a factor of 8, so
R" = k[2A]x[2B]y = 8R (iii)
k2x2y[A]x[B]y = 8R (iv)
from equation (i) and (ii), we get
