Question

The rate law for a reaction is rate=k[A][B] Which one of the following statements is false? The rate law for a reaction is Which one of the following statements is false? If [A] is doubled, the reaction rate will increase by a factor of 2. The reaction is first order overall. k is the reaction rate constant. The reaction is first order in [B]. The reaction is first order in [A].

Answer 1

Answer: The reaction is first order overall.

Explanation: Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

$Rate=k[A]^x[B]^y$

k= rate constant

For the given rate law:

$Rate=k[A]^1[B]^1$

x = 1= order with respect to A

y =1=  order with respect to B

n =( x+y)= (1+1) = 2 = Total order

a)  If [A] is doubled, the reaction rate will increase by a factor of 2: True

$Rate'=k[2A]^1[B]^1$

$Rate'=k[2]^1[A]^1[B]^1$

$Rate'=[2]^1\times Rate$

$Rate'=[2]\times Rate$

b) The reaction is first order overall: False

The overall order is 1+1= 2.

c)  k is the reaction rate constant: True

$Rate=k[A]^x[B]^y$

k= rate constant

d) The reaction is first order in [B]: True

For the given rate law:

$Rate=k[A]^1[B]^1$

x = 1= order with respect to A

e) The reaction is first order in [A]: True

For the given rate law:

$Rate=k[A]^1[B]^1$

y =1=  order with respect to B