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].

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.

k= rate constant

For the given rate law:

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

b) The reaction is first order overall: False

The overall order is 1+1= 2.

c)  k is the reaction rate constant: True

k= rate constant

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

For the given rate law:

x = 1= order with respect to A

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

For the given rate law:

y =1=  order with respect to B

c, liquids evaporate, creating a gas

i think its 5049.

i hope this !