Question

A reaction in which a, b, and c react to form products is zero order in a, one-half order in b, and second order in

c. by what factor does the reaction rate change if the concentration of a is doubled? 1 by what factor does the reaction rate change if the concentration of b is doubled? 1.4 by what factor does the reaction rate change if the concentration of c is doubled? 4

Answer 1

Answer: a) 1

b) 1.414

c) 4

Step-by-step 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.

`A+B+C\rightarrow products`

`Rate=k[A]^0[B]^(1)/(2)[C]^2`

a)
`Rate^'=k[2A]^0[B]^(1)/(2)[C]^2`

`Rate^'=k[2]^0[A]^0[B]^(1)/(2)[C]^2`

`Rate^'=1* Rate`

b)
`Rate^'=k[A]^0[2B]^(1)/(2)[C]^2`

`Rate^'=k[A]^0[2]^(1)/(2)[B]^(1)/(2)[C]^2`

`Rate^'=[2]^(1)/(2)Rate`

`Rate^'=1.414* Rate`

c)
`Rate^'=k[A]^0[B]^(1)/(2)[2C]^2`

`Rate^'=k[A]^0[B]^(1)/(2)[2]^2[C]^2`

`Rate^'=[2]^2Rate`

`Rate^'=4* Rate`