Respuesta :
Answer:
1. Â [tex]R=k[A]^1[B]^2[/tex]
2. Â [tex]R=k[B]^1[/tex]
3. Â [tex]R=k[A]^0[B]^0=k[/tex]
4. Â [tex]R=k[A]^1[B]^{-1}[/tex]
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.
(1) is second order in B and overall third order.
2A + B → C
Order of the reaction = sum of stoichiometric coefficient
= x + 2 = 3
x = 1
Rate of the reaction =R
[tex]R=k[A]^1[B]^2[/tex]
(2) is zero order in A and first order in B.
2A + B → C
Rate of the reaction =R
[tex]R=k[A]^0[B]^1=k[B]^1[/tex]
Order of the reaction = sum of stoichiometric coefficient
= 0 + 1 = 1
(3) is zero order in both A and B .
2A + B → C
Order of the reaction = sum of stoichiometric coefficient
= 0 + 0 = 0
Rate of the reaction =R
[tex]R=k[A]^0[B]^0=k[/tex]
(4) is first order in A and overall zero order.
2A + B → C
Order of the reaction = sum of stoichiometric coefficient
= 1 + x = 0
x = -1
Rate of the reaction = R
[tex]R=k[A]^1[B]^{-1}[/tex]
