# Problem: The proposed mechanism for a reaction is(1) A(g) + B(g) ⇌ X(g)       [fast](2) X(g) + C(g) ⟶Y(g)      [slow](3) Y(g) ⟶ D(g)                [fast](d) Is the mechanism consistent with the actual rate law: Rate = k[A][B][C]?

###### FREE Expert Solution

We’re being asked to determine if the mechanism is consistent with the actual rate law: Rate = k[A][B][C].

When a reaction mechanism is given, the rate law can be determined using the slow step in the reaction mechanism.

rate law only involves the reactants
▪ the coefficients of the reactants in the slow step are the order of the reaction with respect to that reactant
▪ Rate Law has a general form of:

k = rate constant
X & Y = reactants
a & b = reactant orders

We're given the reaction mechanism:

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###### Problem Details

The proposed mechanism for a reaction is

(1) A(g) + B(g) ⇌ X(g)       [fast]
(2) X(g) + C(g) ⟶Y(g)      [slow]
(3) Y(g) ⟶ D(g)                [fast]

(d) Is the mechanism consistent with the actual rate law: Rate = k[A][B][C]?