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:
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]?
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Reaction Mechanism concept. If you need more Reaction Mechanism practice, you can also practice Reaction Mechanism practice problems.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.