Chemical Reaction Mechanisms
Chemistry ⇒ Chemical Reactions and Equations
Chemical Reaction Mechanisms starts at 11 and continues till grade 12.
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A reaction mechanism consists of the following steps: Step 1: A + B → C (slow), Step 2: C + D → E (fast). What is the rate law for this reaction?
A reaction proceeds via the following steps: Step 1: A + B → C (slow), Step 2: C + D → E (fast). If the concentration of D is doubled, what happens to the rate of the reaction?
Define the term 'intermediate' in the context of a reaction mechanism.
Describe the difference between a reaction intermediate and a transition state.
Describe the role of activation energy in a reaction mechanism.
Describe what is meant by a 'bimolecular' elementary step.
Explain the difference between a catalyst and an intermediate in a reaction mechanism.
Explain why a proposed mechanism must be consistent with both the overall balanced equation and the experimentally determined rate law.
Explain why termolecular elementary steps are rare.
Explain why the rate law for a reaction is determined experimentally and not from the overall balanced equation.
In a proposed mechanism, the first step is fast and reversible, and the second step is slow. Which step is likely to be the rate-determining step?
In a reaction mechanism, what is meant by the term 'molecularity'?
In a two-step reaction mechanism, if the first step is slow and the second is fast, which step determines the rate of the overall reaction?
In the following mechanism, identify the intermediate: Step 1: NO2 + F2 → NO2F + F, Step 2: NO2 + F → NO2F
The reaction 2NO + O2 → 2NO2 is proposed to occur via the following steps: Step 1: 2NO ⇌ N2O2 (fast), Step 2: N2O2 + O2 → 2NO2 (slow). What is the intermediate?
What is a reaction mechanism in chemistry?
