Theoretical Background: In chemical reactions, the rate at which a reaction proceeds is determined by the reaction mechanism and the concentrations of the reactants. The rate-determining step is the slowest step in the mechanism and limits the overall rate of the reaction. This concept is crucial in understanding the kinetics of chemical reactions. Consider the following hypothetical reaction: A + B → C + D. The reaction mechanism consists of three elementary steps: Step 1: A + B → E (fast) Step 2: E → F (slow) Step 3: F → C + D (fast) Assuming the rate-determining step is Step 2, answer the following question: Question: How would the rate of the reaction be affected by the following changes: (a) Doubling the concentration of reactant A while keeping the concentration of reactant B constant. (b) Increasing the concentration of reactant B by a factor of four while keeping the concentration of reactant A constant. (c) Decreasing the concentration of reactant A by a factor of two and decreasing the concentration of reactant B by a factor of three simultaneously.
Question:
Theoretical Background: In chemical
Consider the following hypothetical reaction: A + B → C + D. The reaction mechanism consists of three elementary steps:
Step 1: A + B → E (fast)
Step 2: E → F (slow)
Step 3: F → C + D (fast)
Assuming the rate-determining step is Step 2, answer the following question:
Question: How would the rate of the reaction be affected by the following changes:
(a) Doubling the concentration of reactant A while keeping the concentration of reactant B constant.
(b) Increasing the concentration of reactant B by a factor of four while keeping the concentration of reactant A constant.
(c) Decreasing the concentration of reactant A by a factor of two and decreasing the concentration of reactant B by a factor of three simultaneously.
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