Considering homogeneous reaction conditions in the given batch reactor, which of the given reactants would be consumed first assuming the equal initial concentration of both the re... Considering homogeneous reaction conditions in the given batch reactor, which of the given reactants would be consumed first assuming the equal initial concentration of both the reactants?
Understand the Problem
The question is asking which reactant would be consumed in a homogeneous reaction in a batch reactor, given the rates of change for two reactants A and B. The user needs to determine which of A or B would be consumed first based on their initial concentrations and their rates of consumption.
Answer
B would be consumed first.
Answer for screen readers
Reactant B would be consumed first.
Steps to Solve
- Identify the rates of consumption of reactants A and B
The rates of consumption are given as: $$ \frac{dA}{dt} = 5 \text{ units} $$ $$ \frac{dB}{dt} = 6 \text{ units} $$
- Determine which reactant is consumed faster
Compare the absolute values of the rates of consumption. Since:
- A is consumed at a rate of 5 units per time
- B is consumed at a rate of 6 units per time
- Conclusion on consumption
Since the rate of consumption of B (6 units) is greater than that of A (5 units), reactant B is consumed faster.
Reactant B would be consumed first.
More Information
In a batch reactor, the reactant with the higher rate of consumption will decrease in concentration more quickly than the other reactant. This can affect the overall reaction kinetics and equilibrium.
Tips
- Confusing the rates: Ensure you are comparing the correct values of $dA/dt$ and $dB/dt$.
- Forgetting that higher absolute consumption rate indicates faster depletion.
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