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Chapter 1: Problem 15

If zero order kinetics are followed, allowing the reaction to run twice the time will: a. cause the product to be denatured b. halve the amount of product formed c. have no effect on the amount of product formed d. double the amount of product formed e. double the absorbance change per minute

Short Answer

Expert verified
d. double the amount of product formed

Step by step solution

01

- Understanding Zero Order Kinetics

In zero order kinetics, the rate of reaction is constant and independent of the concentration of the reactants. The rate law can be written as: \(\text{Rate} = k\), where k is the rate constant.
02

- Calculating Product Formation

Since the rate is constant, the amount of product formed, [P], is directly proportional to the time, t, given as \([P] = kt \).
03

- Analyzing the Effect of Doubling the Time

If the time is doubled, the new time becomes 2t. The amount of product now will be \([P] = k(2t) = 2kt\). This shows that doubling the time will double the amount of product formed.
04

- Conclusion and Answer Selection

From the analysis, doubling the time in a reaction following zero order kinetics results in doubling the amount of product formed. Therefore, the correct answer is: d. double the amount of product formed.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

reaction rate
Understanding reaction rate is crucial. It tells us how fast a reactant is converted into a product during a chemical reaction. In zero order kinetics, the reaction rate remains constant. This means it doesn't change with the concentration of the reactant. Unlike other reactions where the rate might speed up or slow down as the reactants are used up, in zero order reactions, the rate is solely determined by the rate constant.
rate constant
The rate constant, denoted as k, is pivotal in chemical kinetics. It's a unique value for each reaction that indicates the speed of the reaction. For zero order kinetics, the rate equation is simple: \(\text{Rate} = k\). This implies the reaction occurs at a constant rate determined by k, independent of reactant concentrations. Understanding k helps predict how long a reaction will take and how much product will form over a given time.
product formation
Product formation is directly tied to the reaction's kinetics. For zero order reactions, the amount of product formed over time (t) can be determined using the equation \([P] = kt\). This relationship shows that if time is doubled, the amount of product doubles, as demonstrated in the solution. Zero order reactions provide straightforward calculations, making it easier to predict product amounts at different times.

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