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Chapter 14: Problem 69

Consider the zero-order reaction \(\mathrm{A} \longrightarrow \mathrm{B}\). Sketch the following plots: (a) rate versus [A] and (b) [A] versus \(t\).

Short Answer

Expert verified
Part A: The rate versus [A] plot is a horizontal line, indicating rate is independent of [A]. Part B: The [A] versus time 't' plot is a straight line decreasing with time, indicating [A] decreases at a constant rate.

Step by step solution

01

Sketch the plot for Part A

As this is a zero-order reaction, the rate of the reaction should be independent of the concentration of reactant A. Therefore, plot a graph with 'rate' on the y-axis and '[A]' on the x-axis. Draw a horizontal line on the graph, which represents that the rate is constant and does not change with varying [A]. The rate is equal to the rate constant \( k \) for a zero-order reaction.
02

Sketch the plot for Part B

In a zero-order reaction, the concentration of reactant decreases linearly with time. Therefore, plot a graph with '[A]' on the y-axis and 'time' on the x-axis. Draw a straight line decreasing with time. The slope of the line equals the negative of the rate constant \( k \). This line represents that reactant A is consumed at a constant rate over time.

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