Which of the following graphs most appropriately represents a zero-order reaction?
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The Correct Option is B
Approach Solution - 1
To solve this problem, we need to understand the characteristics of a zero-order chemical reaction. In a zero-order reaction, the rate of reaction is constant and independent of the concentration of the reactants.
The rate equation for a zero-order reaction can be expressed as:
\[\text{Rate} = k\]where \(k\) is the rate constant.
The integrated rate law for a zero-order reaction is given by:
\[[A] = [A]_0 - kt\]where \([A]\) is the concentration of the reactant at time \(t\), \([A]_0\) is the initial concentration, \(k\) is the rate constant, and \(t\) is the time elapsed.
This equation resembles the equation of a straight line:
\[y = mx + c\]In this context, the concentration \([A]\) acts as \(y\), time \(t\) as \(x\), \(-k\) as the slope \(m\), and \([A]_0\) as the intercept \(c\).
Therefore, for a zero-order reaction, a plot of \([A]\) vs. \(t\) will be a straight line with a negative slope. Given the options, the correct graph that represents a zero-order reaction is:
This graph clearly shows a linear decrease in concentration over time, indicating a zero-order reaction.
Let's summarize why other options are incorrect:
- Other graphs would represent different order reactions (like first or second order) typically showing a nonlinear relationship between the concentration and time.
Approach Solution -2
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