Question:
A $\rightarrow$ P is a first-order reaction. The change in concentration of A with time is shown below. The instantaneous rate at points X, Y and Z is \( R_X \), \( R_Y \), and \( R_Z \), respectively. What is the correct order of \( R_X \), \( R_Y \), and \( R_Z \)?
A $\rightarrow$ P is a first-order reaction. The change in concentration of A with time is shown below. The instantaneous rate at points X, Y and Z is \( R_X \), \( R_Y \), and \( R_Z \), respectively. What is the correct order of \( R_X \), \( R_Y \), and \( R_Z \)?
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In a first-order reaction, the rate is directly proportional to the concentration of the reactant. Higher concentration results in a higher reaction rate.
Updated On: Mar 6, 2026
- \( R_Y > R_X > R_Z \)
- \( R_Y > R_Z > R_X \)
- \( R_X > R_Y > R_Z \)
- \( R_Z > R_X > R_Y \)
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The Correct Option is A
Solution and Explanation
Step 1: For a first-order reaction, the rate of the reaction is directly proportional to the concentration of reactant. Thus, the rate at a given point is highest when the concentration of the reactant is highest.
Step 2: From the graph, it is clear that the concentration of A is highest at point Y, followed by point X, and lowest at point Z.
Step 3: The rate is proportional to the concentration of A, so: \[ R_Y>R_X>R_Z \] Thus, the correct order is \( R_Y>R_X>R_Z \).
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