Question:
Which of the following is true in respect of a zero order reaction?
Which of the following is true in respect of a zero order reaction?
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In zero-order, rate is constant and independent of concentration.
Updated On: Apr 28, 2026
- Plot of [Reactant] against time is a straight line with slope equal to k
- Plot of [Reactant] against time is a straight line with slope equal to -k
- Plot of [Reactant] against time is a straight line with slope equal to 2.303 k
- Plot of [Reactant] against time is a straight line with slope equal to -2.303 k
- Plot of [Reactant] against time is a straight line with slope equal to -k/2.303
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The Correct Option is B
Solution and Explanation
Step 1: Concept
The integrated rate law for a zero-order reaction is $[R] = -kt + [R]_0$.
Step 2: Meaning
This follows the linear equation $y = mx + c$.
Step 3: Analysis
Comparing $[R] = -kt + [R]_0$ with $y = mx + c$, the slope $m$ is $-k$.
Step 4: Conclusion
The plot of concentration vs time gives a slope of $-k$. Final Answer: (B)
The integrated rate law for a zero-order reaction is $[R] = -kt + [R]_0$.
Step 2: Meaning
This follows the linear equation $y = mx + c$.
Step 3: Analysis
Comparing $[R] = -kt + [R]_0$ with $y = mx + c$, the slope $m$ is $-k$.
Step 4: Conclusion
The plot of concentration vs time gives a slope of $-k$. Final Answer: (B)
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