Question

Integrated rate law for zero order reaction is

• A. \(K=\frac{2.303}{t}\log _{10}\frac{[A]_{0}}{[A]_{t}}\)
• B. \(K=\frac{2.303}{t}\log _{10}\frac{a}{a-x}\)
• C. \(K=\frac{0.693}{t_{1/2}}\)
• D. \(K=\frac{[A]_{0}-[A]_{t}}{t}\)

Hint:

For zero order the rate is constant, so the concentration falls linearly with time.

Answer 1

The Correct Option is D

Step 1: Understanding the Concept
In a zero order reaction the rate does not depend on concentration: \(-\dfrac{d[A]}{dt}=k\).

Step 2: Integrate
Integrating from \([A]_0\) to \([A]_t\) gives \([A]_0-[A]_t=kt\).

Step 3: Result
So \(k=\dfrac{[A]_0-[A]_t}{t}\), with the unit mol L\(^{-1}\) s\(^{-1}\).

Final Answer:
The zero order integrated rate law is \(k=\dfrac{[A]_0-[A]_t}{t}\). \[ \boxed{\text{(D) }K=\dfrac{[A]_{0}-[A]_{t}}{t}} \]