MCQ
The rate constant of a first order reaction whose half-life is $ 480\,\sec$ , is
- A$2.88 \times {10^{ - 3}}\,{\sec ^{ - 1}}$
- ✓$1.44 \times {10^{ - 3}}\,{\sec ^{ - 1}}$
- C$1.44\,{\sec ^{ - 1}}$
- D$0.72 \times {10^{ - 3}}\,{\sec ^{ - 1}}$
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$2B\xrightarrow{k}{B_2}$ [Slow]
${B_2} + A \to D$ [Fast]
The rate law expression, order with respect to $A$, order with respect to $'B'$ and overall order are respectively