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Chemical Kinetics question

2005 · Q85
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Chemical Kinetics question

2005 · Q85

NEETChemistryChemical KineticsMCQ+4 / −1
For a first order reaction A →\to→ B the reaction rate a reactant concentration of 0.01 M is found to be 2.0 ×\times× 10−-−5 mol L−-−1 s−-−1. The half-life period of the reaction is
  1. A
    30 s
  2. B
    220 s
  3. C
    300 s
  4. D
    347 s
View written solutionFree

Correct answer: D

Given [A] = 0.01 M

Rate = 2.0 × 10–5 mol L–1 S–1

For a first order reaction

Rate = k[A]

k = 2×10−50.01=2×10−3{{2 \times {{10}^{ - 5}}} \over {0.01}} = 2 \times {10^{ - 3}}0.012×10−5​=2×10−3

⇒\Rightarrow⇒ t1/2=0.6932×10−3=347 sec⁡{t_{1/2}} = {{0.693} \over {2 \times {{10}^{ - 3}}}} = 347\,\sec t1/2​=2×10−30.693​=347sec

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