For the following reaction 2 X + Y k P the rate of reaction is d [ P ] dt = k [ X ] . Two…
Chemistry · JEE Advanced · NTA Exams — Chemical Kinetics
For the following reaction
\(2 \mathrm{X}+\mathrm{Y} \xrightarrow{\mathrm{k}} \mathrm{P}\)
the rate of reaction is \(\frac{\mathrm{d}[\mathrm{P}]}{\mathrm{dt}}=\mathrm{k}[\mathrm{X}] .\) Two moles of
X are mixed with one mole of Y to make 1.0 L
of solution. At 50 s, 0.5 mole of Y is left in the
reaction mixture. The correct statement(s) about
the reaction is(are) (Use : ln 2 : 0.693)
(2021)
\(2 \mathrm{X}+\mathrm{Y} \xrightarrow{\mathrm{k}} \mathrm{P}\)
the rate of reaction is \(\frac{\mathrm{d}[\mathrm{P}]}{\mathrm{dt}}=\mathrm{k}[\mathrm{X}] .\) Two moles of
X are mixed with one mole of Y to make 1.0 L
of solution. At 50 s, 0.5 mole of Y is left in the
reaction mixture. The correct statement(s) about
the reaction is(are) (Use : ln 2 : 0.693)
(2021)
- The rate constant, k, of the reaction is
13.86 × 10-4 s-1. - Half-life of X is 50 s.
- At 50 s, \(-\frac{\mathrm{d}[\mathrm{X}]}{\mathrm{dt}}=13.86 \times 10^{-3} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1} .\)
- At 100 s, \(-\frac{\mathrm{d}[\mathrm{Y}]}{\mathrm{dt}}=3.46 \times 10^{-3} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1} .\)
Answer
(B) Half-life of X is 50 s., (C) At 50 s, - d [ X ] dt =13.86 10^ -3 ~mol ~L ^ -1 ~s ^ -1 ., (D) At 100 s, - d [ Y ] dt =3.46 10^ -3 ~mol ~L ^ -1 ~s ^ -1 .
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