Chemistry - Chemical Kinetics Question with Solution | TestHub

ChemistryChemical KineticsFirst Order ReactionsMedium2 minQB

ChemistryMediumsingle choice

Passage / Comprehension

For the first-order dissociation reaction

A₂B₃(aq) → 2A³⁺(aq) + 3B²⁻(aq),

a definite volume of solution is taken at different instants, and its osmotic pressure rise is measured. The osmotic pressure rise at $t = 0$ is $2 mm$ and at $t = 10 min$ is $6 mm$ . [Given density of solution is constant and equal to $1 g m / m l$ , $g = 10 m / s^{2}$ ]

Calculate time for $87.5%$ of the reaction to complete -

Options:

Answer:

Solution:

$K \times 10 = ln 2$

$K = (\frac{ln 2}{10}) = \frac{ln 2}{t _{1/2}} \Rightarrow t_{1/2} = 10 min$

$t_{0.875} = 3 \times 10 = 30 min$

Stream:JEESubject:ChemistryTopic:Chemical KineticsSubtopic:First Order Reactions

⏱ 2mℹ️ Source: QB

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