The equilibrium constant for a reaction A + B ⇋ C + D is 1 × 10 - 2 at 298 K and is 2 at 273 K . The chemical process resulting in the formation of C and D is:

log K 2 K 1 = ΔH 2.303 R 1 T 1 − 1 T 2 T 1 > T 2 & K 2 > K 1 ΔH = − Ve

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ChemistryChemical EquilibriumMiscellaneous/MixedEasy2 minPYQ_2020

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The equilibrium constant for a reaction $A + B ⇋ C + D$ is $1 \times 10^{- 2}$ at $298 K$ and is $2$ at $273 K .$ The chemical process resulting in the formation of $C$ and $D$ is:

Options:

Answer:

Solution:

$log \frac{K_{2}}{K_{1}} = \frac{ΔH}{2.303 R} (\frac{1}{T_{1}} - \frac{1}{T_{2}})$

$T_{1} > T_{2} & K_{2} > K_{1}$

$ΔH = - Ve$

Stream:NTA_ABHYASSubject:ChemistryTopic:Chemical EquilibriumSubtopic:Miscellaneous/Mixed

⏱ 2mℹ️ Source: PYQ_2020

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