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ChemistryChemical KineticsMiscellaneous/MixedEasy2 minPYQ_2020

ChemistryEasysingle choice

For the equilibrium, $A (g) ⇌ B (g), ∆ H is - 40$ kJ/mol. If the ratio of the activation energies of the forward $(E_{f})$ and reverse $(E_{b})$ reactions is $\frac{2}{3}$ then:

Options:

Answer:

Solution:

$A (g) ⇌ B (g); ∆ H = - 40$ kJ/mole

$∆ H = E_{a (f)} - E_{a (b)} = - 40 k J$

$\frac{E_{a (f)}}{E_{a (b)}} = \frac{2}{3}$

$\Rightarrow E_{a (f)} = \frac{2}{3} E_{a (b)}$

$\Rightarrow \frac{2}{3} E_{a (b)} - E_{a (b)} = - \frac{E_{a (b)}}{3} = - 40 k J$

$E_{a (b)} = + 120 k J$

$E_{a (f)} = \frac{2}{3} \times 120 = 80 k J$

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

⏱ 2mℹ️ Source: PYQ_2020

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