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Zorluk: OrtaLe Chatelier's Principle
For the Haber process reaction represented by the thermochemical equation: N2(g)+3H2(g)⇌2NH3(g)ΔH=−92 kJ mol−1N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \quad \Delta H = -92\text{ kJ mol}^{-1} Match each applied stress condition on the left with its corresponding effect on the equilibrium system on the right.
  • Increasing the temperature of the systemShifts equilibrium to the left, decreasing NH3(g)NH_3(g) yield
  • Increasing total pressure by decreasing container volumeShifts equilibrium to the right, increasing NH3(g)NH_3(g) yield
  • Adding finely divided iron catalystIncreases rates of forward and reverse reactions equally without shifting equilibrium position
  • Adding argon gas at constant volumeHas no effect on partial pressures or equilibrium position

Cevap

Increasing temperature matches shifting equilibrium to the left (decreasing NH3NH_3 yield); Increasing total pressure matches shifting equilibrium to the right (increasing NH3NH_3 yield); Adding iron catalyst matches increasing rates equally without shifting position; Adding argon gas at constant volume matches having no effect on partial pressures or equilibrium position.
Each stress condition matches its specific thermodynamic or kinetic outcome according to Le Chatelier's principle: heating an exothermic reaction favors the reverse endothermic direction; increasing pressure favors the side with fewer gas moles (products); adding a catalyst accelerates both reaction directions equally; and adding inert gas at constant volume leaves partial pressures unchanged.

Adım Adım Çözüm

1
Analyze temperature perturbation using exothermic enthalpy data
The forward reaction releases heat (\Delta H = -92\text{ kJ mol}^{-1}). Heating shifts equilibrium in the heat-absorbing (endothermic/reverse) direction.
Le Chatelier's principle predicts the system counteracts temperature elevation by favoring the endothermic reaction.
2
Analyze pressure perturbation using stoichiometric gas coefficients
Reactants contain 4 moles of gas (1N2+3H21N_2 + 3H_2) while products contain 2 moles (2NH32NH_3). Increased pressure shifts equilibrium toward fewer gas moles.
Decreasing volume increases gas pressure, so the system relieves pressure by forming fewer gaseous molecules.
3
Determine catalyst effect on dynamic equilibrium
The iron catalyst accelerates both forward and reverse rates equally.
Catalysts alter the reaction mechanism to lower activation energy equally in both directions, leaving equilibrium composition unchanged.
4
Determine inert gas effect at constant volume
Adding argon at constant volume does not change concentrations or partial pressures of N2N_2, H2H_2, or NH3NH_3.
Equilibrium position depends strictly on partial pressures of reacting species, which remain constant.

Anahtar Kavram

Le Chatelier's Principle (effects of temperature, pressure, catalysts, and inert gas additions)
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Le Chatelier's Principle

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