MODEL 2: Le Châtelier\'s Principle If a change is imposed on a system, the posit
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MODEL 2: Le Châtelier's Principle If a change is imposed on a system, the position of equilibrium will shift in a direction that tends to reduce that change. KEY QUESTIONS What will happen to the number of students in the two rooms in Model 1 if the temperature in Classroom 124 rises because the air exchange system for that room fails? Explain your answer in terms of Le Châtelier's Principle. 6. According to Le Châtelier's Principle, what will happen in a chemical reaction at equilibrium if a reaction product is removed? 7. 217 Activity 31-Dynamic Equilibrium and Le Châtelier's Principle www.rspaperproducts.comExplanation / Answer
7. if the product is removed from a reaction system, the concentration of product will decrease and system will try to increase its concentration by increasing the rate of forward reaction.
8. if more reactant is added, system will try to decrease the concentration of reactant by increasing the rate of forward reaction.
9. The rate of ice melting is proportional to formation of ice
the equilibrium existence between oxygen and carbon dioxide in the nature
10. CH4 + H2O <=> 3H2 + CO
CO removed; product removed, then system will readjust the equilibrium to product side to nullify the removal effect of product. So forward reaction will be faster.
Water vapor removed; reactant removed, then system will readjust equilibrium towards backward direction to increase the concentration of water vapor.
Methane is added: reactant concentration increases, so forward reaction will be faster to decrease the concentration of reactant and more product will produced.
CO is added, again product concentration increases, so backward reaction will be faster to remove the higher concentration of CO, so more reactant will produce.
Argon is a non reactive inert gas, so will not affect the equilibrium.
If pressure decreased, reaction in which number of moles increases will occur. That is forward reaction will occur( 2 moles ? 4 moles)
catalyst can increase or decrease the rate of reaction.
11. N2 + O2 <=> 2 NO
here the number of moles of reactant and product are same, so no role for pressure. The reaction will not change its equilibrium.
12. N2 + 3 H2 <=> 2NH3 + heat
here high pressure and low temperature needed to get maximum product. Because if pressure increases, forward reaction will favor by decreasing number of moles from 4 to 2 and produce more ammonia, while, decrease in temperature will result in the increase of temperature by increasing the rate of exothermic forward reaction.
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