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Brief equilibrium presentation. No problems Equilibrium constants . Haber Process . TED Ed Lessons https :// ed.ted.com/lessons/the-chemical-reaction-that-feeds-the-world-daniel-d-dulek New concept: equilibrium . Issues- Chemical reactions Good & Evil .
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Brief equilibrium presentation No problems Equilibrium constants
Haber Process • TED Ed Lessons • https://ed.ted.com/lessons/the-chemical-reaction-that-feeds-the-world-daniel-d-dulek • New concept: equilibrium
Issues- Chemical reactions Good & Evil • Haber received much criticism for his involvement in the development of chemical weapons in pre-World War II Germany, both from contemporaries and from modern-day scientists. • The research results show the ambivalence of his scientific activity: on the one hand, development of ammonia synthesis for the manufacture of explosives and of a technical process for the industrial manufacture and use of poison gas in warfare; but on the other hand, development of an industrial process without which the food supply for today's world population would be greatly diminished
Chemical Reaction Equilibrium • Reversible reactions: ↔⇄ • Explain what a reversible reaction will do to products and reactants
Chemical Reaction Equilibrium • Reversible reactions: ↔⇄ • Can happens naturally • Products can be turned back to reactants • In other words: Products recombine to form the original substances
Reversible reactions and Equilibrium • Equilibrium = balance between the amount of reactants and products in a reversible reaction Needs a closed system: no additional reactants added and no products are taken away or escape as a gas) Dynamic equilibrium Forward and backward reactions taking place at the same rate
Upsetting the equilibrium to make more product Upsetting the equilibrium = shifting the equilibrium • Change temperature If an endothermic reaction -absorb or release heat? -example of types of reaction? CaCO₃ + heat ⇄ CaO + CO₂ Add more heat (raise the temperature) to make more product If an exothermic reaction– reduce the amount heat (lower the temperature) to make more product Reaction will try to replace the heat that was taken away
Upsetting the equilibrium to make more product • Change the pressure • Important when gases react • Many reactions will have greater volume on one side (more product or more reactant) If we increase the pressure – The reaction will “favor” the reaction side with less volume If we lower the pressure – The reaction will “favor” the reaction side with more volume N₂ + 3 H₂ ⇄ 2NH₃
Le Chatelier Principle • If you change the conditions, the position of the equilibrium will shift to oppose the change.