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Question 1 Prior to 1886, Aluminum was rarer and more expensive than gold! It was in 1886, that brother and sister Charles Martin Hall and Julia Brainerd Hall discovered the electrolytic process that separated Aluminum from Aluminum Oxide ore. Today, over 41 million tons are processed for use in everything from beer cans to aircraft skins. a) How many coulombs of electricity must pass through the cell to produce 40.0 g of Aluminum (26.981539 g/mol)Fm an Ala(Soy), cap solution ". b) If the reaction needs to be completed in 1.00 hour, what amperage must be used? p.2 Question 2 Answer the following questions with: a- Always run spontaneously forward regardless of the temperature b-Never run spontaneously forward at any temperature c-Run spontaneously forward only at high temperatures d-Run spontaneously forward only at low temperatures 2 pts. each i- If both the Entropy&Enthalpy are negative, the reaction will be ii-If the Entropy is positive and the Enthalpy is negative, the reaction will be ili- If both the Entropy&Enthalpy are positive, the reaction will iv- If the Entropy is negative and the Enthalpy is positive, the reaction will be Did you know that our nation's Sulfuric Acid production is used as an indicator of our industrial strength? Sulfuric Acid is used to produce batteries, paint, fertilizer, ore processing, steel production, gasoline, detergents, water treatment and so much more. Industry uses it in greater quantities than any other chemical. INDUSTRY Synthesis of Sulfuric Acid Reaction: 2 H2SO4(aq) at 25.0° C 25(s) + 3 Oz(g) + H2O(l) a) Based solely on the entropy indicated by this equation, do you predict that this reaction will run spontaneously forward or in reverse? Explain Chem 4, Dr. La Gattuta p.3 Version 2, Exam 4 Spring 2019 Question 3 (cont) 4 pts. each b) Use the given data to calculate Δ Η..in Joules. Do NOT round off. INDUSTRY Synthesis of Sulfuric Acid Reaction: 25(s) + 3 Olg) + H2O(I) 2 HSOdaq) at 25.0°C aHf k İndzero -285.8 193.9 zero c) If the Entropy of the reaction, AS+98.254 J/K, calculate the Gibbs' Free Energy for this reaction. Express the answer with 4 significant figures d) Based upon your calculations, will this reaction run in the forward direction as written? If not, what, if anything, can be done to force the reaction to run forward? INDUSTRY e) Calculate the Equilibrium constant, keq for this reaction.

Answer 1

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