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Phase-I sepera 1 11 Dipote-[ lon-Di Dispersi Hydroge N-H₂ O Surfacet CONESA adnesio Viscosit equilion Polling Pol normalk CriticalT entual ligultat), concent fractiona folligati solution ismosis: concentra em perm smohe p olliod-di! rat COY alflife- Ctivation atalyst-Su eterogeneo стадели 4. The Haber process is used to synthesize ammonia from nitrogen gas: N₂(g) + 3H2(g) 2NH3(g) a) The equilibrium constant (K.) for this reaction is 1.2 at 375 °C. Starting with the initial concentrations of [N₂] = 0.60 M, [H₂] = 0.76 M and [NH3] = 0.48 M, calculate Qc. Which direction does the reaction need to go to reach equilibrium? b) Build an ICE table. Just built the ICE table, you don't need to go further because solving for x is very complex. c) This is a very important reaction for the synthesis of ammonia using in fertilizer. Using Le Chatelier's Principle, describe 3 processes that can be done to increase the yield of ammonia. 5. The equilibrium constant for the following reaction is 33.3 at 100 °C. Blue + Groo 2Rod

Phase-I sepera 1 11 Dipote-[ lon-Di Dispersi Hydroge N-H₂ O Surfacet CONESA adnesio Viscosit equilion Polling Pol normalk CriticalT entual ligultat), concent fractiona folligati solution ismosis: concentra em perm smohe p olliod-di! rat COY alflife- Ctivation atalyst-Su eterogeneo стадели 4. The Haber process is used to synthesize ammonia from nitrogen gas: N₂(g) + 3H2(g) 2NH3(g) a) The equilibrium constant (K.) for this reaction is 1.2 at 375 °C. Starting with the initial concentrations of [N₂] = 0.60 M, [H₂] = 0.76 M and [NH3] = 0.48 M, calculate Qc. Which direction does the reaction need to go to reach equilibrium? b) Build an ICE table. Just built the ICE table, you don't need to go further because solving for x is very complex. c) This is a very important reaction for the synthesis of ammonia using in fertilizer. Using Le Chatelier's Principle, describe 3 processes that can be done to increase the yield of ammonia. 5. The equilibrium constant for the following reaction is 33.3 at 100 °C. Blue + Groo 2Rod

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Phase-1 sepera 1 11 Dipute-[ lon-Dir Dispersi Hydroge N-H₂₂ O Surfacet Conesa adnesio viscosity equilibr Polling Pol Hormalk criticall entual Tiquitat, concent fractiona folligati solution osmosis - concentra Bemi perm Asmotic p Bolliod.di! rat COY hout life- & activation catalyst-Su heterogeneo homogene Henry's секр 4. The Haber process is used to synthesize ammonia from nitrogen gas: N₂(g) + 3H₂(g) 2NH3(g) a) The equilibrium constant (K.) for this reaction is 1.2 at 375 °C. Starting with the initial concentrations of [N₂] = 0.60 M, [H₂] = 0.76 M and [NH3] = 0.48 M, calculate Qc. Which direction does the reaction need to go to reach equilibrium? b) Build an ICE table. Just built the ICE table, you don't need to go further because solving for x is very complex. c) This is a very important reaction for the synthesis of ammonia using in fertilizer. Using Le Chatelier's Principle, describe 3 processes that can be done to increase the yield of ammonia. 5. The equilibrium constant for the following reaction is 33.3 at 100 °C. 4Blue + Green 3 Red Below are three experiments. For each experiment, calculate Qc and describe how the reactants and products need to change to reach equilibrium
Transcribed Image Text:Phase-1 sepera 1 11 Dipute-[ lon-Dir Dispersi Hydroge N-H₂₂ O Surfacet Conesa adnesio viscosity equilibr Polling Pol Hormalk criticall entual Tiquitat, concent fractiona folligati solution osmosis - concentra Bemi perm Asmotic p Bolliod.di! rat COY hout life- & activation catalyst-Su heterogeneo homogene Henry's секр 4. The Haber process is used to synthesize ammonia from nitrogen gas: N₂(g) + 3H₂(g) 2NH3(g) a) The equilibrium constant (K.) for this reaction is 1.2 at 375 °C. Starting with the initial concentrations of [N₂] = 0.60 M, [H₂] = 0.76 M and [NH3] = 0.48 M, calculate Qc. Which direction does the reaction need to go to reach equilibrium? b) Build an ICE table. Just built the ICE table, you don't need to go further because solving for x is very complex. c) This is a very important reaction for the synthesis of ammonia using in fertilizer. Using Le Chatelier's Principle, describe 3 processes that can be done to increase the yield of ammonia. 5. The equilibrium constant for the following reaction is 33.3 at 100 °C. 4Blue + Green 3 Red Below are three experiments. For each experiment, calculate Qc and describe how the reactants and products need to change to reach equilibrium
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