Explain chemical equilibrium (Le Chatelier’s Principle): how changes in temperature, pressure, volume, or concentration affect the...

Explain chemical equilibrium (Le Chatelier’s Principle): how changes in temperature, pressure, volume, or concentration affect the equilibrium position for a chemical reaction

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queen_honey_blossom answered 2 years ago

CHEM 114 ‐ Lab Experiment 8 Equilibrium II – Le Chatelier’s Principle 2. There is chemical...

CHEM 114 ‐ Lab Experiment 8 Equilibrium II – Le Chatelier’s Principle 2. There is chemical waste that must be disposed of properly in this lab. Identify which wastes are highly hazardous and explain why they must be properly discarded.

Define Le Chatelier’s Principle in your own words: If concentration of a reactant is increased, explain...

Define Le Chatelier’s Principle in your own words: If concentration of a reactant is increased, explain which way (and why) the equilibrium will shift If product is removed from a reaction at equilibrium, it will cause a shift in which direction? Why? If the temperature of an endothermic reaction is raised, what will be the effect on equilibrium? Explain. If the temperature of an exothermic reaction is decreased, what will be the effect on equilibrium? Explain.

How is Le Chatelier’s Principle used to ensure the reaction will go to completion?

CHEM 114 ‐ Lab Experiment 8 Equilibrium II – Le Chatelier’s Principle 1. There are safety...

CHEM 114 ‐ Lab Experiment 8 Equilibrium II – Le Chatelier’s Principle 1. There are safety hazards in this lab experiment. Specifically, what are the safety hazards associated with the experimental procedure? Be sure to clearly identify and explain why these are hazards.

1. Explain how a concentration dependant monomer-dimer equilibrium agrees with Le Châtelier’s principle. Hint, in order...

1. Explain how a concentration dependant monomer-dimer equilibrium agrees with Le Châtelier’s principle. Hint, in order for a dimer to form two monomers must collide and dimers, once formed, do dissociate after a period of time.

10- Describe Le Chatelier’s Principle 11-Consider the following reaction at equilibrium. What effect will reducing some...

10- Describe Le Chatelier’s Principle 11-Consider the following reaction at equilibrium. What effect will reducing some C have on the system? Why? CO2(g) + C(graphite) ⇌ 2 CO(g) 12- Consider the following reaction at equilibrium. What effect will increasing the volume of the reaction mixture have on the system? Why? CuS(s) + O2(g) ⇌ Cu(s) + SO2(g) 13-Consider the following reaction at equilibrium. What effect will reducing the volume of the reaction mixture have on the system? Why?...

Lab Experiment 8 Equilibrium II – Le Chatelier’s Principle Part A ? Lead Compounds Given: Pb2+ + 2...

Lab Experiment 8 Equilibrium II – Le Chatelier’s Principle Part A ? Lead Compounds Given: Pb2+ + 2 I ? ? PbI2 Pb2+ + 2 OH? ? Pb(OH)2 2. Describe the change observed when sodium hydroxide is added in step b (step b. Add enough 0.1M NaOH to cause a change. Swirl/stir to mix thoroughly) and explain why this change is consistent with Le Chatelier's principle. {Note – to explain in terms of Le Chatelier’s principle means to explain the new change in conditions (in terms of...

Lab Experiment 8 Equilibrium II – Le Chatelier’s Principle Part B ‐ Thiocyanate Complexes Given: Fe3+ + SCN‐...

Lab Experiment 8 Equilibrium II – Le Chatelier’s Principle Part B ‐ Thiocyanate Complexes Given: Fe3+ + SCN‐ ⇌ FeSCN2+ Ag+ + SCN‐ ⇌ AgSCN 2. Describe the change observed when silver nitrate is added in step b(b. Add enough AgNO3 to cause a change. Swirl/stir to mix thoroughly) and explain why this change is consistent with Le Chatelier's principle. 3. Describe the change observed when sodium chloride is added in step c (c. Add enough NaCl to cause a change. Swirl/stir to mix...

How to use Le Chatelier's principle to predict the effect of a change in concentration on...

How to use Le Chatelier's principle to predict the effect of a change in concentration on the equilibrium position and on K?

Give 2 examples showing how competing equilibrium reactions affect one another. ( Le Chatlier's Principle)

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