Le Chatelier's principle
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Le Chatelier's principleQuestions
- How can we use Le Chatelier's Principle to increase yields of chemical reactions?
- How does Le Chatelier's Principle describe an equilibrium response to a stress?
- How is Le Chatelier's Principle used in the Haber process?
- What is Le Chatelier's principle?
- What is an example of a Le Chatelier's principle practice problem?
- Does Le Chatelier's principle apply to electrochemical cells?
- Does Le Chatelier's principle apply to aqueous solutions?
- How was Le Chatelier's principle used to determine the extinction coefficient?
- What is Le Chatelier's principle in terms of thermodynamic quantities?
- How can Le Chatelier's principle help maximize the yield of reactions?
- How does concentration effect Le Chatelier's principle?
- How does Le Chatelier's principle affect equilibrium?
- How is Le Chatelier's principle used to treat CO poisoning?
- Why is Le Chatelier's principle important?
- Can you use Le Chatelier's principle explain the role of OH ions in the CrO₄²⁻ ⇌ Cr₂O₇²⁻ equilibrium?
- The formation of CoCl4 2- from Co 2+ and Cl- is endothermic. Are the color changes that accompany heating and cooling of equilibrium mixture in accord with Le Chatelier's principle?
- Based on Le Chatelier's principle, what is the predicted effect on solubility of CaCl when a saturated solution?
- Can you explain in terms of Le Chatelier's principle why the concentration of NH3 decreases when the temperature of the equilibrium system increases?
- Based on Le Chatelier's principle, what is the predicted effect on the solubility of calcium chloride?
- Based on Le Chatelier's principle, what would happen to a saturated solution of borax at equilibrium if we added more solid borax?
- Based on Le Chatelier's principle, what would happen to a saturated solution of borax at equilibrium if we added more B4O5(OH)4 2- ions?
- In a closed can of soda, dissolved carbonic acid is in equilibrium with CO2 and H2O. When the can is opened CO2 is produced until the pop goes flat. How do these observations relate to equilibrium and Le Chatelier's principle?
- According to Le Chatelier's Principle: What happens when you add DIFFERENT species to the equilibrium?
- According to Le Chatelier's Principle what will happen to this equilibrium: C2H4O (g) ---> CH4 (g) + CO (g) if we add CH4?
- According to Le Chatelier's Principle what will happen to this equilibrium: C2H4O (g) ---> CH4 (g) + CO (g) if we decrease the size of the container?
- Question #b2e84
- Question #763e3
- Given that the equilibrium...#4NH_3(g) + 3O_2(g)rarr2N_2(g) + 6H_2O(l) + Delta# is exothermic...what will be effect on the equilibrium if... #i.# #"Oxygen is removed;"# #ii.# #"Nitrogen is added;"# #iii.# #"Water is removed;"# #iv.# #"If heat is added?"#
- Question #e0f51
- Question #400da
- The following reaction is in equilibrium: #N_(2(g)) + O_(2(g)) rightleftharpoons 2NO_((g))#, what effect does an increase in pressure have on the yield of #NO#?
- Question #eb54b
- Question #3142c
- What is common ion effect ? Give 3 examples of salt that xan affect the ionization of HNO2 solution?
- According to Le Chateliers principle, how would a change in pressure affect a system in equilibrium?
- According to Le Chateliers principle, what happens if heat is added to a system?
- Question #852d3
- Question #145f0
- Is it true that solids and liquids are not included in the expression of the equilibrium constant?
- Question #eaaa1
- What would happen if #O_2# were added to #N_2(g) + O_2 (g) rightleftharpoons 2NO(g)# at equilibrium?
- Question #4afa9
- What are examples of heterolytic and homolytic cleavage? Could the former happen with methane?
- What is common ion effect?
- What is the levelling effect?
- Question #32a47
- Explain Le Chatelier's principle in simple terms?
- Question #f89d7
- In the synthesis of ammonia, what is the effect of a decrease in the reaction temperature?
- How would the equilibrium concentration of #H_2O# be affected by removing #H_2# from the mixture?
- Question #acd19
- Question #f4a99
- For a given equilibrium reaction for which #K_"eq"=6.4#...what scenario will alter the equilibrium value?
- How is La Chatelier's principle useful in the chemistry industry? What is the effect of temperature on the equilibrium constant?
- If #Na_2S# is added to a solution containing #AgCl#, a black precipitate of #Ag_2S# forms. Why does this happen using Le Chateliers's principle?
- Applying Le Chateliers principle, what can you conclude about the change #2CrO_4^(-2) -> Cr_2O_7^(-2)# and its dependence on hydrogen ions, #H^+#?
- How do you explain Le Chatelier's principle?
- Using Le Chatelier's Principle for this equation, #Fe^(3+) + SCN^(-) -> [Fe(SCN)]^(2+)#, which way would the equilibrium shift occur if #KSCN# was added?
- How would you use Le Chatelier's principle to predict whether the solubility of #BaF_2# will increase, decrease, or remain the same on addition of each of the following substances?
- Consider the equilibrium system #CO(g) + Fe_3O_4(s) ⇌ CO_2(g) + 3FeO(s)# How does the equilibrium position shift as a result of each of the following disturbances?
- How would you use Le Chatelier's principle to explain the different colors found in the following equilibria? #Ni^(2+)#, #NH_3# , and #[Ni(NH_3)_6]^(2+)#?
- How is Le Chatelier's principle used in the Haber Process for making ammonia?
- How would you explain Le Chatelier's principle?
- How does concentration effect Le Chatelier's principle?
- How does volume effect Le Chatelier's principle?
- How do you graph Le Chatelier's principle?
- How was Le Chatelier's principle discovered?
- What does Le Chatelier's principle state?
- What does Le Chatelier's principle say?
- What is Le Chatelier's principle and why is it important?
- What is Le Chatelier's principle for systems in equilibrium?
- What is Le Chatelier's principle in chemistry?
- What is Le Chatelier's principle used to explain?
- Why does Le Chatelier's principle work?
- Does Le Chatelier's Principle state that if a system has a change in concentration, volume or temperature the system will shift to counter-act the change to the system?
- How would decreasing the volume of the reaction vessel affect each of the following equilibria?
- Can someone please fully explain the affect of temperature on equilibrium using Le Chatelier's principle? Also, how does kinetic energy of the mc relate to this? Thanks.
- I understand that when you increase pressure for a reaction at equilibrium it shifts to the side that makes less moles of product and when you decrease pressure, it shifts to the side that makes more moles. Why does the reaction shift in these directions?
- Consider the following reaction at equilibrium: #2NH_3(g) rightleftharpoons N_2(g) + 3H_2(g)# #DeltaH = +92.4 kJ#. What does Le Chatelier's Principle predicts will happen when adding #N_2(g)# to the system at equilibrium?
- For a Le Chatelier Principle lab, I added Thymol Blue (blue) and HCl together. What would be the equilibrium equation to represent this situation?
- For a saturated solution of #AgNO_3(aq)#, what will be the effects of: (i) addition of silver nitrate salt; (ii) addition of nitric acid; (iii) addition of silver perchlorate...?
- Question #ac451
- For the reaction, #"CaCO"_3"(s)" ⇌ "CaO(s) + CO"_2"(g)"#,what will happen in each of the followig cases?
- Question #81435
- Given the equation representing a system at equilibrium: #N_2(g) + 3H_2(g) rightleftharpoons 2NH_3(g) + "energy"#, what changes occur when the temperature of this system is decreased?
- Question #0318d
- Question #d34eb
- According to Le Chatelier's principle, how will a pressure increase a a gaseous system?
- Question #b292b
- Question #7fc24
- Question #28ec0
- Question #b826c
- Question #842ec
- What is #K_"sp"#?
- Question #eb3d7
- Question #43f8e
- Question #77a0a
- Question #c0ac4
- In this reaction: #"HIn" (aq) rightleftharpoons "H"^(+)(aq) + "In"^(-)(aq)# What happens when these stressors are added? Does the stress add or remove products or reactants? What's the shift? Which ion is involved in the reaction?
- Question #3c6f1
- Question #cc8dd
- Le Chatelier's Principle: #N2 (g) + 3H2 (g) -> 2NH2 (g)# ?
- Question #f395d
- Question #f3be3
- Question #77b85
- A system at equilibrium is placed under stress by adding more reactant. If this reaction has a small equilibrium constant (Keq), how will the addition of this stress affect the equilibrium of this system?