Question

Describe Le Chatelier's principle of dynamic equilibrium. Then, explain why the equilibrium shifts, and which way...

Describe Le Chatelier's principle of dynamic equilibrium. Then, explain why the equilibrium shifts, and which way it shifts, if I2 is removed.

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
According to Le Chatelier's principle, which of the following changes will shift the position of equilibrium...
According to Le Chatelier's principle, which of the following changes will shift the position of equilibrium to the left for the rection: N2 (g) <===> 2NH3 (g) + heat double the concentraion of N2 increase the concentration of H2 decrease the concentration of NH3 triple the temperature
The reaction below is at equilibrium. Use Le Chatelier's principle to predict the effect of adding...
The reaction below is at equilibrium. Use Le Chatelier's principle to predict the effect of adding ammonia gas to the equilibrium reaction mixture. N2(g) + 3H2(g) 2NH3(g) A. The equilibrium position will remain unchanged. B. The equilibrium position will shift to the right. C. The equilibrium position will shift to the left. D. The equilibrium constant will increase. E. All of the nitrogen gas will be used up.
According to Le Chätelier's principle, for the equilibrium reaction A(g) "equilibrium arrow" 2B(g) ,what will the...
According to Le Chätelier's principle, for the equilibrium reaction A(g) "equilibrium arrow" 2B(g) ,what will the response of the system be if we: 1.removed B from the system? 2.increased the temperature of the system? 3.added an inert gas (such as nitrogen gas)?
4.   Predict whether the reaction shifts right or left when 12 M HCl is added. Explain...
4.   Predict whether the reaction shifts right or left when 12 M HCl is added. Explain your prediction. [Note: Use the balanced equation, Co(H2O)62+ + 4Cl- CoCl42- + 6 H2O, to explain the shift. Specifically, which component of the equation is added? And identify the result according to Le Chatelier's Principle.] 5.   Identify the mL of HCl needed to shift the equilibrium. 6.   Calculate the value of the equilibrium expression at the new concentrations. (Show your work.) PART C 7.  ...
Define Le Chatelier’s Principle in your own words. Then, describe an everyday example (not strictly related...
Define Le Chatelier’s Principle in your own words. Then, describe an everyday example (not strictly related to our course) of Le Chatelier’s Principle in nature.
CHEM 114 ‐ Lab Experiment 8 Equilibrium II – Le Chatelier’s Principle 3. When cleaning your...
CHEM 114 ‐ Lab Experiment 8 Equilibrium II – Le Chatelier’s Principle 3. When cleaning your test tubes, excess rinsings and soapy water should not be placed in waste. Think about how chemical waste must be handled and explain why it would be good laboratory practice to avoid putting excessive rinse and soapy water into the hazardous waste containers.    4. In your own words, explain the difference between Q and K. 5. Which description below is most accurate for a...
The common-ion effect is an application of Le Châtelier's principle, which states that an equilibrium system...
The common-ion effect is an application of Le Châtelier's principle, which states that an equilibrium system that is stressed will work to alleviate that stress and reestablish equilibrium. The common-ion effect and solubility The solubility of a slightly soluble salt can be greatly affected by the addition of a soluble salt with a common ion, that is, with one of the ions in the added soluble salt being identical to one of the ions of the slightly soluble salt. The...
Consider LeChatelier’s principle. Explain how the equilibrium of a gas phase reaction will generally shift when...
Consider LeChatelier’s principle. Explain how the equilibrium of a gas phase reaction will generally shift when the partial pressure (or concentration) of each gaseous reactant and product is increased proportionally. Determine which way the equilibrium will shift for the HI reaction if it is at equilibrium and then all three partial pressures are doubled.
What supply shifts best describe the change in the equilibrium shown in the accompany-ing graph?
What supply shifts best describe the change in the equilibrium shown in the accompany-ing graph?
A) Which way will equilibrium shift if add sodium acetate to 0.1 M acetic acid? Why...
A) Which way will equilibrium shift if add sodium acetate to 0.1 M acetic acid? Why does it shift this way? B) Which way will equilibrium shift if add NaOH to acetic acid? Why does it shift this way?