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April 18, 2014

Search: Chemistry - Le Chatelier's principle(help)

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Chemistry
Adding NO will favor products. Le Chatelier's Principle. Removing NO2 will favor products. Le Chatelier's Principle. decreasing volume of the container will have no effect since the number of moles on the left is the same as the number of moles on the right. Your post isn't ...
Saturday, January 22, 2011 at 3:21pm by DrBob222

chemistry
System: Co(H2O)6^2+(aq) + 4Cl^-(aq) <==> CoCl4^2-(aq) + 6H2O(l) Q: What would happen when you add HCl as a source of Cl- ions? Explain the observations in terms of Le Chatelier's principle. Would the answer be that the reaction shifts to the right? How would you say this...
Friday, November 14, 2008 at 2:32am by Tanimoto

chemistry
im doing a lab on le chatelier's priciple and the question is 'describe what you observe when the saturated solution of sodium chloride was stressed by the addition of CL- ions, write the ionic equation and explain how le chatelier's principle is applied to this experiment.' i...
Sunday, January 24, 2010 at 5:07pm by Anonymous

chemistry help plz
Le chatelier's principle? co(g)+cl2(g)=cocl2(g)is reversible and ,after a certain amount of time ,will reach equilibrium.Explain,using Le chatelier's principle,what effect: 1)increasing the pressure (at constant temperature) 2)increasing the temperature (at constant pressure) ...
Saturday, January 5, 2013 at 4:49pm by centya

chemistry
RE: Le Chatelier's principle. this was the whole question i was given. Write a short account of around 250 words in total, with reference to Le Chatelierís principle, in which you explain the following: (i) The effect on the equilibrium yield of nitric oxide of increasing the ...
Wednesday, January 28, 2009 at 7:42pm by trigger

chem
un-ionized aspirn molecules can readily penetrate the stomach lining into a region of less adicity. This is where the stomach irritation associated with aspirn occurs. Use Le Chatelier's principle to explain why irritation occurs in this area. Could someone explain the ...
Monday, July 27, 2009 at 3:26am by Lena

chemistry
You can look up Le Chatelier's Principle in your text or on-line. The principle is based on the idea that a system at equilibrium will shift in such as way so as to relieve the stress.
Friday, January 22, 2010 at 8:27pm by DrBob222

Chemistry
Le Chatelier's Principle.
Tuesday, May 15, 2012 at 12:47pm by DrBob222

Chemistry
It's all about Le Chatelier's Principle.
Monday, February 20, 2012 at 1:47pm by DrBob222

Chemistry
Le Chatelier's Principle. Which way will the reaction shift?
Tuesday, May 15, 2012 at 12:49pm by DrBob222

CHEM-Le' Chatelier's Principle
I think you're on the right track because the amount of H+ or OH- affects the equilibrium, which relates to the principle
Wednesday, March 4, 2009 at 7:37pm by sometimesknows

CHEM-Le' Chatelier's Principle
I think you're on the right track because the amount of H+ or OH- affects the equilibrium, which relates to the principle
Wednesday, March 4, 2009 at 7:37pm by sometimesknows

Chemistry - Le Chatelier's Principle
Thank you Dr.Bob. I got it now.
Sunday, March 9, 2014 at 1:30pm by Constantine

Chemistry
As a follow up to GK's response, think in terms of Le Chatelier's Principle.
Sunday, June 21, 2009 at 7:24am by DrBob222

chemistry
defie le chatelier's principle and the role equilibrium plays in the reduction of stress
Friday, January 22, 2010 at 8:27pm by lala

chemistry
How does Le Chatelier's principle explain the result you obtained after the addition of NaOH?
Saturday, April 7, 2012 at 1:41pm by Emily

Chemistry
to decipher properties of acid-base chemistry and how they adhere to Le Chatelierís principle. I appreciate any input on it.
Tuesday, November 30, 2010 at 11:16am by Colleen

Chemistry
Le Chatelier's principle states that increasing temperature moves in the direction of the endothermic reaction.
Friday, August 8, 2008 at 5:04pm by bobpursley

chemistry
What was Le Chatelierís principle, in The effect on the equilibrium yield of nitric oxide of increasing the pressure?
Tuesday, January 6, 2009 at 7:04am by trigger

chemistry
I would go with Le Chatelier's Principle. Increasing (O2) will shift the equilibrium to the right.
Tuesday, February 21, 2012 at 12:22pm by DrBob222

Chemistry
How does Le Chatelier's principle explain the result you obtained when you added HCL to a suspension of Ca(OH)2 in water?
Sunday, October 9, 2011 at 2:55pm by mary

chemistry lab
I can help you through this but I don't want to write it for you. The common ion effect is just an example of Le Chatelier's Principle.
Monday, July 9, 2012 at 11:04pm by DrBob222

chemistry
Very carefully, but breifly discuss, with specific example, Le Chatelier Principle and its relationship to common ion effect.
Thursday, October 13, 2011 at 7:47pm by travis

Chemistry - Le Chatelier's principle(help)
Le Chatelier's principle states that " a dynamic equilibrium tends to respond as to relieve the effect of any change in the conditions that affect the equilibrium." I understand the above, now i am trying to predict the response of the system and i am confused how to do it, so...
Tuesday, March 22, 2011 at 6:13am by Babelii

Chemistry
I think the definitions in texts and lecture notes sounds so very esoteric when discussing Le Chatelier's Principle; however, it seems to confuse most students. Therefore, I've developed my own definition for purposes of Le Chatelier's Principle. In a nutshell, in a system at ...
Tuesday, December 6, 2011 at 9:12pm by DrBob222

science - chemistry (Le Chatelier's)
How does the concentration of the reactants affect the amount of product obtained? In general, does an increased concentration of reactant give more product? What are the exceptions? Does it matter if it's exothermic or endothermic? If the reactants/products are in liquid/...
Saturday, August 25, 2007 at 4:35am by siobhan

CHEM-Le' Chatelier's Principle
your wronggg
Wednesday, March 4, 2009 at 7:37pm by funnny

Chemistry
I honestly don't know how to answer this question. Le Chatelier's Principle applies to acid/base chemistry, of course, but no differently than to any other reaction of any other kind.
Tuesday, November 30, 2010 at 3:49pm by DrBob222

Chem.....
Methanol, CH3OH, is produced on an industrial scale from carbon monoxide and hydrogen. At the temperatures used, gaseous methanol is formed according to the following thermochemical equation: CO(g)+ 2H2(g) <---> CH3OH(g) H = -90Kj 1. State Le Chateliers principle and ...
Sunday, March 4, 2007 at 12:53pm by Jon

Chemistry Help.......
State the Le Chatelier's principle and explain the following i) The effect that incresing the pressure will have on the eaualibrium yield of methanol ii) The effect of increasing the temperature will have on the equalibrium yeild of methanol iii) The effect of the increasing ...
Monday, March 12, 2007 at 4:36pm by Lacey

Chemistry II
Do you have any answers from which to choose? I've never called it a type of reaction, other than an equilibrium equation and it shifts to the left because of Le Chatelier's Principle.
Wednesday, October 28, 2009 at 12:01pm by DrBob222

Chemistry
NH4HS(s) reverse reaction arrow NH3(g) + H2S(g) Using Le Chatelier's principle, explain how increasing the temperature would affect the equilibrium.
Wednesday, May 25, 2011 at 2:16pm by Kat

Chemistry
Increasing T will make the reaction shift to the left; therefore, the amount of SO3 will decrease. BUT you need to be able to do these by yourself. What is confusing you about Le Chatelier's Principle?
Friday, March 12, 2010 at 7:12pm by DrBob222

chemistry
a. what is the effect on the Kc when the temperature of an exothermic reaction is lowered? b. according to Le Chatelier's principle, how is equilibrium in part a established.
Friday, November 30, 2012 at 10:03am by Boo Boo

Chemistry
Either reactant in excess will drive the equilibrium to the right (Le Chatelier's Principle). Also, look to see if side reactions are possible, and if so, how those might be affected.
Friday, February 12, 2010 at 9:44am by DrBob222

Chemistry
According to Le Chatelier's principle, does the equilibrium shift to the products or reactants when O2 is added to the equilibrium mixture of the following: A. 302(g) - 2O3(g)
Wednesday, April 20, 2011 at 9:42pm by Eric

Chemistry
I need to be able to tie in acetic acid and boric acid. To decipher properties of acid-base chemistry and how they adhere to Le Chatelierís principle. I appreciate any input....
Tuesday, November 30, 2010 at 3:49pm by Colleen

Chemistry
All of these questions are Le Chatelier's Principle. This really is a simple concept. Tell me what you don't understand about it and perhaps I can set you up to answer all of them.
Monday, October 18, 2010 at 6:01pm by DrBob222

Chemistry
Acetic acid is CH3COOH. Boric acid is H3BO3. You need to be more specific about Le Chatelier's Principle in relation to these two chemicals.
Tuesday, November 30, 2010 at 11:16am by DrBob222

Chemistry
How does Le Chatelier's principle explain the result you obtained when you add HCL to a suspension of Ca(OH)2 in water? Where the result was, precipitate dissappeared and an increase in temperature resulted.
Monday, February 24, 2014 at 10:51pm by J

chemistry
it depends on the reaction, can you type the reaction equation? for the Le Chatelier's principle you need to know the whole reaction, not just the product
Tuesday, January 27, 2009 at 6:59pm by Anonymous

general
Hundreds of sites are available but it depends upon what in chemistry you need help with. The easiest thing to do is to go to Google and type in the subject (not chemistry but the area of chemistry). For example, Le Chatelier's principle if you need help with that or gas laws ...
Saturday, October 26, 2013 at 10:42pm by DrBob222

chemistry
How does Le Chatelier's principle explain the result you obtained when you added HCL to a suspension of Ca(OH)2 in water? Where the result was, precipiatate dissappeared and an increase in temperature resulted.
Sunday, October 9, 2011 at 5:00pm by mary

chemistry
The system H2 (g) + 3N2 (g) = NH3 (s) is at equilibrium.Use Le Chatelier's principle to predict the direction in which the equilibrium will shift if the ammonia is withdrawn from the reaction chamber.
Wednesday, March 6, 2013 at 12:31pm by Shane

Chem
Le Chatelier's principle involves equillibriums. I don't understand the equillibrium involved in thsi situation?
Sunday, July 26, 2009 at 9:51pm by Lena

Le Chatelier's Principle
adding more positive ions. It shifts to the left,trying to remove them.
Tuesday, April 19, 2011 at 7:53pm by bobpursley

chemistry
What do you not understand about Le Chatelier's Principle? It says that a reaction in equilibrium will shift to undo what we do to it. Hint for this question: Remember solids and pure liquids are not included in equilibrium constants.
Saturday, July 21, 2012 at 11:21pm by DrBob222

Chemistry
I was given extra credit to find who Le Ch‚telier's High School Principal was. Not his PrincipLE, but his PrincipAL. My chemistry teacher told us only one student of his out of all these years came with the answer. Think outside of the box. Thanks.
Saturday, March 2, 2013 at 3:23pm by Enrico

Chemistry
I was given extra credit to find who Le Ch‚telier's High School Principal was. Not his PrincipLE, but his PrincipAL. My chemistry teacher told us only one student of his out of all these years came with the answer. Think outside of the box. Thanks.
Monday, March 11, 2013 at 9:12pm by John

chem
All of the texts give really GREAT (and quite esoteric) descriptions of Le Chatelier's Principle. I find that putting it down to earth helps. In plain words, Le Chatelier's Principle says that when we do something to a system at equilibrium it will react in such a ways so as ...
Tuesday, March 27, 2012 at 5:13pm by DrBob222

CHM
This ia Le Chatelier's Principle problem. When working with those problems I find it best to include heat as part of the equation. for dH = + it means endothermic; for dH = - it means exothermic. Therefore, I add heat to the appropriate side. HCN + heat ==> H^+ + CN^- Le ...
Tuesday, April 16, 2013 at 9:11am by DrBob222

chemistry
____ 14. Adding a charged particle common to two solutes decreases solute concentration. This observation demonstrates a. the common-ion effect. c. hydrolysis. b. Le Ch‚telier's principle. d. buffering.
Tuesday, March 1, 2011 at 5:26pm by alex

CHEM-Le' Chatelier's Principle
Use Le' Chatelier's Principle. this is a solution at equilibrium: 2CrO4^2-(aq)+ 2H^+(aq)< >Cr2O7^2-(aq) +H20 2CrO4^2- yellow Cr2O7^2- orange I just have to make predictions of the colour changes when: a)Add 0.3 M NaOH drop to 5 drops of 0.3 M K2CrO4 b)Add 0.3 M HCl by ...
Wednesday, March 4, 2009 at 7:37pm by lostttt

chemistry help plz
Chem principle #1. DON'T try to get by without using the caps key. CO, Co, and co are different. Remember that. Le Chatelier's Principle, in very basic English, tells us that a system in equilibrium will try to UNDO what we do to it. Increasing P will make the reaction shift ...
Saturday, January 5, 2013 at 4:49pm by DrBob222

chemistry
Remember what I told you in the last response. Le Chatelier's Principle--with gases-- the system shifts to the side with the fewer moles of gas. There are three moles on the left and 2 on the right. Goes to the right.
Tuesday, April 3, 2012 at 6:08pm by DrBob222

CHEM-Le' Chatelier's Principle
so lets say for c. HCl adds H+ ions to the product side which makes it more acidic and therefore yellow?
Wednesday, March 4, 2009 at 7:37pm by lostttt

Chem
There are Le Chatelier's Principle type question. You want answers that will shift the equilibrium to the left since that will decrease the H^+ (thus the pH will go up)
Wednesday, February 9, 2011 at 9:35am by DrBob222

chemistry
i just have a question about le chatelier's principle lets say you have: A(g) + B(s) --> C(g) + D(g) does adding more of B which is a solid shift it to the right? or will it have no effect because it is a solid? thanks
Sunday, April 19, 2009 at 2:50pm by brad

Chemistry
Le Chatelier's Principle says that when a system in equilibrium is disturbed that the system will try to undo what we've done to it. So if you add acetate to it the system will try to use it. How can it do that. By shifting to the left. That increases the CH3COOH and it ...
Sunday, May 19, 2013 at 11:29pm by DrBob222

science
It works just like Le Chatelier's Principle. The higher the concentration, the more must leave to try to return the original sample to equilibrium.
Saturday, October 17, 2009 at 7:09pm by DrBob222

chemistry
Just remember this about Le Chatelier's Principle. When a system at equilibrium is disturbed it will shift so as to undo what we've done to it. So if we add heat the system will shift to use up the heat. Which way is that?
Thursday, June 7, 2012 at 10:53pm by DrBob222

CHEM-Le' Chatelier's Principle
Adding HCl adds H^+ and that drives the reaction to the right. What product and what color are formed on the right?
Wednesday, March 4, 2009 at 7:37pm by DrBob222

science
That will depend upon whether the number of moles increases or decreases in the forward direction. Are you talking about any particular reaction? Consider Le Chatelier's Principle.
Friday, January 28, 2011 at 7:12am by drwls

chemistry
This is a question on Le Chatelier's Principle. Basically that principle tells us that a system in equilibrium will try to undo what we do to it. That isn't what you read in a text but it is one way to look at it. So if we ADD H2 to the system it will try to undo that. How can...
Saturday, October 15, 2011 at 3:19pm by DrBob222

chemistry
I completely understand Le Chateliers principle but I have no idea about these questions. They're due tomorrow so fast help would be appreciated. Why did adding water to the equilibrium involving CoCl_4_^2-^ cause the color to change? Use Le Chateliers principle to explain the...
Wednesday, December 1, 2010 at 8:50pm by k

chemistry
I think you meant N2 + 3h2 ==> 2NH3 + heat Le Chatelier's Principle says that a system in equilibrium will shift to undo what we do to it. Therefore, if we cool it the reaction will shift to increase the heat we've removed. So it will shift to the right.
Saturday, April 27, 2013 at 1:38pm by DrBob222

grade 12 chemistry
I'm confused by the whole thing because I can't tell what you wrote, what you are asking, and what you copied from the text. To answer your last question, however, EVERYTHING, is an equilibrium process. You can even use equilibrium and Le Chatelier's Principle to explain why ...
Monday, July 20, 2009 at 11:24pm by DrBob222

chemistry
Would you spend a few minutes telling me what you don't understand about Le Chatelier's Principle? This is such a simple concept but students get confused. Perhaps if you tell me what is so daunting, I can understand and pitch my answers to help you understand. Just giving the...
Sunday, September 19, 2010 at 10:19pm by DrBob222

chemistry
According to Le Chatelier's Principle, an increase in pressure will shift the equilibrium to the side with fewer mols. That will be the side with NH3; therefore, additional N2 will react with additional H2 to form additional NH3.
Monday, February 27, 2012 at 9:24pm by DrBob222

Chemistry
I think the problem was constructed with the false assumption that the yield is independent of concentration and I accepted it uncritically. Le Chatelier's Principle still rules. Glad you were so alert. I checked [A]=[B]=3M with my setup and got a 75% yield, farther to the ...
Tuesday, July 22, 2008 at 1:16pm by GK

chem
IT is a bit of a stretch to use Le Chatelier's principle, but... If the area of the somach lining is less acid, then more of the aspirin will ionize to try to restablish the acid pH.
Monday, July 27, 2009 at 3:26am by bobpursley

Chemistry
In a not so esoteric statement, Le Chatelier's Principle says that an equation in equilibrium tries to UNDO what we do to it. Therefore, if we take away N2 the reaction will shift so as to increase N2. That means it shifts to the left which means H2 increases. It also means ...
Thursday, December 5, 2013 at 12:24am by DrBob222

chemistry
Two things to remember about Le Chatelier's Principle. 1. Always true--When a system in equilibrium is subjected to a stress it will shift to undo what we've done. 1a. True in gaseous systems--Increased pressure will shift the equilibrium to the side with the fewer moles of gas.
Tuesday, April 3, 2012 at 5:43pm by DrBob222

Chemistry
Le Chatelier's Principle says that a system at equilibrium (this is at equilibrium) will shift so as to UNDO what we do to it. So if you add acid, that H^+ combines with the OH^-, that reduces the OH^- (because H2O is formed) and reducing OH^- means the reaction will increase ...
Monday, October 29, 2012 at 12:40pm by DrBob222

Chemistry
Methanol, CH3OH, is produced on an industrial scale from carbon monoxide and hydrogen. At the temperatures used, gaseous methanol is formed according to the following thermochemical equation: CO(g)+ 2H2(g) <---> CH3OH(g) Ā£H = -90Kj 1. State Le Chateliers principle and ...
Friday, March 2, 2007 at 12:48pm by Adam

Chem
This is concerning Le Chatelier's Principle and Equilbrium... After I give a definition of what it means when it is said that salt is soluble and what is meant by insoluble, I am asked: Why are these terms very broad and not very accurate? Can someone start me on this... ...
Wednesday, February 21, 2007 at 10:49pm by Marisol

chemistry
You need to review Le Chatelier's Principle. I think the definition given in text books is so esoteric and it really sounds good to me. However, I find that most students don't understand it. I don't know why but here is my definition. Not nearly so esoteric but students ...
Sunday, February 26, 2012 at 1:05pm by DrBob222

Chemistry (or Physio/Biochem)
H2O + CO2 <==> H2CO3 <==> H^+ + HCO3^- So if we restrict the breathing, CO2 rises, and Le Chatelier's Principle says that will force the reaction to the right; therefore, my best guess is that the blood pH will decrease (become more acid).
Sunday, March 14, 2010 at 9:14pm by DrBob222

chemistry
Le Chatelier's Principle, in not so eloquent terms, says that a reaction at equilibrium will shift to try and undo what we've done to it. a. So if we remove CO2 it will move to the left so as to increase CO2. b. Adding H2 molecules it will shift to the right to try to use up ...
Monday, March 25, 2013 at 7:33pm by DrBob222

Le Chatelier's Principle
If the equation is : Cd2+(aq) + Cl-(aq) °Í CdCl+ What would happen when Na+ is added would it shift to the right or will there be no change/effect to the system?
Tuesday, April 19, 2011 at 7:53pm by Nicole

chemistry
Le Chatelier's Principle says, in ordinary terms, that a system in equilibrium tries to undo what we do to it. a. This system produces heat. Therefore, if we ADD heat to it it must try to get rid of it. How can it do that? Simple. By shifting to the left it USES heat and that'...
Friday, November 23, 2012 at 7:37pm by DrBob222

Chem
I have another question related to this one. The un-ionized aspirn penetrates the area of the stomach were there is less acidity thus causing irritation. How would Le Chatelier's principle explain why the irritation occurs?
Sunday, July 26, 2009 at 9:51pm by Lena

Chemistry
Le Chatelier's Principle says, in simple terms, that a system in equilibrium will try to undo what we do to it. If we add more N it will shift to use N. So it will shift to the right. If we remove NH3 it will shift to add NH3 back so it will shift to the right.
Monday, November 12, 2012 at 10:48am by DrBob222

Chemistry
Le Chatelier's Principle states, in simple terms, that a reaction at equilibrium will shift to undo what we've done to it. So adding Cr^+3 (from CrCl3) will make it move so as to reduce Cr^+3. Isn't that to the left in order to use Cr^+3? If HCl is added, it will neutralize ...
Sunday, February 27, 2011 at 11:46pm by DrBob222

chemistry
Using the Le Chatelier's principle, predict the direction of the net reaction in each of the following equilibrium systems, as a result of increasing the pressure at constant temperature. a)N2(g) + O2(g) ==> 2NO(g) <== b)PCl5 ==> PCl3(g) + Cl2(g) <== c)CO(g) + Cl2(...
Monday, June 14, 2010 at 6:05pm by karl

chemistry
Are you sure the question isn't AgCl --> Ag^+ + Cl^- Le Chatelier's Principle tells us that when we do something to a reaction in equilibrium, the reaction will shift in such as way as to undo what has been done. So if we add Cl^- to the solution, the reaction will try to ...
Monday, July 19, 2010 at 3:22pm by DrBob222

Chemistry
Le Chatelier's Principle says that a system in equilibrium will try to undo what we do to it. When volume is reduced that means pressure must be increased so the system will shift to the side with the fewer mols of gas. In this reaction there are 4 mols gas on the left and 4 ...
Wednesday, February 27, 2013 at 9:15pm by DrBo222

chemistry
Read about Le Chatelier's Principle. Cocn: shifts to side AWAY from added reactant or product. Pressure: shifts to side with smaller number of moles for increase in P. Temperature: Shifts to side away from added heat.
Saturday, May 28, 2011 at 9:53am by DrBob222

Chemistry- Please Help!!
Ca(IO3)2 ==> Ca^2+ + 2IO3^- The easy way to remember what happens is to remember Le Chatelier's principle. It says that a system is equilibrium will try to undo what we do to it. Therefore, if we increase Ca^2+ (whether starting or not) the reaction will try to remove Ca2+ ...
Sunday, July 28, 2013 at 10:46pm by DrBob222

science - chemistry (Le Chatelier's)
By your question, it is evident you missed the point of Le Chatelier: Reaction dynamics tend to undo a reaction in equilibrium if a reaction condition (temp, pressure, concentration) has been altered. This article explains it well, somewhat wordy, but well: http://en.wikipedia...
Saturday, August 25, 2007 at 4:35am by bobpursley

Organic Chemistry
The purpose of adding concentrated H2SO4 to the Diels-Alder adduct was to: A. hydrolyze the product to make the product precipitate more easily B. catalyze the diels alder reaction C. use Le Chatelierís principle to drive the reaction to completion D. to quench excess reagents...
Friday, March 6, 2009 at 5:18am by nilee

Chemistry
It is impossible to draw diagrams on the board to show you how this works and words sometimes fail to communicate properly; however, remember Le Chatelier's Principle. A reaction at equilibrium will try to UNDO what we do to it (although Le Chatelier's statement was much more ...
Sunday, November 28, 2010 at 4:02pm by DrBob222

organic
I don't know how to answer your question; it all depends upon what you call a high yield. I think a typical esterification may be about 65-80%. They reaction can be driven to the right (Le Chatelier's principle) by using an excess of alcohol AND/OR removing the ester by some ...
Wednesday, February 10, 2010 at 2:58pm by DrBob222

chemistry
Add Cl^- (the common ion effect--just a practical example of Le Chatelier's Principle) puts the stress on the equilibrium, the reaction shifts to as to relieve the stress which means that the reaction must try to reduce the Cl^-. The only way it can do that is to shift to the ...
Sunday, January 24, 2010 at 5:07pm by DrBob222

Chemistry- Le chatelier's Principle
HOw would you predict the colour change or changes in number of states for the following: To a solution of 5 drops of 0.3 M K2CrO4 ans 2 drops of 0.3M NaOH add a drop at a time 0.1 M Ba(NO3)2 until a change is noticed. Given: BaCrO4(s) ---> Ba2+ + CrO42- 2CrO42-+2H+ --->...
Wednesday, March 4, 2009 at 9:27pm by meme

chem
Did you do the experiment with KClO3.What happened to the oxygen? Le Chatelier's Principle, stated a little differently than the esoteric manner in which it is portrayed in texts, is this: When a system in equilibrium is subjected to a stress,the reaction will try to undo what...
Wednesday, February 1, 2012 at 9:26pm by DrBob222

chemistry
Have you read anything about Le Chatelier's Principle. That principle states that when a system in equilibrium is subjected to a stress, the system will react (shift equilibrium) in such a way so as to remove the stress. So what do we have? We have a system in equilibrium. We ...
Monday, March 31, 2008 at 2:43pm by DrBob222

Chemistry - Le Chatelier's Principle
I don't know what it is you don't understand. Frankly you seem to understand it very well. You add H3O^+ and the rxn shifts to the right producing more dichromate which is what you want. The equation is already there. That is the initial equation, the intermediate equation, ...
Sunday, March 9, 2014 at 1:30pm by DrBob222

Chemistry - Le Chatelier's principle(help)
No, it is not correct. Let me restate Le Chatelier's Principle but in slightly different words. In a system in dynamic equilibrium the reaction will shift in the direction to undo what we've done to it. So, yes, the water is on the product side, but starting here I do it ...
Tuesday, March 22, 2011 at 6:13am by DrBob222

Chemistry
Consider the following buffer equilibrium: HF (high concentration) + H2O <--> H3O+ (low concentration) + F- ( high concentration) Using Le Chatelier's Principle, explain what happens to the pH of the buffer solution when a small amount of NaOH is added. Wouldn't OH- ...
Thursday, June 3, 2010 at 1:49pm by sh

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