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The Haber Process - 4 views

www.chm.bris.ac.uk/...haber.htm

shared by james huang on 14 Feb 13 - No Cached

NH3 is oxidised to NO2 and NO3,
- james huang on 14 Feb 13
  
  How does the oxidation of NH3 to form NO2 and NO3 signficant in real life?
  
  <div class="cArrow"> </div><div class="cContentInner">How does the oxidation of NH3 to form NO2 and NO3 signficant in real life?</div>
  
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N2 + 3 H2 2 NH3
- james huang on 14 Feb 13
  
  This represents a chemical equation that displays the reaction between nitrogen and hydrogen to form ammonia.
  
  <div class="cArrow"> </div><div class="cContentInner">This represents a chemical equation that displays the reaction between nitrogen and hydrogen to form ammonia.</div>
  
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chlorine gas in 1915 at the battle of Ypres, where it took the unsuspecting (and unprotected) French troops by surprise - killing over 10,000 of them in in few minutes.
- james huang on 14 Feb 13
  
  How does the discovery of chlorine as a poison affect the knowledge of chlorine and how to use it in the future?
  
  <div class="cArrow"> </div><div class="cContentInner">How does the discovery of chlorine as a poison affect the knowledge of chlorine and how to use it in the future?</div>
  
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Equillibrium (Explanation and Examples) - 1 views

ic.galegroup.com/...ReferenceDetailsWindow

shared by james huang on 14 Feb 13 - No Cached

the reaction continues to completion--the reactants are consumed and only products are present at the completion of the reaction.
- james huang on 14 Feb 13
  
  Not all reactions can complete to completion. Certain characteristics and processes allow a reaction to have the full amount of products and zero reactants left.
  
  <div class="cArrow"> </div><div class="cContentInner">Not all reactions can complete to completion. Certain characteristics and processes allow a reaction to have the full amount of products and zero reactants left.</div>
  
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products accumulate, and eventually stops even though there may still be a significant amount of the reactants present.
- james huang on 14 Feb 13
  
  The amount of products and reactants that are left varies base don reactants and products. As learned in chemical kinetics, some reactions can not produce the full amount of products because they do not have correct orientation or do not meet the requirements of the activation energy.
  
  <div class="cArrow"> </div><div class="cContentInner">The amount of products and reactants that are left varies base don reactants and products. As learned in chemical kinetics, some reactions can not produce the full amount of products because they do not have correct orientation or do not meet the requirements of the activation energy.</div>
  
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A and B molecules continue to be consumed at a decreasing rate. But additional A and B molecules are being produced in the reverse reaction at an increasing rate. At some point, A and B are being produced in the reverse reaction as quickly as they are being used up in the forward reaction. At this point the amounts of reactant and product remain constant, and the reaction appears to cease. The reaction is now at equilibrium.
- james huang on 14 Feb 13
  
  The reaction appears to cease. But it doesnt. This is because the forward and reverse reactions are occuring at the same rates and it seems like the reaction has ceased. However, this only proves that the reaction is at equilibrium.
  
  <div class="cArrow"> </div><div class="cContentInner">The reaction appears to cease. But it doesnt. This is because the forward and reverse reactions are occuring at the same rates and it seems like the reaction has ceased. However, this only proves that the reaction is at equilibrium.</div>
  
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...6 more annotations...
The resulting zero in the denominator of the Ksp equation means that its solubility constant is undefined.
- james huang on 14 Feb 13
  
  Considering the fact that solubility constant is undefined, how is the solubility displayed in an experiment?
  
  <div class="cArrow"> </div><div class="cContentInner">Considering the fact that solubility constant is undefined, how is the solubility displayed in an experiment?</div>
  
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For instance for the heterogeneous reaction of solid (s) carbon and gaseous (g) oxygen: 2C(s) + O2(g) ↔ 2CO(g), the equilibrium constant equation is: K = (PCO)2 / (PO2), and the amount of carbon monoxide (CO) formed at equilibrium is independent of the amount of carbon initially present.
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When nitrogen and hydrogen are mixed and their reaction is triggered, very little ammonia is formed.
- james huang on 14 Feb 13
  
  The formation of nitrogen and hydrogen forming very little ammonia is an example of an equilbrium process.
  
  <div class="cArrow"> </div><div class="cContentInner">The formation of nitrogen and hydrogen forming very little ammonia is an example of an equilbrium process.</div>
  
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an acid dissolves completely in solution, it releases a hydrogen ion (H+) that gives the solution its acidic property.
- james huang on 14 Feb 13
  
  Does this mean that the increase in hydrogen ions gives the solution a low pH?
  
  <div class="cArrow"> </div><div class="cContentInner">Does this mean that the increase in hydrogen ions gives the solution a low pH?</div>
  
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capable of reacting with each other are mixed together
- james huang on 14 Feb 13
  
  How do we know which chemicals are being capable of reacting with each other when mixed?
  
  <div class="cArrow"> </div><div class="cContentInner">How do we know which chemicals are being capable of reacting with each other when mixed?</div>
  
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an equilibrium constant with a large value such as 2 x 107 indicates that the product is favored to such an extent that, at equilibrium, virtually all of the hydrogen and chlorine gas have reacted to form gaseous hydrogen chloride.
- james huang on 14 Feb 13
  
  What would an equilbrium constant with a small value indicate on the product favored?
  
  <div class="cArrow"> </div><div class="cContentInner">What would an equilbrium constant with a small value indicate on the product favored?</div>
  
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Gale Science In Context - Document - 14 views

ic.galegroup.com/...DocumentToolsPortletWindow

shared by james huang on 14 Feb 13 - No Cached

When ammonium hydroxide is treated with iodine crystals, an explosive brown solid, nitrogen triiodide, is formed.
- james huang on 14 Feb 13
  
  Example of chemical reaction with the use of ammonia.
  
  <div class="cArrow"> </div><div class="cContentInner">Example of chemical reaction with the use of ammonia.</div>
  
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where it may have originally formed from metal nitrides reacting with water.
- james huang on 14 Feb 13
  
  How do we know the origins of why liquid and solid ammonia exist on other planets? Where is the proof regarding this theory?
  
  <div class="cArrow"> </div><div class="cContentInner">How do we know the origins of why liquid and solid ammonia exist on other planets? Where is the proof regarding this theory?</div>
  
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Ammonia will continue to be important for agriculture and for the whole nitrogen chemicals industry.
- james huang on 14 Feb 13
  
  Ammonia and its impact in the future. Ammonia has served many purpose in the past, present and in the years to come.
  
  <div class="cArrow"> </div><div class="cContentInner">Ammonia and its impact in the future. Ammonia has served many purpose in the past, present and in the years to come.</div>
  
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...1 more annotation...
ammonia is able to react with acidic gases such as nitrogen oxides and sulfur oxides to form ammonium salts
- james huang on 14 Feb 13
  
  What basic properties allow Ammonia to react with acidic gases and form salts?
  
  <div class="cArrow"> </div><div class="cContentInner">What basic properties allow Ammonia to react with acidic gases and form salts?</div>
  
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Gale Science In Context - Document - 2 views

ic.galegroup.com/...DocumentToolsPortletWindow

shared by james huang on 14 Feb 13 - No Cached

such as Jupiter, where it may have originally formed from metal nitrides reacting with water.
- james huang on 14 Feb 13
  
  How do we know where liquid and solid ammonia have have formed? Do we know that these theories are correct?
  
  <div class="cArrow"> </div><div class="cContentInner">How do we know where liquid and solid ammonia have have formed? Do we know that these theories are correct?</div>
  
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ammonia is able to react with acidic gases such as nitrogen oxides and sulfur oxides to form ammonium salts
- james huang on 14 Feb 13
  
  Ammonia's special chemical properties allow it to react with acidic gases to form salts.
  
  <div class="cArrow"> </div><div class="cContentInner">Ammonia's special chemical properties allow it to react with acidic gases to form salts.</div>
  
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