{"id":7047,"date":"2014-05-28T16:59:12","date_gmt":"2014-05-28T16:59:12","guid":{"rendered":"https:\/\/schooltutoring.com\/help\/?p=7047"},"modified":"2014-12-02T08:25:29","modified_gmt":"2014-12-02T08:25:29","slug":"chemistry-review-of-equilibrium","status":"publish","type":"post","link":"https:\/\/schooltutoring.com\/help\/chemistry-review-of-equilibrium\/","title":{"rendered":"Chemistry Review of Equilibrium"},"content":{"rendered":"

Overview:<\/h3>\n

Chemical equilibrium refers to the state in which opposite processes balance each other so that one does not occur more than the other.\u00a0 Many chemical processes exist which are reversible.\u00a0 Equilibrium does not mean that reactions come to a stop, but that they balance dynamically.<\/p>\n

Reversible Reactions<\/h3>\n

Reversible reactions are chemical processes that oppose one another.\u00a0 The molecule NO2<\/sub> is a brown gas called nitrogen dioxide, a major component of smog that is in automobile exhaust.\u00a0 It is converted into another component of smog, a colorless gas called dinitrogen tetroxide (N2<\/sub>O4<\/sub>). The colorless dinitrogen tetroxide is converted back to nitrogen dioxide in an opposing reaction.\u00a0 If a sample of nitrogen dioxide is sealed, so that the reaction can continue, the brown color of the original sample will fade as the concentration of nitrogen dioxide is lowered, but it will not fade completely.<\/p>\n\n\n\n
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Figure 1:\u00a0 The double half-arrow going in both directions in a symbol of a reversible reaction.<\/p>\n<\/div>\n<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n

\"monohybridcross\"<\/a><\/p>\n

Dynamic Equilibrium<\/h3>\n

Imagine that 20 passengers leave the main bus terminal.\u00a0 At the first stop, two get off the bus, but two more riders come aboard.\u00a0 At the next stop, one rider leaves the bus, and another rider gets on the bus at the following stop.\u00a0 At the fourth stop, three riders get on the bus, but another three leave.\u00a0 There are still 20 passengers on the bus, because the same number have come aboard as have left.\u00a0 There is a lot of activity, even though the overall number of passengers is unchanged.\u00a0 This is similar to the process of dynamic equilibrium, as there is a great deal of activity at the molecular level, yet the substances themselves are not static.<\/p>\n\n\n\n
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Figure 2:\u00a0 The surfboarder constantly changes position to balance while riding the wave.\u00a0This is an example of dynamic equilibrium.<\/p>\n<\/div>\n<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n

\"monohybridcross\"<\/a><\/p>\n

Le Chatelier\u2019s Principle<\/h3>\n

Even though a chemical reaction is at equilibrium, it can be shifted away from equilibrium by changing conditions.\u00a0 Le Chatelier\u2019s principle states that if a system is at equilibrium and something happens to disturb the equilibrium, the system will tend to correct in the direction to compensate for the change in conditions.\u00a0 Imagine a tightrope walker using a pole as a balance tool.\u00a0 The pole can be tilted one way or another to compensate for movement to the left or to the right.<\/p>\n

Changes in Concentration, Temperature and Pressure<\/h3>\n

Some of the changes in a system that can disturb equilibrium are changes in concentration, temperature, and pressure.\u00a0 Suppose that the concentration of nitrogen dioxide is increased in the smog solution.\u00a0 That will make more nitrogen dioxide available to change, so that the reaction will consume more of it, to bring the system back to equilibrium.\u00a0 Similarly, changes in pressure or temperature will shift the system towards one direction or another.<\/p>\n

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Overview: Chemical equilibrium refers to the state in which opposite processes balance each other so that one does not occur more than the other.\u00a0 Many chemical processes exist which are reversible.\u00a0 Equilibrium does not mean that reactions come to a stop, but that they balance dynamically. Reversible Reactions Reversible reactions are chemical processes that oppose […]<\/p>\n","protected":false},"author":22,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"_acf_changed":false,"inline_featured_image":false,"footnotes":""},"categories":[5],"tags":[2700,595,2701],"class_list":["post-7047","post","type-post","status-publish","format-standard","hentry","category-chemistry","tag-dynamic-equilibrium","tag-equilibrium","tag-le-chateliers-principle"],"acf":[],"aioseo_notices":[],"_links":{"self":[{"href":"https:\/\/schooltutoring.com\/help\/wp-json\/wp\/v2\/posts\/7047","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/schooltutoring.com\/help\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/schooltutoring.com\/help\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/schooltutoring.com\/help\/wp-json\/wp\/v2\/users\/22"}],"replies":[{"embeddable":true,"href":"https:\/\/schooltutoring.com\/help\/wp-json\/wp\/v2\/comments?post=7047"}],"version-history":[{"count":0,"href":"https:\/\/schooltutoring.com\/help\/wp-json\/wp\/v2\/posts\/7047\/revisions"}],"wp:attachment":[{"href":"https:\/\/schooltutoring.com\/help\/wp-json\/wp\/v2\/media?parent=7047"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/schooltutoring.com\/help\/wp-json\/wp\/v2\/categories?post=7047"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/schooltutoring.com\/help\/wp-json\/wp\/v2\/tags?post=7047"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}