{"id":14563,"date":"2022-11-21T10:00:37","date_gmt":"2022-11-21T04:30:37","guid":{"rendered":"https:\/\/www.aplustopper.com\/?p=14563"},"modified":"2022-11-21T10:13:19","modified_gmt":"2022-11-21T04:43:19","slug":"collision-theory-chemistry","status":"publish","type":"post","link":"https:\/\/www.aplustopper.com\/collision-theory-chemistry\/","title":{"rendered":"What is the collision theory in chemistry?"},"content":{"rendered":"
<\/p>\n
People also ask<\/strong><\/p>\n III. A hydrogen molecule and a bromine molecule collide with their total energy greater than or equal to the activation energy <\/strong>and with the correct orientation,<\/strong> as shown in Figure. An effective collision<\/strong> occurs. Activation energy:<\/strong><\/p>\n Relationship between the frequency of collision and the activation energy with the rate of reaction:<\/strong><\/p>\n <\/p>\n","protected":false},"excerpt":{"rendered":" What is the collision theory in chemistry? According to the kinetic theory of matter, particles of matter are in continuous motion and constantly in collision with each other. For a reaction to occur, the particles of the reactants (atoms, molecules or ions) must touch each other through collision for bond breaking and bond formation […]<\/p>\n","protected":false},"author":3,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_genesis_hide_title":false,"_genesis_hide_breadcrumbs":false,"_genesis_hide_singular_image":false,"_genesis_hide_footer_widgets":false,"_genesis_custom_body_class":"","_genesis_custom_post_class":"","_genesis_layout":"","footnotes":""},"categories":[84],"tags":[5612,5614,5615,5616,5617,5613,5543,5609,5507,5623,5621,5611,5610,5622],"yoast_head":"\n\n
\n\n
\n Situations<\/strong><\/td>\n Will it result in a reaction?<\/strong><\/td>\n<\/tr>\n \n I. A hydrogen molecule and a bromine molecule collide with the correct orientation<\/strong> but the energy<\/strong> of the colliding particles is less than the activation energy,<\/strong> as shown in Figure.
\n<\/td>\nThis collision will not<\/strong> result in a reaction\u00a0(Ineffective collision)<\/strong><\/td>\n<\/tr>\n \n II. A hydrogen molecule and a bromine molecule collide with their total energy greater than or equal to the activation energy <\/strong>but with the wrong orientation,<\/strong> as shown in Figure.
\n<\/td>\nThis collision will not<\/strong> result in a reaction (Ineffective collision)<\/strong><\/td>\n<\/tr>\n \n \n
\n<\/p>\n<\/td>\n\n
\nThis collision results in a reaction<\/strong> to form hydrogen bromide molecules.<\/p>\n<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\nWhat is Activation Energy?<\/h2>\n
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\n<\/li>\nWhat is the relationship between activation energy and collision theory?<\/strong><\/h2>\n
\n
\n(a) frequency<\/strong> of collision
\n(b) magnitude<\/strong> of activation energy<\/li>\n
\n(a) If the frequency of collision<\/strong> for a reaction is high,<\/strong> then the frequency of effective collision<\/strong> that can result in a reaction is also high.<\/strong>
\n(b) Hence, the rate of reaction is high, and vice versa
\n(c) Figure illustrates this relationship.
\n<\/li>\n
\n(a) The values of are different for different reactions.
\n(b) If the activation energy<\/strong> of a reaction is high,<\/strong> fewer number of colliding particles are able to achieve this high energy. Hence, the frequency of effective collision <\/strong>is low.<\/strong> As a result, the rate<\/strong> of reaction is low.<\/strong>
\n(c) Conversely, if the activation energy<\/strong> of a reaction is low,<\/strong> the rate<\/strong> of reaction is high.<\/strong><\/li>\n