Degenerated reaction of calcium carbonate obtained by the\npollutant sulfur dioxide. The amount of sulfur dioxide in the air depends on\nthe rate of reaction. SO2<\/sub> is an acidic oxide, it combines with water\nvapor to produce H2<\/sub>SO3<\/sub>. The reaction is as follows:<\/p>\n\n\n\n SO2 <\/sub>+ H2<\/sub>O = H2<\/sub>SO3<\/sub><\/p>\n\n\n\n Then calcium carbonate reacts with sulfurous acid<\/p>\n\n\n\n CaCO3<\/sub> + H2<\/sub>SO3<\/sub> = CaSO3<\/sub> + CO2<\/sub> + H2<\/sub>O<\/p>\n\n\n\n The concentration of Sulfur dioxide is high in a polluted\nair. In the polluted air the calcium carbonate more degenerates as compared to less\npolluted air.<\/p>\n\n\n\n On the other hand, Phosphorus burns at a great rate in a pure\noxygen than in air.<\/p>\n\n\n\n Unit<\/strong><\/p>\n\n\n\n Concentration is usually measured in moles per liter.<\/p>\n\n\n\n It is a speed at which chemical reaction proceeds. Reactants\nare converted into products. It is expressed in terms of concentration (amount\nper unit time) of the product. It means the concentration of the reactant is\nconsumed in a unit of time. <\/p>\n\n\n\n Rate= change in concentration\/change\nin time<\/p>\n\n\n\n Nature of Reactants<\/strong><\/p>\n\n\n\n Nature of the reacting substance has a major contribution in\nthe chemical reaction. Same condition\nreactions may have different rates depending on their identity of reactants.\nFor example, the small section of iron metal and sodium is exposed to air, iron\nhave a little effect but the sodium reacts completely with air overnight. The hydrogen gas and a base is formed by the\nreaction of active metal calcium and sodium. Both react with water. Thus,\ncalcium reacts at the moderate rate whereas, sodium reacts so quickly and its\ntemperature is too high, due to this, the reaction is so much explosive.<\/p>\n\n\n\n Definition of the\nConcentration<\/strong><\/p>\n\n\n\n A quantitative measure of the amount of solute dissolved in a\ngiven quantity of solution. It is expressed in terms of mass per unit volume.<\/p>\n\n\n\n Chemical Kinetics<\/strong><\/p>\n\n\n\n Chemical kinetics plays a great role in physical chemistry.\nIt involves the study of the reaction rate. It deals with the effect of\ndifferent variables e.g. temperature, concentration.<\/p>\n\n\n\n Factors That Affect the Rate of Reaction<\/strong><\/p>\n\n\n\n Relationship between\nthe Rate of Reaction and Concentration of Reactants<\/strong><\/p>\n\n\n\n There is a mathematical relationship between the rate of\nreaction and the concentration of reactants. The rate of reaction is directly\nproportional to the number of collisions per second between the reactant\nmolecules. If the concentration decreases with time the number of collisions\nalso decreases. It depends upon the frequency of the total number of collisions.\nIf the frequency increases then the rate of reaction also increases. The\ncomposition of this reaction is known as chemical\nkinetics<\/strong>. <\/p>\n\n\n\n Higher concentration = More collisions<\/strong><\/p>\n\n\n\n Reaction involving two\nparticles<\/strong><\/p>\n\n\n\n According to the collision theory, the reaction is the same whether the collision between two different particles or collisions between the same particles. Particles first collide in any reaction, whether both particles are in solution or one in solution or other one is solid. On the higher concentration, higher will be the collision.<\/p>\n\n\n\n Reaction involving one\nparticle<\/strong><\/p>\n\n\n\n The orientation of the collision of the molecules is\nirrelevant. Suppose that at any one time 2 in a million particles have enough\nenergy to equal or exceed the activation energy. If you have 300 million\nparticles then 300 of them would react. By doubling the concentration, double\nwill be the rate of reaction.<\/p>\n\n\n\n Following are the cases where the concentration doesn\u2019t\naffect the rate of reaction<\/p>\n\n\n\n Working of catalyst on\nits maximum capacity<\/strong><\/p>\n\n\n\n Suppose, a small amount of solid catalyst is using in a\nreaction and concentration of the reactant in a solution is too high. So, the\nreacting particles were muddled up on a catalyst surface. If we increase the\nconcentration of reactants then it also doesn’t have any effect because the\ncatalyst is already working on its maximum capacity. <\/p>\n\n\n\n Multi-step reactions<\/strong><\/p>\n\n\n\n Suppose we react to different variables. Some are of high spend of some of slow. The reaction occurs in a series of small paces. If A and B react together in these different steps of the reaction.<\/p>\n\n\n\n By increasing the concentration of A, how fast reaction\ndissociates A to make X and Y.<\/p>\n\n\n\n By decreasing the concentration it will reduce the rate of\nthe second reaction.<\/p>\n\n\n\n By increasing the\nconcentration of reactant or product<\/strong><\/p>\n\n\n\n Add N2 <\/sub>(reactant) = shift Right (toward products)<\/p>\n\n\n\n Add H2 <\/sub>(reactant) = shift Right (toward products)<\/p>\n\n\n\n Add NH3 <\/sub>(reactant) = shift left (toward reactants)<\/p>\n\n\n\n By decreasing the concentration\nof reactant or product<\/strong><\/p>\n\n\n\n Remove N2<\/sub> (reactant) = shift Left (toward reactants)<\/p>\n\n\n\n Remove H2<\/sub> (reactant) = shift Left (toward reactants)<\/p>\n\n\n\n Remove NH3 <\/sub>(product) = shift Right (toward products)<\/p>\n\n\n\n How to find the\nconcentration of reactants<\/strong><\/p>\n\n\n\n To find the concentration reactants, the conversion will\nstill the same throughout the reaction. Suppose a reaction between A and B. the\nreaction rate is zero concerning B. The rate of reaction is independent of the\nconcentration of reactant B.<\/p>\n\n\n\n Concentration of\nreactants of solid and liquid<\/strong><\/p>\n\n\n\n The reaction\nrate of solids and liquids is increasing by increasing the surface area. If the\nsurface area of solid is increasing then there is a decrease in particle size.<\/p>\n\n\n\n Concentration of\nreactant of gases<\/strong><\/p>\n\n\n\n We will ignore the pressure of solids and liquids because\nthere pressure is so small but we will not ignore the pressure of reaction of\ngases that contain gases. There is a remarkable difference between the pressure\nof reaction of solid, liquid and gases.<\/p>\n\n\n\n If we write the reactants and products in two sides of the\nchemical equation then the reaction is carried out in a single container, both\nreactants and products are in a same container. So, that we cannot assume the\nincreasing pressure of products or reactants. Therefore, the pressure is\nchanged in a reaction and this pressure is caused by the change of volume in a\nreaction container. Volume of the container is changed but it doesn\u2019t directly\nchange the number of particles in a container. \nVolume of each unit is changed and it also changes the pressure of the\nreaction.<\/p>\n\n\n\n Volume increase is number of collisions per unit of surface area decreases lower the pressure<\/p>\n\n\n\n There are less number of molecules of reactant and products\nper unit volume.<\/p>\n\n\n\n As we know, change in concentration has an effect to an equilibrium. We need to be very careful when we increase the concentration of both reactant and product molecules. <\/p>\n\n\n\n There is 1 molecule of gaseous product and 2 molecules of gaseous reactant. Thus, forward reaction have a greater effect by increasing concentration. This unbalanced on the reaction will affect the equilibrium. Change occurs due to change in pressure. There is another example for gaseous reactants.<\/p>\n\n\n\n It contain 2 molecules of gaseous reactant and 2 molecules of\ngaseous product. By increasing the pressure, the rate of forward reaction\nincreases and there is a great effect on reverse reaction. In case of both\nreaction rates are equal then equilibrium is not shifted.<\/p>\n\n\n\n Changing pressure has no effect on equilibrium if the number\nof gaseous reactant molecules and gaseous product molecules are equal.<\/p>\n\n\n\n So, it is concluded that if the number of gaseous reactant\nand gaseous product are same then there is no effect on an equilibrium but if\nthe number of molecules of gaseous reactant and gaseous product are different\nthen there is a great effect on an equilibrium.<\/p>\n\n\n\n The increase in the concentration of reactants, the rate of reaction increases. Ions and molecules interact to form a new compound on increasing the concentration. The decrease in the concentration of reactants, fewer molecules and ions are present and the rate of reaction decreases. In the reaction of gases, if we increase the pressure there … Read more<\/a><\/p>\n","protected":false},"author":6,"featured_media":0,"comment_status":"closed","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"rating_form_position":"","rating_results_position":"","mr_structured_data_type":""},"categories":[1],"tags":[],"multi-rating":{"mr_rating_results":[{"adjusted_star_result":0,"star_result":0,"total_max_option_value":5,"adjusted_score_result":0,"score_result":0,"percentage_result":0,"adjusted_percentage_result":0,"count":0,"post_id":1167}]},"_links":{"self":[{"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/posts\/1167"}],"collection":[{"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/users\/6"}],"replies":[{"embeddable":true,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/comments?post=1167"}],"version-history":[{"count":7,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/posts\/1167\/revisions"}],"predecessor-version":[{"id":1308,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/posts\/1167\/revisions\/1308"}],"wp:attachment":[{"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/media?parent=1167"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/categories?post=1167"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/tags?post=1167"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Definition of the Reactant<\/h2>\n\n\n\n
![\"\"](\"https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-33.png\")
<\/figure><\/div>\n\n\n\nCONCENTRATION AFFECT THE RATE OF REACTION<\/h2>\n\n\n\n
![\"\"](\"https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-34.png\")
<\/figure><\/div>\n\n\n\nCONCENTRATION DOESN\u2019T AFFECT THE RATE OF REACTION<\/h2>\n\n\n\n
![\"\"](\"https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-35.png\")
<\/figure><\/div>\n\n\n\nEFFECT OF CONCENTRATION<\/h2>\n\n\n\n
![\"\"](\"https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-36.png\")
<\/figure><\/div>\n\n\n\n![\"\"](\"https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-37.png\")
<\/figure>\n\n\n\n![\"\"](\"https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-38.png\")
<\/figure>\n\n\n\nREFERENCES<\/h4>\n\n\n\n