{"id":959,"date":"2019-10-14T14:33:15","date_gmt":"2019-10-14T14:33:15","guid":{"rendered":"http:\/\/chemdictionary.org\/?p=959"},"modified":"2019-10-14T14:33:22","modified_gmt":"2019-10-14T14:33:22","slug":"charless-law","status":"publish","type":"post","link":"https:\/\/chemdictionary.org\/charless-law\/","title":{"rendered":"Charles&#8217;s Law"},"content":{"rendered":"\n<h2><strong>Definition<\/strong><\/h2>\n\n\n\n<p>It is a quantitative relationship between temperature and volume of a gas. It was given by French scientist J. Charles in 1787. <\/p>\n\n\n\n<p>According to this law,\nthe volume of the given mass of a gas is directly proportional to the absolute\ntemperature when the pressure is kept constant.<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; V&nbsp;&nbsp;&nbsp; \u03b1&nbsp;&nbsp; T&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; (when pressure and number\nof moles are constant)<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; V&nbsp;&nbsp;&nbsp; =&nbsp;&nbsp;\nkT<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; V\/T&nbsp; &nbsp;&nbsp;=&nbsp;&nbsp;&nbsp; k<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; &nbsp;&nbsp;&nbsp;&nbsp;<\/p>\n\n\n\n<p>If the temperature is\nchanged from T<sub>1<\/sub> to T<sub>2<\/sub> and volume changes from V<sub>1<\/sub>\nto V<sub>2<\/sub>, then <\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; V <sub>1<\/sub>\/ T<sub>1<\/sub> &nbsp;&nbsp;=&nbsp;&nbsp;&nbsp; k and&nbsp;&nbsp;&nbsp; V<sub>2<\/sub>&nbsp;\/ T<sub>2<\/sub> &nbsp;&nbsp;=&nbsp;&nbsp;&nbsp;k<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp; So,&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; V <sub>1<\/sub>\/ T<sub>1<\/sub> &nbsp;&nbsp;=&nbsp;&nbsp;&nbsp;&nbsp; V<sub>2<\/sub>\/ T<sub>2<\/sub>&nbsp;<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;<\/p>\n\n\n\n<p>V<sub>1<\/sub> = initial\nvolume <\/p>\n\n\n\n<p>T<sub>1 <\/sub>= initial\ntemperature<\/p>\n\n\n\n<p>V<sub>2<\/sub>= final\nvolume <\/p>\n\n\n\n<p>T<sub>2<\/sub> = final\ntemperature <\/p>\n\n\n\n<p>It can be written as <\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; V<sub>2<\/sub> = V<sub>1<\/sub>\n(T<sub>2<\/sub> \/ T<sub>1<\/sub>)<\/p>\n\n\n\n<p>V<sub>2<\/sub>= final\nvolume <\/p>\n\n\n\n<p>T<sub>2<\/sub> = final\ntemperature <\/p>\n\n\n\n<p>V<sub>1<\/sub> = initial\nvolume <\/p>\n\n\n\n<p>T<sub>1 <\/sub>= initial\ntemperature<\/p>\n\n\n\n<p>The ratio of volume to\ntemperature remains constant for same amount of gas at same pressure.<\/p>\n\n\n\n<p>The law determines the linear relationship between volume and temperature. The temperatures are measured in Kelvin, which is SI unit of temperature.<\/p>\n\n\n\n<h2><strong>Explanation\n<\/strong><\/h2>\n\n\n\n<p>James Clerk Maxwell claimed that a space is occupied by a gas is dependent upon the motion of its particles. The particles continuously collide with the walls of the container. This rapid collision exerts force on the container surface, that force creates pressure.<\/p>\n\n\n\n<p>The impact of this force is inconsequential but collectively the collision exerts pressure on the surface of the container. Gas pressure is proportional to the magnitude of collision and the force. So, the more collision results in higher pressure. However, it is also realized that the pressure is increasing with the increase in temperature provided the volume of the container kept constant. This behaviour is evident in the air pumps that churn out hot air when their piston is periodically pushed and pulled. <\/p>\n\n\n\n<p>Volume increases in heated gas because volume isn\u2019t bounded as ball expands pressure is also increases. The rubber expands as more hot gas is pumped in and the exhilarated particles bounce and push on the inside of the surface, pushing it outward. They obey Charles\u2019s law [1].<\/p>\n\n\n\n<p><strong>Experimental\nVerification<\/strong><\/p>\n\n\n\n<p>Let us consider a certain\namount of a gas enclosed in a cylinder fitted with a moveable piston. The\nvolume of the gas is V<sub>1<\/sub> and its temperature is T<sub>1<\/sub>. When\nthe gas in the cylinder is heated both volume and the temperature of the gas\nincrease. The new values of volume and temperature are V<sub>2<\/sub> and T<sub>2<\/sub>\nrespectively.<\/p>\n\n\n\n<p><strong>Example\n<\/strong><\/p>\n\n\n\n<p>If 250 cm<sup>3<\/sup> of\nhydrogen is cooled from 127<sup>o<\/sup>C to -27<sup>o<\/sup>C by maintaining the\npressure constant. Calculate the new volume of the gas at low temperature.<\/p>\n\n\n\n<p><strong>Solution\n<\/strong><\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; Pressure has been kept constant so this gas is obeying\nthe Charles\u2019s law<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp; &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; Initial\nvolume (V<sub>1<\/sub>)&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; &nbsp;&nbsp;&nbsp;&nbsp;=250cm<sub>3<\/sub> =0.25 dm<sup>3<\/sup><\/p>\n\n\n\n<p><sub>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; <\/sub>Initial temperature (T<sub>1<\/sub>)&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; = 127<sup>O<\/sup>C +273 K =400K<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; Final temperature (T<sub>2<\/sub>)&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; = -27<sup>O<\/sup>C +273 K = 246 K<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; Final volume (V<sub>2<\/sub>)&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; = \u0241<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; According to Charles\u2019s law <\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; V <sub>1<\/sub>\/ T1 &nbsp;&nbsp;=&nbsp;&nbsp;&nbsp;&nbsp; V<sub>2<\/sub>\/ T<sub>2<\/sub>&nbsp; &nbsp;&nbsp;<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; V<sub>2<\/sub>=&nbsp;&nbsp; V<sub>1<\/sub> x T<sub>2<\/sub> \/  T1<\/p>\n\n\n\n<p><sub>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;<\/sub>&nbsp; V<sub>2<\/sub> =&nbsp;&nbsp; 0.25 dm<sup>3<\/sup> x 246K \/400K&nbsp;&nbsp;= 0.153 dm<sup>3<\/sup>&nbsp;&nbsp;     = 153 cm<sup>3<\/sup> Answer<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;<\/p>\n\n\n\n<p>So, by decreasing the temperature the volume of the gas has decreased at constant temperature.<\/p>\n\n\n\n<h2><strong>Graphical Explanation <\/strong><\/h2>\n\n\n\n<p>If we plot a graph between temperature on x-axis and the volume of one mole of an ideal gas on the y-axis, we get a straight line which cuts the temperature axis at -273.16<sup>o<\/sup> C. this can be possible only if we extrapolate the graph upto -273.16<sup>o<\/sup>C. This temperature is the lowest possible temperature which would have been achieved if the substance remains in the gaseous state. Actually, all the gases are converted into liquids above this temperature. <\/p>\n\n\n\n<p>Charles\u2018s law is obeyed when the temperature is taken on Kelvin scale. For example, at 238 K (10<sup>O<\/sup> C) the volume is 566cm<sup>3<\/sup> while at 373 K (100<sup>o<\/sup>C) the volume is 746 cm<sup>3. <\/sup>According to Charles\u2019s law <\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;V <sub>1<\/sub>\/ &nbsp;&nbsp;T<sub>1<\/sub>&nbsp;&nbsp;=&nbsp;&nbsp;&nbsp;&nbsp; V<sub>2<\/sub>\/T<sub>2 <\/sub> &nbsp;&nbsp;= k&nbsp; <\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;566\/283 &nbsp;&nbsp;=&nbsp;&nbsp;&nbsp;&nbsp; 746\/373&nbsp; &nbsp;&nbsp;=2= k<\/p>\n\n\n\n<p>Greater the mass of gas taken, greater will be the slope of straight line. The reason is that greater the number of moles greater the volume occupied. All these straight lines when extrapolated meet at a single point of -273.16<sup>o<\/sup>C (0 Kelvin). It is apparent that this temperature of -273.16<sup>o<\/sup>C will be attained when the volume becomes zero. But for real gas the zero volume is impossible which shows that this temperature cannot be attained for a real gas. This is how we recognized that -273.16<sup>o<\/sup> C must represent the coldest temperature.<\/p>\n\n\n\n<figure class=\"wp-block-image\"><img loading=\"lazy\" width=\"428\" height=\"245\" src=\"https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/10\/image-42.png\" alt=\"\" class=\"wp-image-963\" srcset=\"https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/10\/image-42.png 428w, https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/10\/image-42-300x172.png 300w\" sizes=\"(max-width: 428px) 100vw, 428px\" title=\"\"><\/figure>\n\n\n\n<p><strong>Relation to Absolute zero<\/strong><\/p>\n\n\n\n<p>According\nto Charles\u2019s law gas will descend to zero at certain temperature. Gay- Lussac\nsaid that this law is not applicable at low temperature:<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; He said that compressed vapours\nremain entirely in their elastic state and they require temperature to enable them\nto resist the pressure.<\/p>\n\n\n\n<p>At\nabsolute zero temperature gas has zero energy so molecule restrict their motion\nGay-Lussac also demonstrate that the Charles\u2019s law doesn\u2019t applicable just\nabove the boiling point of the liquid. For example, ether is only a little\nabove of its boiling point.<\/p>\n\n\n\n<p>William\nThomson was the first who mention that volume of a gas might descend to zero.\nHe describe absolute zero in terms of the second law of thermodynamics.<\/p>\n\n\n\n<p><strong>Derivation of Absolute\nZero<\/strong><\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; In order to derive absolute zero of\ntemperature, consider the following quantitative definition of Charles\u2019s law.<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; At constant pressure the volume of\nthe given mass of the gas increases or decreases by 1\\273 of its original\nvolume at 0<sup>o<\/sup>C for every 1<sup>o<\/sup>C rise or fall in temperature\nrespectively. <\/p>\n\n\n\n<p>The\ngeneral equation to know the volume of the gas at various temperature is<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; V<sub>t<\/sub>= V<sub>0<\/sub>\n(1+t\\273)<\/p>\n\n\n\n<p>V<sub>t<\/sub>\n= volume of gas at temperature T<\/p>\n\n\n\n<p>V<sub>0<\/sub>\n= volume of gas at 0<sup>o<\/sup> C<\/p>\n\n\n\n<p>t\n= temperature on centigrade or Celsius scale<\/p>\n\n\n\n<p>if\na gas is warmed by 1<sup>o<\/sup>C, it expands by 1\\273 of its original volume\nat 0<sup>0<\/sup> C. Since original volume is 546cm<sup>3<\/sup>, so for 1<sup>0<\/sup>\nC rise in temperature 2cm<sup>3 <\/sup>increase in volume will take place. 2cm<sup>3<\/sup>\nis the 1\\273 of 546cm<sup>3<\/sup>. Similarly for 100<sup>0<\/sup>C rise in\ntemperature, a change of 200cm<sup>3<\/sup>will take place.<\/p>\n\n\n\n<p>For\nexample, the increase in temperature from 10<sup>0<\/sup>C to 100<sup>0<\/sup> C,\nincrease in volume from 566cm<sup>3 <\/sup>to 746cm<sup>3<\/sup>. <\/p>\n\n\n\n<p><strong>Relation to kinetic\ntheory<\/strong><\/p>\n\n\n\n<p>The\nkinetic theory of gases is related to the macroscopic properties of gases like\npressure and volume. It is also related to the microscopic properties of\nmolecules like speed and mass of the molecules which make up the gas. In this\ntheory temperature is taken as proportional to the average kinetic energy of\nthe gas molecule. <\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; T \u03b1 <em>E<\/em><sub>k<\/sub><\/p>\n\n\n\n<h2><strong>Application <\/strong><\/h2>\n\n\n\n<ol><li><strong>Hot\nair balloons<\/strong><\/li><\/ol>\n\n\n\n<p>`An object floats in a\nfluid when it weigh less than the fluid it displaces. According to Charles\u2019s\nlaw, balloon is filled with heated gas, so volume expand. At elevated volume,\nthe balloon occupies a greater volume in the same weight. Its density is lesser\nthan the cold air so balloon begins to rise.<\/p>\n\n\n\n<ul><li><strong>Bloated\ntires<\/strong><\/li><\/ul>\n\n\n\n<p>According to Charles law,\nthe bloated tubes protruding out from a tire when we left in summer heat. The\nheat outside steadily enter into tubes and gradually causes the tire to expand.\nIt is highly recommended to check your tires daily in summers. Because if subjected\nto further expansion the tires can burst at any second.<\/p>\n\n\n\n<ul><li><strong>Automobiles\n<\/strong><\/li><\/ul>\n\n\n\n<p>In automobile engine series of pistons are lined up\nthey are periodically bob up and down when there is presence or absence of\nfluid. The one end of piston is attached with crankshaft so rise or fall rotate\nthe shaft and other end is attached with rear wheel of automobile. According to\nCharles\u2019s law pistons are pushed by gas which is produced by fuel combustion.\nThe combustion produce great amount of heat. So temperature rise and converted\ngas expands. They push them with force and thrust the vehicle forward.<\/p>\n\n\n\n<p><strong>Properties of Gases<\/strong><\/p>\n\n\n\n<ul><li>Gases\ndon\u2019t have a definite volume and occupy all the available space. The volume of\na gas is the volume of the container.<\/li><li>They\ndon\u2019t have a definite shape and take the shape of the container just like\nliquids.<\/li><li>Due\nto low densities of gases, as compared to those of liquids and solids, the\nbubble through liquids and tend to rise up.<\/li><li>Gases\ncan diffuse and effuse.<\/li><li>Gases\ncan be compressed by applying a pressure because there are large empty spaces\nbetween their molecules.<\/li><li>Gases\ncan expands on heating.<\/li><li>When\nsudden expansion of gases occurs cooling takes place, it is called Joule\nThomson effect.<\/li><li>Molecules\nof gases are in a constant state of random motion. They can exert a certain\npressure on the walls of the container and this pressure is due to the number\nof collisions.<\/li><li>The\nintermolecular forces in gases are very weak [3].<\/li><li>Gases\ntemperature is proportional to the average kinetic energy of the molecules.<\/li><\/ul>\n\n\n\n<p><strong>The Ideal Gas Equation <\/strong><\/p>\n\n\n\n<p>According\nto Boyle\u2019s law:<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; V\u03b1 1\/P<\/p>\n\n\n\n<p>According\nto Charles\u2019s law: <\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; V\u03b1 T<\/p>\n\n\n\n<p>It\nis well known fact that volume of the given gas at constant temperature and\npressure is directly proportional to the number of moles (Avogadro\u2019s law)<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;V\u03b1 n<\/p>\n\n\n\n<p>So\nby these equations <\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; V\u03b1&nbsp;&nbsp;&nbsp; nT\/P<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; V= constant nT\/P<\/p>\n\n\n\n<p>The\nconstant is R which is called general gas constant.<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; V= R&nbsp;&nbsp; nT\/P<\/p>\n\n\n\n<p><strong>Reference <\/strong><\/p>\n\n\n\n<ol><li><a href=\"https:\/\/www.scienceabc.com\/nature\/universe\/charles-law-definition-formula-equation.html\" target=\"_blank\" rel=\"noopener\">https:\/\/www.scienceabc.com\/nature\/universe\/charles-law-definition-formula-equation.html<\/a><\/li><li><a href=\"https:\/\/en.wikipedia.org\/wiki\/Charles%27s_law\" target=\"_blank\" rel=\"noopener\">https:\/\/en.wikipedia.org\/wiki\/Charles%27s_law<\/a><\/li><li>https:\/\/www.chemguide.co.uk\/physical\/kt\/idealgases.html<\/li><\/ol>\n","protected":false},"excerpt":{"rendered":"<p>Definition It is a quantitative relationship between temperature and volume of a gas. It was given by French scientist J. Charles in 1787. According to this law, the volume of the given mass of a gas is directly proportional to the absolute temperature when the pressure is kept constant. &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; V&nbsp;&nbsp;&nbsp; \u03b1&nbsp;&nbsp; T&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; (when pressure &#8230; <a title=\"Charles&#8217;s Law\" class=\"read-more\" href=\"https:\/\/chemdictionary.org\/charless-law\/\" aria-label=\"More on Charles&#8217;s Law\">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":[20,2],"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":959}]},"_links":{"self":[{"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/posts\/959"}],"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=959"}],"version-history":[{"count":5,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/posts\/959\/revisions"}],"predecessor-version":[{"id":986,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/posts\/959\/revisions\/986"}],"wp:attachment":[{"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/media?parent=959"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/categories?post=959"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/tags?post=959"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}