{"id":518,"date":"2017-08-21T10:00:42","date_gmt":"2017-08-21T10:00:42","guid":{"rendered":"http:\/\/americanboard.org\/Subjects\/chemistry\/?page_id=518"},"modified":"2020-12-29T06:32:27","modified_gmt":"2020-12-29T06:32:27","slug":"gas-laws","status":"publish","type":"page","link":"https:\/\/americanboard.org\/Subjects\/chemistry\/gas-laws\/","title":{"rendered":"Gas Laws"},"content":{"rendered":"<div class=\"twelve columns\" style=\"margin-top: 10%;\">\n<div class=\"advance\">\n<p><a class=\"button\" href=\"http:\/\/americanboard.org\/Subjects\/chemistry\/gas-laws-and-solutions\">Workshop Index<\/a>\u00a0<a class=\"button button-primary\" href=\"http:\/\/americanboard.org\/Subjects\/chemistry\/solution-formation-and-concentrations\">Next Lesson \u27a1<\/a><\/p>\n<\/div>\n<p><!-- UPDATE NEXT\/PREVIOUS ABOVE --><\/p>\n<p><!-- CONTENT STARTS HERE --><\/p>\n<h1 id=\"title\">Gas Laws and Solutions: Gas Laws<\/h1>\n<h4>Objective<\/h4>\n<p>In this lesson we will study the kinetic molecular theory and the basic properties of gas laws and their\u00a0calculations.<\/p>\n<section>\n<h3>Kinetic Molecular Theory (KMT)<\/h3>\n<p>The <abbr title=\"Explains the forces between molecules and the energy that they possess.\">kinetic molecular theory<\/abbr> is based on the assumption of an ideal, or \u201cperfect,\u201d gas. Although the perfect gas does not exist in the real world, the kinetic molecular theory is describing this imaginary gas and the KMT is extremely useful for predicting gas behavior. Remember, the KMT is a theory. It has been proven many times, but it is not absolute. It is an attempt to treat all real gases as if they were the same and their differing behaviors are approximated by the ideal gas.<\/p>\n<ul>\n<li><strong>A gas consists of objects with a defined mass and zero volume.<br \/>\n<\/strong>This is based on the idea that all real gas particles are of extremely small volume. To\u00a0apply this to real gases, it is assumed that they are all the same volume and that volume is\u00a0zero. The masses of real gases are usually small and this allows for them to have a defined mass\u00a0of zero also.<\/li>\n<li><strong>The gas particles travel randomly in straight-line motion where their movement can be\u00a0described by the fundamental laws of mechanics.<\/strong><br \/>\nGas particles are always in motion except at <abbr title=\"The temperature of \u2212273.16\u00b0C (\u2212459.69\u00b0F), or 0 K, the hypothetical point at which all molecular activity ceases \">absolute\u00a0zero <\/abbr>(0 K). The particles will travel in random straight line paths. The only deviation from this\u00a0straight line path is collisions with other particles. If a gas is in a closed system, then it\u00a0will expand outward to fit the larger volume of its container.<\/li>\n<li><strong>All collisions involving gas particles are elastic. No energy is lost and no heat is\u00a0produced.<\/strong><br \/>\nAn elastic collision is one in which there is no loss of <abbr title=\"The energy of a moving object. K = \u00bdmv2, where m is the mass of the moving object, and v is its speed.\">kinetic energy<\/abbr>. While\u00a0the gas phase system undergoes elastic collisions, it is possible for the distribution of the\u00a0kinetic energy in the system to change. That is, kinetic energy can be transferred; some objects\u00a0can gain kinetic energy, but only if others lose kinetic energy. The important point is that the\u00a0<em>total<\/em> kinetic energy of the system remains constant.<\/li>\n<li><strong> The gas particles do not interact with each other or with the walls of their container.<\/strong><br \/>\nEven though the gas particles collide with each other, they do not react with each other.\u00a0This also applies to the container\u2019s walls. No bonds or attractions can form, if they did, this\u00a0would lead to restricted motion of the gas particles.<\/li>\n<li><strong> Temperature is directly proportional to the kinetic energy of the gas phase\u00a0system.<\/strong><br \/>\nIf the temperature of a gas remains constant then the average kinetic energy of the system will\u00a0also remain constant.<\/li>\n<\/ul>\n<h3>Ideal Gases<\/h3>\n<p>The <abbr title=\"A perfect gas: a hypothetical gas consisting of identical particles of zero volume, with no intermolecular forces\">ideal\u00a0gas<\/abbr> model states:<\/p>\n<ul>\n<li>Ideal gas particles are so small that the volume of the individual particles if they were at\u00a0rest would be essentially zero when compared with the total volume of the gas.<\/li>\n<li>Ideal gas particles are in constant, rapid, random motion, moving in straight lines in all\u00a0directions until they collide with other particles or the sides of their container.<\/li>\n<li>There are no attractive or repulsive forces between particles, and collisions between them are\u00a0elastic.<\/li>\n<li>The average kinetic energy of the particles is directly proportional to the absolute temperature\u00a0(measured in Kelvin).<\/li>\n<\/ul>\n<h3>Real Gases<\/h3>\n<p><abbr title=\"A gas that deviates from the ideal gas model.\">Real gases<\/abbr> are defined as gases that do not\u00a0fit the kinetic molecular theory. Even one deviation places the gas in the real gas category. The\u00a0KMT will always cause problems for scientists, after all, it is a theory and still being tested.\u00a0However, two main characteristics cause deviations from ideal behavior:<\/p>\n<ul>\n<li>Very large volume gas molecules will deviate significantly from ideal behavior. Since an ideal\u00a0gas is able to move anywhere in the container, large volume particles will be restricted from\u00a0parts of the container that are occupied by the other gas particles. Ideal gas behavior is based\u00a0on the volume of a gas being very small. Theoretically, helium is the smallest volume gas\u00a0commonly found in our environment.<\/li>\n<li>Gas particles that exhibit polar qualities are going to differ from ideal gas behavior. Any gas\u00a0that is highly polar, such as water vapor, will experience significant attractions for the other\u00a0particles in the system. This creates problems with the concept of ideal gases not interacting\u00a0with each other.<\/li>\n<\/ul>\n<p>When the system is at high pressure or low temperature it again deviates from ideal behavior. These\u00a0circumstances cause the particles to be close together and improve the chance of interactions.<\/p>\n<p>The four variables used to describe gases are temperature, pressure, moles, and volume. Temperature is the measure\u00a0of the average kinetic energy of random motion of the particles in a sample of matter. Because many properties of\u00a0gases depend on the temperature of the studied system, calculations with gases include a specific temperature.\u00a0Kelvin is used for all gas law calculations. If you are given a value in \u00baC, it must be converted to Kelvin.<\/p>\n<p class=\"center\">K = \u00b0C + 273<br \/>\n<em>T = t<\/em> + 273<\/p>\n<p class=\"center\">K = Kelvin<br \/>\n<em>T<\/em> = absolute temperature<br \/>\n<em>t<\/em> = Celsius temperature<\/p>\n<p><abbr title=\"The force exerted per unit area.\">Pressure<\/abbr>is the force exerted per unit\u00a0area. In\u00a0relation to gases, pressure is a measure of the total force exerted by the moving particles of a gas as they collide\u00a0with the walls of the container.<\/p>\n<p><center><img loading=\"lazy\" decoding=\"async\" src=\"http:\/\/americanboard.org\/Subjects\/Images\/chemistry\/img\/gaslaw\/s1_001.gif\" width=\"180\" height=\"41\" \/><\/center><abbr title=\"The temperature of 0\u00b0C and pressure of 1 atmosphere, usually taken as the conditions when stating properties of gases\">STP<\/abbr> is standard temperature and pressure. They\u00a0are the accepted values for all gas law calculations. Unless given specific information of the gas variables, use\u00a0STP. The table below includes STP values.<\/p>\n<table>\n<thead>\n<tr>\n<th>Pressure<\/th>\n<th>Temperature<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>1.0000 atm<\/td>\n<td>273.16 K<\/td>\n<\/tr>\n<tr>\n<td>101.325 kPa<\/td>\n<td>273.16 K<\/td>\n<\/tr>\n<tr>\n<td>760.0 mm Hg<\/td>\n<td>273.16 K<\/td>\n<\/tr>\n<tr>\n<td>760.0 torr<\/td>\n<td>273.16 K<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p>&nbsp;<\/p>\n<p><abbr title=\"The fundamental SI unit used to measure the amount of a substance.\">Moles<\/abbr> is\u00a0the\u00a0fundamental SI unit used to measure the amount of a substance. Moles tell you the quantity of the gas. This\u00a0expresses the number of objects in the system and does not directly indicate their masses.<\/p>\n<p><abbr title=\"The amount of space an object occupies.\">Volume<\/abbr> is the amount of space an\u00a0object\u00a0occupies. Gas particles are widely spaced and the volume of a gas is primarily empty space between particles. As a\u00a0gas contracts, its particles move closer together. As it expands, they move farther apart.<\/p>\n<p><abbr title=\"A gas will effuse at a rate that is inversely proportional to the square root of its molecular mass\">Graham\u2019s\u00a0Law of Effusion<\/abbr> states that a gas will effuse\u00a0at a rate that is inversely proportional to the square root of its molecular mass, <em>\u00b5<\/em>.<\/p>\n<p><center><img loading=\"lazy\" decoding=\"async\" src=\"http:\/\/americanboard.org\/Subjects\/Images\/chemistry\/img\/gaslaw\/s1_002.gif\" width=\"69\" height=\"50\" \/><\/center><\/p>\n<p class=\"center\"><em> r<\/em><sub>1<\/sub> = velocity of gas 1<br \/>\n<em>\u00b5<\/em><sub>1<\/sub> = molecular mass of gas 1<br \/>\n<em>r<\/em><sub>2<\/sub> = velocity of gas 2<br \/>\n<em>\u00b5<\/em><sub>2<\/sub> = molecular mass of gas 2<\/p>\n<h4>Sample Problem<\/h4>\n<p>An O<sub>2<\/sub> molecule travels at 480 m\/s at room temperature. How fast would a molecule of\u00a0SO<sub>3<\/sub> travel at the same temperature?<\/p>\n<p>First, list the given values:<br \/>\n<em>r<\/em><sub>1<\/sub> = 48 0 m\/s<br \/>\n<em>\u00b5<\/em><sub>1<\/sub> = 32 g\/mol (16 g\/mol \u00d7 2)<br \/>\n<em>\u00b5<\/em><sub>2<\/sub> = 80 g\/mol (32 g\/mol + 16 g\/mol \u00d7 3)<\/p>\n<p>Then, write the equation:<\/p>\n<p><center><img loading=\"lazy\" decoding=\"async\" class=\"aligncenter\" src=\"http:\/\/americanboard.org\/Subjects\/Images\/chemistry\/img\/gaslaw\/s1_002.gif\" width=\"69\" height=\"50\" \/><\/center>Finally, plug in the known values and solve:<\/p>\n<p class=\"center\"><img loading=\"lazy\" decoding=\"async\" class=\"no_margin aligncenter\" src=\"http:\/\/americanboard.org\/Subjects\/Images\/chemistry\/img\/gaslaw\/s1_005.gif\" width=\"158\" height=\"49\" \/>;<em>r<\/em><sub>2<\/sub> = 304 m\/s<\/p>\n<p><abbr title=\"The sum of the individual pressures of all the gases that make up a mixture is equal to the total pressure.\">Dalton\u2019s\u00a0Law<\/abbr> states that the sum of the\u00a0individual pressures of all the gases that make up a mixture is equal to the total pressure.<\/p>\n<p class=\"center\" style=\"text-align: center;\"><em>P<\/em><sub>T<\/sub> = <em>P<\/em><sub>1<\/sub> + <em>P<\/em><sub>2<\/sub> + <em>P<\/em><sub>3<\/sub> + \u2026, or <img loading=\"lazy\" decoding=\"async\" class=\"no_margin\" src=\"http:\/\/americanboard.org\/Subjects\/Images\/chemistry\/img\/gaslaw\/s1_009.gif\" width=\"150\" height=\"41\" \/><\/p>\n<h4>Sample Problem<\/h4>\n<p>A 32.0 mL sample of H<sub>2<\/sub> gas collected over water has a pressure of 750.0 torr. What is the partial pressure of H<sub>2<\/sub> gas if the total pressure is 875.5 torr?<\/p>\n<p><em>P<\/em><sub>1<\/sub> = 750.0 torr<br \/>\n<em>P<sub>2<\/sub><\/em> = <em>P<\/em> 2<br \/>\n<em>P<\/em><sub>T<\/sub> = 875.5 torr<\/p>\n<p class=\"center\"><em>P<\/em><sub>T<\/sub> = <em>P<\/em><sub>1<\/sub> + <em>P<\/em><em><sub>2<\/sub><\/em> +<br \/>\n<em>P<\/em><sub>3<\/sub> + \u2026..<br \/>\n875.5 torr = 750.0 torr + <em>P<\/em><em><sub>2<br \/>\n<\/sub><\/em><em>P<\/em><em><sub>2<\/sub><\/em> = 125.5 torr<\/p>\n<section class=\"question\">\n<h4>Question<\/h4>\n<p>A 15.0 mL sample of N<sub>2<\/sub> gas collected over water has a pressure of 1.00 atm. What is the partial\u00a0pressure\u00a0of the N<sub>2<\/sub> gas if the total pressure is 4.6 atm?<\/p>\n<p><a class=\"button button-primary q-answer\"> Reveal Answer <\/a><\/p>\n<p class=\"q-reveal center\"><em>P<sub>1<\/sub> <\/em>= 1.00 atm<br \/>\n<em>P<\/em><sub>2<\/sub> = <em>P<\/em><sub>2<\/sub><br \/>\n<em>P<\/em><sub>T<\/sub> = 4.6 atm<br \/>\n<em>P<\/em><sub>T<\/sub> = <em>P<\/em><sub>1<\/sub> + <em>P<\/em><em><sub>2<\/sub><\/em> +<br \/>\n<em>P<\/em><sub>3<\/sub> + \u2026..<br \/>\n4.6 atm = 1.00 atm + <em>P<\/em><em><sub>2<br \/>\n<\/sub><\/em><em>P<\/em><em><sub>2<\/sub><\/em> = 3.6 atm<\/p>\n<p class=\"q-reveal\">The correct answer is 3.6 atm.<\/p>\n<\/section>\n<p><abbr title=\"The volume of a gas varies directly with the Kelvin temperature, assuming that the pressure is constant.\">Charles\u2019s Law<\/abbr> states that the volume of\u00a0a gas varies directly with the Kelvin temperature, assuming that the pressure is constant. As one goes up, the other\u00a0goes up.<\/p>\n<p><center><img loading=\"lazy\" decoding=\"async\" src=\"http:\/\/americanboard.org\/Subjects\/Images\/chemistry\/img\/gaslaw\/s1_010.gif\" width=\"57\" height=\"46\" \/><\/center><\/p>\n<h4>Sample Problem<\/h4>\n<p>A sample of nitrogen occupies a volume of 250.0 mL at 298 K. What volume will it occupy at 368 K?<\/p>\n<p><em>V<\/em><sub>1<\/sub> = 250 mL<br \/>\n<em>T<\/em><sub>1<\/sub> = 298 K<br \/>\n<em>T<\/em><sub>2<\/sub>= 368 K<\/p>\n<p class=\"center\"><img loading=\"lazy\" decoding=\"async\" src=\"http:\/\/americanboard.org\/Subjects\/Images\/chemistry\/img\/gaslaw\/s1_010.gif\" width=\"57\" height=\"46\" \/><br \/>\n<img loading=\"lazy\" decoding=\"async\" src=\"http:\/\/americanboard.org\/Subjects\/Images\/chemistry\/img\/gaslaw\/s1_012.gif\" width=\"124\" height=\"42\" \/><br \/>\n<em>V<\/em><sub>2<\/sub> = 309 mL<\/p>\n<p><abbr title=\"The volume of a gas varies inversely with its pressure if temperature is held constant.\">Boyle\u2019s Law<\/abbr> states that the volume of a\u00a0gas varies inversely with its pressure if temperature is held constant. As one goes up, the other goes down.<\/p>\n<p class=\"center\"><em> P<\/em><sub>1<\/sub> \u00d7 <em>V<\/em><sub>1<\/sub> = <em>P<\/em><sub>2<\/sub> \u00d7 <em>V<\/em><sub>2<\/sub><\/p>\n<h4>Sample Problem<\/h4>\n<p>A sample of CO<sub>2<\/sub> gas occupies a volume of 3.50 L at 125 kPa. What pressure would the gas exert if the\u00a0volume were decreased to 2.0 L?<\/p>\n<p><em> P<\/em><sub>1<\/sub> = 125 kPa<br \/>\n<em>V<\/em><sub>1<\/sub> = 3.50 L<br \/>\n<em>V<\/em><sub>2<\/sub> = 2.0 L<\/p>\n<p class=\"center\"><em>P<\/em><sub>1<\/sub> \u00d7 <em>V<\/em><sub>1<\/sub> = <em>P<\/em><sub>2<\/sub> \u00d7 <em>V<\/em><sub>2<br \/>\n<\/sub>125 kPa \u00d7 3.50 L = <em>P<\/em><sub>2<\/sub> \u00d7 2.0 L<br \/>\n<em>P<\/em><sub>2<\/sub> = 220 kPa<\/p>\n<section class=\"question\">\n<h4>Question<\/h4>\n<p>Ammonia gas occupies a volume of 250.0 mL at a pressure of 720.0 mm Hg. What volume will it occupy at STP?<\/p>\n<p><a class=\"button button-primary q-answer\"> Reveal Answer <\/a><\/p>\n<p class=\"q-reveal\"><em> P<\/em><sub>1<\/sub> = 720.0 mm Hg<br \/>\n<em>V<\/em><sub>1<\/sub> = 250.0 mL<br \/>\n<em>P<\/em><sub>2<\/sub> = 760.0 mm Hg<br \/>\n<em>P<\/em><sub>1<\/sub> \u00d7 <em>V<\/em><sub>1<\/sub> = <em>P<\/em><sub>2<\/sub> \u00d7 <em>V<\/em><sub>2<\/sub><br \/>\n720.0 mm Hg \u00d7 250.0 mL = 760.0 mm Hg \u00d7 <em>V<\/em><sub>2<\/sub><br \/>\nThe correct answer is 236.8 mL.<\/p>\n<\/section>\n<p><abbr title=\"Uses the four gas variables in relationship to each other. Temperature is always calculated in Kelvin.\">Ideal Gas Law<\/abbr> uses the four gas variables in relationship to each other. Remember temperature is always calculated in Kelvin.<\/p>\n<p class=\"center\"><em>PV = nRT<br \/>\nR<\/em> = 0.0821 L<strong>\u2219<\/strong>atm\/mol<strong>\u2219<\/strong>K<br \/>\n<em>R<\/em> = 8.314 L<strong>\u2219<\/strong>kPa\/mol<strong>\u2219<\/strong>K<\/p>\n<h4>Sample Problem<\/h4>\n<p>How many moles of oxygen will occupy a volume of 2.5 L at 1.2 atm and 298 K?<\/p>\n<p><em>P<\/em> = 1.2 atm<br \/>\n<em>V <\/em>= 2.5 L<\/p>\n<p class=\"center\"><em>PV = nRT<br \/>\n<\/em>1.2 atm \u00d7 2.5 L = <em>n<\/em> \u00d7 (0.0821 L<strong>\u2219<\/strong>atm\/mol<strong>\u2219<\/strong>K) \u00d7 298 K<br \/>\n<em>n<\/em> = 0.12 mol<\/p>\n<p>Be sure to use the same pressure units for the problem and the <em>R<\/em> constant.<\/p>\n<section class=\"question\">\n<h4>Question<\/h4>\n<p>Calculate the volume of 1 mol of CCl<sub>4<\/sub> at STP.<\/p>\n<p><a class=\"button button-primary q-answer\"> Reveal Answer <\/a><\/p>\n<p class=\"q-reveal\"><em>P<\/em> = 1.0 atm<br \/>\n<em>n<\/em> = 1 mol<br \/>\n<em>T<\/em> = 273.16 K<br \/>\n<em>PV = nRT<br \/>\n<\/em>1.0 atm \u00d7 <em> V<\/em> = 1 \u00d7 (0.0821 L<strong>\u2219<\/strong>atm\/mol<strong>\u2219<\/strong>K) \u00d7 273.16 K<br \/>\n<em>V<\/em> = 22.4 L.<\/p>\n<\/section>\n<h3>Review of Gas Laws<\/h3>\n<p><object class=\"old_animation\" width=\"650\" height=\"390\" classid=\"clsid:d27cdb6e-ae6d-11cf-96b8-444553540000\" codebase=\"http:\/\/fpdownload.macromedia.com\/pub\/shockwave\/ca= bs\/flash\/swflash.cab#version=6,0,0,0\" align=\"middle\"><param value=\"sameDomain\" name=\"allowScriptAccess\" \/><param value=\"flashPlayer.swf?sURL=images\/GSC03_gaslaw_jm.swf\" name=\"movie\" \/><param value=\"high\" name=\"quality\" \/><param value=\"#ffffff\" name=\"bgcolor\" \/><embed src=\"http:\/\/americanboard.org\/Subjects\/Images\/biology\/flash\/gaslaw\/flashplayer.swf?sURL=http:\/\/americanboard.org\/Subjects\/Images\/biology\/flash\/gaslaw\/GSC03_gaslaw.swf\" quality=\"high\" bgcolor=\"#ffffff\" width=\"750\" height=\"450\" name=\"flashPlayer\" align=\"middle\" allowscriptaccess=\"sameDomain\" type=\"application\/x-shockwave-flash\" pluginspage=\"http:\/\/www.macromedia.com\/go\/getflashplayer\"><\/object><\/p>\n<div class=\"slider-container new_animation\">\n<iframe loading=\"lazy\" src=\"https:\/\/americanboard.org\/Subjects\/animation_sliders\/gas_law\/gas_law.html\" width=\"750\" height=\"450\" frameborder=\"0\" scrolling=\"no\"><\/iframe>\n<\/div>\n<\/section>\n<p><!-- CONTENT ENDS HERE --><\/p>\n<p><!-- UPDATE NEXT\/PREVIOUS BELOW --><\/p>\n<div class=\"advance\"><a class=\"button\" href=\"http:\/\/americanboard.org\/Subjects\/chemistry\/gas-laws-and-solutions\">Workshop Index<\/a>\u00a0<a class=\"button button-primary\" href=\"http:\/\/americanboard.org\/Subjects\/chemistry\/solution-formation-and-concentrations\">Next Lesson \u27a1<\/a><\/div>\n<p><a class=\"backtotop\" href=\"#title\">Back to Top<\/a><\/p>\n<\/div>\n","protected":false},"excerpt":{"rendered":"<p>Workshop Index\u00a0Next Lesson \u27a1 Gas Laws and Solutions: Gas Laws Objective In this lesson we will study the kinetic molecular theory and the basic properties of gas laws and their\u00a0calculations. Kinetic Molecular Theory (KMT) The kinetic molecular theory is based on the assumption of an ideal, or \u201cperfect,\u201d gas. Although the perfect gas does not [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":0,"parent":0,"menu_order":0,"comment_status":"closed","ping_status":"closed","template":"","meta":{"footnotes":""},"class_list":["post-518","page","type-page","status-publish","hentry"],"_links":{"self":[{"href":"https:\/\/americanboard.org\/Subjects\/chemistry\/wp-json\/wp\/v2\/pages\/518","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/americanboard.org\/Subjects\/chemistry\/wp-json\/wp\/v2\/pages"}],"about":[{"href":"https:\/\/americanboard.org\/Subjects\/chemistry\/wp-json\/wp\/v2\/types\/page"}],"author":[{"embeddable":true,"href":"https:\/\/americanboard.org\/Subjects\/chemistry\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/americanboard.org\/Subjects\/chemistry\/wp-json\/wp\/v2\/comments?post=518"}],"version-history":[{"count":23,"href":"https:\/\/americanboard.org\/Subjects\/chemistry\/wp-json\/wp\/v2\/pages\/518\/revisions"}],"predecessor-version":[{"id":543,"href":"https:\/\/americanboard.org\/Subjects\/chemistry\/wp-json\/wp\/v2\/pages\/518\/revisions\/543"}],"wp:attachment":[{"href":"https:\/\/americanboard.org\/Subjects\/chemistry\/wp-json\/wp\/v2\/media?parent=518"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}