{"id":36227,"date":"2025-06-25T05:31:56","date_gmt":"2025-06-25T05:31:56","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=36227"},"modified":"2025-06-25T05:31:59","modified_gmt":"2025-06-25T05:31:59","slug":"how-many-moles-of-hydrogen-h2gas-are-contained-in-a-volume-of-2lat-280kand-1-5atm","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/how-many-moles-of-hydrogen-h2gas-are-contained-in-a-volume-of-2lat-280kand-1-5atm\/","title":{"rendered":"How many moles of hydrogen H2,gas are contained in a volume of 2Lat 280Kand 1.5atm"},"content":{"rendered":"\n<p>How many moles of hydrogen H2,<br>gas are contained in a volume of 2L<br>at 280K<br>and 1.5atm<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-vivid-cyan-blue-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>To calculate how many <strong>moles of hydrogen gas (H\u2082)<\/strong> are contained in a gas sample, we can use the <strong>Ideal Gas Law<\/strong>:PV=nRTPV = nRTPV=nRT<\/p>\n\n\n\n<p>Where:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>PPP = pressure (in atmospheres, atm)<\/li>\n\n\n\n<li>VVV = volume (in liters, L)<\/li>\n\n\n\n<li>nnn = number of moles (what we are solving for)<\/li>\n\n\n\n<li>RRR = ideal gas constant = 0.0821 L\u00b7atm\/mol\u00b7K<\/li>\n\n\n\n<li>TTT = temperature (in Kelvin, K)<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Step 1: Interpret the question<\/h3>\n\n\n\n<p>We are told:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Volume V=2V = 2V=2 liters<\/li>\n\n\n\n<li>Temperature T=280T = 280T=280 Kelvin<\/li>\n\n\n\n<li>Pressure P=1.5P = 1.5P=1.5 atm<\/li>\n<\/ul>\n\n\n\n<p>We need to solve for the number of moles nnn.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Step 2: Rearranging the ideal gas law<\/h3>\n\n\n\n<p>n=PVRTn = \\frac{PV}{RT}n=RTPV\u200b<\/p>\n\n\n\n<p>Substitute the known values:n=(1.5&nbsp;atm)\u22c5(2&nbsp;L)0.0821&nbsp;L\\cdotpatm\/mol\\cdotpK\u22c5280&nbsp;Kn = \\frac{(1.5\\ \\text{atm}) \\cdot (2\\ \\text{L})}{0.0821\\ \\text{L\u00b7atm\/mol\u00b7K} \\cdot 280\\ \\text{K}}n=0.0821&nbsp;L\\cdotpatm\/mol\\cdotpK\u22c5280&nbsp;K(1.5&nbsp;atm)\u22c5(2&nbsp;L)\u200bn=3.022.988n = \\frac{3.0}{22.988}n=22.9883.0\u200bn\u22480.1305&nbsp;moln \\approx 0.1305\\ \\text{mol}n\u22480.1305&nbsp;mol<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Final Answer:<\/h3>\n\n\n\n<p><strong>Approximately 0.131 moles of hydrogen gas<\/strong> are contained in the sample.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation <\/h3>\n\n\n\n<p>The number of gas particles in a sample is usually measured in <strong>moles<\/strong>, which helps chemists relate macroscopic quantities to microscopic particles. To find the number of moles of a gas under certain conditions, the ideal gas law is a reliable formula as long as the gas behaves ideally, which hydrogen generally does under standard conditions.<\/p>\n\n\n\n<p>In this case, we were given the <strong>volume<\/strong>, <strong>temperature<\/strong>, and <strong>pressure<\/strong>, and we wanted to find how many moles of hydrogen gas were present. The ideal gas law, expressed as PV=nRTPV = nRTPV=nRT, is rearranged to solve for moles: n=PV\/RTn = PV \/ RTn=PV\/RT. Each variable must be in the proper unit. Pressure should be in atmospheres, volume in liters, and temperature in Kelvin. The gas constant RRR is always 0.0821 L\u00b7atm\/mol\u00b7K when using these units.<\/p>\n\n\n\n<p>Plugging in the numbers, we got a pressure of 1.5 atm, a volume of 2 liters, and a temperature of 280 K. The formula gave us the result of about 0.131 moles of hydrogen gas. This value tells us how many &#8220;chemical packages&#8221; of hydrogen molecules are in the container under the specified conditions.<\/p>\n\n\n\n<p>Understanding this principle is essential in chemistry, especially in reactions involving gases. By using the ideal gas law, we can predict and quantify how gases behave and how much of them is involved in reactions or processes like combustion, respiration, or industrial synthesis.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"852\" height=\"1024\" src=\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-781.jpeg\" alt=\"\" class=\"wp-image-36228\" srcset=\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-781.jpeg 852w, https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-781-250x300.jpeg 250w, https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-781-768x923.jpeg 768w\" sizes=\"auto, (max-width: 852px) 100vw, 852px\" \/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>How many moles of hydrogen H2,gas are contained in a volume of 2Lat 280Kand 1.5atm The Correct Answer and Explanation is: To calculate how many moles of hydrogen gas (H\u2082) are contained in a gas sample, we can use the Ideal Gas Law:PV=nRTPV = nRTPV=nRT Where: Step 1: Interpret the question We are told: We [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1],"tags":[],"class_list":["post-36227","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/36227","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/comments?post=36227"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/36227\/revisions"}],"predecessor-version":[{"id":36229,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/36227\/revisions\/36229"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=36227"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=36227"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=36227"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}