{"id":20541,"date":"2025-06-14T14:11:06","date_gmt":"2025-06-14T14:11:06","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=20541"},"modified":"2025-06-14T14:11:12","modified_gmt":"2025-06-14T14:11:12","slug":"exactly-1-0-mole-of-oxygen-gas-and-7-0-moles-of-nitrogen-gas-are-in-a-container","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/exactly-1-0-mole-of-oxygen-gas-and-7-0-moles-of-nitrogen-gas-are-in-a-container\/","title":{"rendered":"Exactly 1.0 mole of oxygen gas and 7.0 moles of nitrogen gas are in a container"},"content":{"rendered":"\n<p>Exactly 1.0 mole of oxygen gas and 7.0 moles of nitrogen gas are in a container. The total gas pressure is 5.7 atm. What is the partial pressure of nitrogen in atm?<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-vivid-cyan-blue-color\"><strong>The correct answer and explanation is:<\/strong><\/mark><\/p>\n\n\n\n<p><strong>Correct Answer:<\/strong><br>The partial pressure of nitrogen gas (N\u2082) is <strong>5.0 atm<\/strong>.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Explanation (300 words):<\/strong><\/h3>\n\n\n\n<p>To calculate the <strong>partial pressure<\/strong> of a gas in a mixture, we use <strong>Dalton\u2019s Law of Partial Pressures<\/strong>, which states:<\/p>\n\n\n\n<blockquote class=\"wp-block-quote is-layout-flow wp-block-quote-is-layout-flow\">\n<p><strong>Total pressure<\/strong> of a gas mixture is equal to the <strong>sum of the partial pressures<\/strong> of each individual gas.<\/p>\n<\/blockquote>\n\n\n\n<p>Mathematically: Ptotal=PO2+PN2P_{\\text{total}} = P_{O_2} + P_{N_2}<\/p>\n\n\n\n<p>Each gas&#8217;s partial pressure is proportional to the number of moles it contributes, and is given by: Pgas=(ngasntotal)\u00d7PtotalP_{\\text{gas}} = \\left( \\frac{n_{\\text{gas}}}{n_{\\text{total}}} \\right) \\times P_{\\text{total}}<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Step-by-step solution:<\/strong><\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Given:<\/strong>\n<ul class=\"wp-block-list\">\n<li>Moles of oxygen gas (O2O_2) = 1.0 mol<\/li>\n\n\n\n<li>Moles of nitrogen gas (N2N_2) = 7.0 mol<\/li>\n\n\n\n<li>Total pressure = 5.7 atm<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Calculate total moles of gas:<\/strong><\/li>\n<\/ol>\n\n\n\n<p>ntotal=nO2+nN2=1.0+7.0=8.0&nbsp;moln_{\\text{total}} = n_{O_2} + n_{N_2} = 1.0 + 7.0 = 8.0 \\text{ mol}<\/p>\n\n\n\n<ol start=\"3\" class=\"wp-block-list\">\n<li><strong>Find the mole fraction of nitrogen:<\/strong><\/li>\n<\/ol>\n\n\n\n<p>\u03c7N2=nN2ntotal=7.08.0=0.875\\chi_{N_2} = \\frac{n_{N_2}}{n_{\\text{total}}} = \\frac{7.0}{8.0} = 0.875<\/p>\n\n\n\n<ol start=\"4\" class=\"wp-block-list\">\n<li><strong>Calculate the partial pressure of nitrogen:<\/strong><\/li>\n<\/ol>\n\n\n\n<p>PN2=\u03c7N2\u00d7Ptotal=0.875\u00d75.7=4.9875\u22485.0&nbsp;atmP_{N_2} = \\chi_{N_2} \\times P_{\\text{total}} = 0.875 \\times 5.7 = 4.9875 \\approx \\boxed{5.0 \\text{ atm}}<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Conclusion:<\/strong><\/h3>\n\n\n\n<p>The partial pressure of a gas in a mixture depends on its <strong>relative mole fraction<\/strong>. Since nitrogen contributes 7 out of the 8 total moles, it dominates the mixture and exerts a larger share of the pressure. Using the mole fraction and total pressure, we determine nitrogen\u2019s partial pressure is approximately <strong>5.0 atm<\/strong>.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Exactly 1.0 mole of oxygen gas and 7.0 moles of nitrogen gas are in a container. The total gas pressure is 5.7 atm. What is the partial pressure of nitrogen in atm? The correct answer and explanation is: Correct Answer:The partial pressure of nitrogen gas (N\u2082) is 5.0 atm. Explanation (300 words): To calculate the [&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-20541","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/20541","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=20541"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/20541\/revisions"}],"predecessor-version":[{"id":20542,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/20541\/revisions\/20542"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=20541"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=20541"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=20541"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}