{"id":196841,"date":"2025-03-06T06:00:41","date_gmt":"2025-03-06T06:00:41","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=196841"},"modified":"2025-03-06T06:00:43","modified_gmt":"2025-03-06T06:00:43","slug":"a-gas-mixture-contains-6-moles-of-h2-and-2-moles-of-n2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/06\/a-gas-mixture-contains-6-moles-of-h2-and-2-moles-of-n2\/","title":{"rendered":"A gas mixture contains 6 moles of H2 and 2 moles of N2"},"content":{"rendered":"\n

A gas mixture contains 6 moles of H2 and 2 moles of N2. If the total pressure of the gaseous mixture is 4 kgf\/cm2; then the partial pressure of N2 in the mixture will be _<\/em><\/strong> kgf\/cm2.<\/p>\n\n\n\n

The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n

To find the partial pressure of nitrogen ((\\text{N}_2)) in the gas mixture, we use Dalton\u2019s Law of Partial Pressures<\/strong>, which states:<\/p>\n\n\n\n

[
P_{\\text{partial}} = \\left( \\frac{\\text{moles of gas}}{\\text{total moles of gas}} \\right) \\times P_{\\text{total}}
]<\/p>\n\n\n\n

Given Data:<\/h3>\n\n\n\n
    \n
  • Moles of Hydrogen (H\u2082)<\/strong> = 6<\/li>\n\n\n\n
  • Moles of Nitrogen (N\u2082)<\/strong> = 2<\/li>\n\n\n\n
  • Total pressure ((P_{\\text{total}}))<\/strong> = 4 kgf\/cm\u00b2<\/li>\n<\/ul>\n\n\n\n

    Step 1: Calculate Total Moles of Gas<\/h3>\n\n\n\n

    [
    \\text{Total moles} = 6 + 2 = 8
    ]<\/p>\n\n\n\n

    Step 2: Mole Fraction of N\u2082<\/h3>\n\n\n\n

    [
    \\text{Mole fraction of N}_2 = \\frac{\\text{moles of N}_2}{\\text{total moles}}
    ]<\/p>\n\n\n\n

    [
    = \\frac{2}{8} = 0.25
    ]<\/p>\n\n\n\n

    Step 3: Calculate Partial Pressure of N\u2082<\/h3>\n\n\n\n

    [
    P_{\\text{N}2} = (\\text{Mole fraction of N}_2) \\times P<\/em>{\\text{total}}
    ]<\/p>\n\n\n\n

    [
    = 0.25 \\times 4
    ]<\/p>\n\n\n\n

    [
    = 1 \\text{ kgf\/cm}^2
    ]<\/p>\n\n\n\n

    Final Answer:<\/h3>\n\n\n\n

    The partial pressure of nitrogen ((N_2)) in the mixture is 1 kgf\/cm\u00b2.<\/strong><\/p>\n\n\n\n

    \n\n\n\n

    Explanation:<\/h3>\n\n\n\n

    Dalton\u2019s Law states that each gas in a mixture exerts pressure independently, proportional to its mole fraction. Since the total pressure is 4 kgf\/cm\u00b2, and nitrogen contributes 25% (from its mole fraction), its partial pressure is 1 kgf\/cm\u00b2. This principle applies universally to ideal gas mixtures.<\/p>\n\n\n\n

    Now, I’ll generate an image to illustrate this concept.<\/p>\n\n\n\n

    \"\"<\/figure>\n\n\n\n

    Here is the scientific diagram illustrating Dalton’s Law of Partial Pressures. It visually represents how nitrogen and hydrogen contribute to the total pressure of the gas mixture.<\/p>\n","protected":false},"excerpt":{"rendered":"

    A gas mixture contains 6 moles of H2 and 2 moles of N2. If the total pressure of the gaseous mixture is 4 kgf\/cm2; then the partial pressure of N2 in the mixture will be _ kgf\/cm2. The correct answer and explanation is : To find the partial pressure of nitrogen ((\\text{N}_2)) in the gas […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-196841","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/196841","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=196841"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/196841\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=196841"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=196841"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=196841"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}