How many C2H 4 molecules are contained in 45.8 mg of C2H 4? The molar mass of C2H 4 is 28.05 g\/mol.<\/p>\n\n\n\n
7.74 x 1026 C2H4 molecules
4.69 x 1023 C2H4 molecules
3.69 x 1023 C2H4 molecules
9.83 x 1020 C2H4 molecules
% 1020 C2H4 molecules<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n To determine how many molecules of C\u2082H\u2084 (ethylene) are contained in 45.8 mg of C\u2082H\u2084, we need to go through the following steps:<\/p>\n\n\n\n We are given 45.8 mg of C\u2082H\u2084, but we need the mass in grams. Since there are 1000 mg in 1 g:<\/p>\n\n\n\n [ Next, we use the molar mass of C\u2082H\u2084 to convert the mass into moles. The molar mass of C\u2082H\u2084 is given as 28.05 g\/mol. The number of moles (n) can be calculated using the formula:<\/p>\n\n\n\n [ Substituting the known values:<\/p>\n\n\n\n [ To calculate the number of molecules, we use Avogadro’s number, which is (6.022 \\times 10^{23}) molecules per mole. The number of molecules is:<\/p>\n\n\n\n [ Where (N_A) is Avogadro\u2019s number. Substituting the values:<\/p>\n\n\n\n [ [ The correct answer is 9.83 \u00d7 10\u00b2\u2070<\/strong> molecules of C\u2082H\u2084.<\/p>\n\n\n\n In this problem, we used basic stoichiometric conversions. First, we converted the given mass to grams, then used the molar mass of C\u2082H\u2084 to find the number of moles. Finally, we multiplied by Avogadro\u2019s number to find the number of molecules. This is a standard process in chemistry to determine the number of molecules or atoms in a given sample.<\/p>\n","protected":false},"excerpt":{"rendered":" How many C2H 4 molecules are contained in 45.8 mg of C2H 4? The molar mass of C2H 4 is 28.05 g\/mol. 7.74 x 1026 C2H4 molecules4.69 x 1023 C2H4 molecules3.69 x 1023 C2H4 molecules9.83 x 1020 C2H4 molecules% 1020 C2H4 molecules The Correct Answer and Explanation is : To determine how many molecules of […]<\/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-189438","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/189438","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=189438"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/189438\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=189438"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=189438"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=189438"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Step 1: Convert mass to grams<\/h3>\n\n\n\n
45.8 \\, \\text{mg} = \\frac{45.8}{1000} \\, \\text{g} = 0.0458 \\, \\text{g}
]<\/p>\n\n\n\nStep 2: Calculate the number of moles of C\u2082H\u2084<\/h3>\n\n\n\n
n = \\frac{\\text{mass}}{\\text{molar mass}}
]<\/p>\n\n\n\n
n = \\frac{0.0458 \\, \\text{g}}{28.05 \\, \\text{g\/mol}} = 0.001634 \\, \\text{mol}
]<\/p>\n\n\n\nStep 3: Calculate the number of molecules<\/h3>\n\n\n\n
\\text{Number of molecules} = n \\times N_A
]<\/p>\n\n\n\n
\\text{Number of molecules} = 0.001634 \\, \\text{mol} \\times 6.022 \\times 10^{23} \\, \\text{molecules\/mol}
]<\/p>\n\n\n\n
\\text{Number of molecules} = 9.83 \\times 10^{20} \\, \\text{molecules}
]<\/p>\n\n\n\nConclusion:<\/h3>\n\n\n\n
Explanation:<\/h3>\n\n\n\n