{"id":39075,"date":"2025-06-26T19:03:38","date_gmt":"2025-06-26T19:03:38","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=39075"},"modified":"2025-06-26T19:03:38","modified_gmt":"2025-06-26T19:03:38","slug":"how-many-c2h4-molecules-are-in-45-8-g-of-c2h4","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/how-many-c2h4-molecules-are-in-45-8-g-of-c2h4\/","title":{"rendered":"How many C2H4 molecules are in 45.8 g of C2H4"},"content":{"rendered":"\n

How many C2H4 molecules are in 45.8 g of C2H4? The molar mass of C2H4 is 28.05 g\/mol. Group of answer choices 3.69 x 1023 C2H4 molecules 9.83 x 1023 C2H4 molecules 4.69 x 1026 C2H4 molecules 2.71 x 1023 C2H4 molecules 7.74 x 1026 C2H4 molecules<\/p>\n\n\n\n

The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n

To find how many C\u2082H\u2084 molecules<\/strong> are in 45.8 grams<\/strong> of C\u2082H\u2084, we use the following steps:<\/p>\n\n\n\n

\n\n\n\n

Step 1: Use the molar mass to find moles<\/h3>\n\n\n\n

Given:<\/p>\n\n\n\n

    \n
  • Mass of ethene (C\u2082H\u2084) = 45.8 grams<\/li>\n\n\n\n
  • Molar mass of C\u2082H\u2084 = 28.05 g\/mol<\/li>\n<\/ul>\n\n\n\n

    Moles of C\u2082H\u2084 =<\/strong>massmolar mass=45.8 g28.05 g\/mol\u22481.633 mol\\frac{\\text{mass}}{\\text{molar mass}} = \\frac{45.8\\ \\text{g}}{28.05\\ \\text{g\/mol}} \\approx 1.633\\ \\text{mol}molar massmass\u200b=28.05 g\/mol45.8 g\u200b\u22481.633 mol<\/p>\n\n\n\n

    \n\n\n\n

    Step 2: Use Avogadro’s number to convert moles to molecules<\/h3>\n\n\n\n

    Avogadro\u2019s number is6.022\u00d71023 molecules\/mol6.022 \\times 10^{23}\\ \\text{molecules\/mol}6.022\u00d71023 molecules\/mol<\/p>\n\n\n\n

    So the number of molecules is1.633 mol\u00d76.022\u00d71023 molecules\/mol\u22489.83\u00d71023 molecules1.633\\ \\text{mol} \\times 6.022 \\times 10^{23}\\ \\text{molecules\/mol} \\approx 9.83 \\times 10^{23}\\ \\text{molecules}1.633 mol\u00d76.022\u00d71023 molecules\/mol\u22489.83\u00d71023 molecules<\/p>\n\n\n\n

    \n\n\n\n

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

    9.83 \u00d7 10\u00b2\u00b3 C\u2082H\u2084 molecules<\/strong><\/p>\n\n\n\n

    \n\n\n\n

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

    To determine the number of ethene molecules in a given mass, we must connect grams to individual particles using two key concepts: molar mass<\/strong> and Avogadro’s number<\/strong>. The molar mass of a compound tells us how many grams are in one mole of that substance. For ethene, or C\u2082H\u2084, the molar mass is 28.05 grams per mole. This means one mole of ethene weighs 28.05 grams and contains exactly 6.022 \u00d7 10\u00b2\u00b3 molecules, which is Avogadro’s constant.<\/p>\n\n\n\n

    We start by converting grams into moles. This is done by dividing the mass of the sample by its molar mass. For 45.8 grams of ethene, we divide by 28.05 g\/mol, giving approximately 1.633 moles. Each mole represents a very large number of molecules, so we then multiply the number of moles by Avogadro\u2019s number to find the actual count of molecules.<\/p>\n\n\n\n

    When 1.633 moles are multiplied by 6.022 \u00d7 10\u00b2\u00b3, the result is around 9.83 \u00d7 10\u00b2\u00b3 molecules. This is the total number of ethene molecules in 45.8 grams of the compound.<\/p>\n\n\n\n

    This process shows how chemical quantities in grams relate to microscopic quantities of particles. It is a fundamental concept in chemistry, helping chemists understand how much of a substance is present at the molecular level, even when working with amounts that are visible and measurable in a laboratory setting.<\/p>\n\n\n\n

    \n\n\n\n

    \u2705 Correct choice: 9.83 \u00d7 10\u00b2\u00b3 C\u2082H\u2084 molecules<\/strong><\/p>\n\n\n\n

    \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

    How many C2H4 molecules are in 45.8 g of C2H4? The molar mass of C2H4 is 28.05 g\/mol. Group of answer choices 3.69 x 1023 C2H4 molecules 9.83 x 1023 C2H4 molecules 4.69 x 1026 C2H4 molecules 2.71 x 1023 C2H4 molecules 7.74 x 1026 C2H4 molecules The Correct Answer and Explanation is: To find […]<\/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-39075","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/39075","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=39075"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/39075\/revisions"}],"predecessor-version":[{"id":39077,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/39075\/revisions\/39077"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=39075"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=39075"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=39075"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}