{"id":41067,"date":"2025-06-28T05:22:17","date_gmt":"2025-06-28T05:22:17","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=41067"},"modified":"2025-06-28T05:22:18","modified_gmt":"2025-06-28T05:22:18","slug":"the-formula-for-dinitrogen-tetrafluoride-is-n2f4","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/the-formula-for-dinitrogen-tetrafluoride-is-n2f4\/","title":{"rendered":"The formula for dinitrogen tetrafluoride is N2F4."},"content":{"rendered":"\n

The formula for dinitrogen tetrafluoride is N2F4
F
. a. How many grams of nitrogen are present in 3.08 moles of dinitrogen tetrafluoride? grams b. How many moles of fluorine are present in 2.23 grams of dinitrogen tetrafluoride? moles<\/p>\n\n\n\n

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

Given compound:<\/strong>
Dinitrogen tetrafluoride \u2192 Formula: N\u2082F\u2084<\/strong><\/p>\n\n\n\n

\n\n\n\n

a. How many grams of nitrogen<\/strong> are in 3.08 moles<\/strong> of N\u2082F\u2084?<\/h3>\n\n\n\n

Step 1: Molar mass of nitrogen<\/h4>\n\n\n\n

Atomic mass of nitrogen (N) = 14.01 g\/mol
Each molecule of N\u2082F\u2084 has 2 nitrogen atoms<\/strong>, so:<\/p>\n\n\n\n

Mass of nitrogen per mole of N\u2082F\u2084 = 2 \u00d7 14.01 = 28.02 g<\/strong><\/p>\n\n\n\n

Step 2: Multiply by number of moles<\/h4>\n\n\n\n

Grams of nitrogen = 3.08 moles \u00d7 28.02 g\/mole
= 86.31 grams of nitrogen<\/strong><\/p>\n\n\n\n

\u2705 Answer for part (a):<\/strong> 86.31 grams<\/strong><\/p>\n\n\n\n

\n\n\n\n

b. How many moles of fluorine<\/strong> are in 2.23 grams<\/strong> of N\u2082F\u2084?<\/h3>\n\n\n\n

Step 1: Molar mass of N\u2082F\u2084<\/h4>\n\n\n\n
    \n
  • Nitrogen: 2 \u00d7 14.01 = 28.02 g<\/li>\n\n\n\n
  • Fluorine: 4 \u00d7 18.998 = 75.992 g<\/li>\n\n\n\n
  • Total = 28.02 + 75.992 = 104.012 g\/mol<\/strong><\/li>\n<\/ul>\n\n\n\n

    Step 2: Find moles of N\u2082F\u2084 in 2.23 g<\/h4>\n\n\n\n

    Moles = mass \u00f7 molar mass = 2.23 \u00f7 104.012 \u2248 0.02143 moles of N\u2082F\u2084<\/strong><\/p>\n\n\n\n

    Step 3: Fluorine atoms in one mole of N\u2082F\u2084<\/h4>\n\n\n\n

    Each mole of N\u2082F\u2084 has 4 moles of fluorine atoms<\/strong>, so:<\/p>\n\n\n\n

    Moles of fluorine = 0.02143 \u00d7 4 = 0.0857 moles<\/strong><\/p>\n\n\n\n

    \u2705 Answer for part (b):<\/strong> 0.0857 moles<\/strong><\/p>\n\n\n\n

    \n\n\n\n

    \ud83e\udde0 Explanation (300 words-ish)<\/h3>\n\n\n\n

    Dinitrogen tetrafluoride, N\u2082F\u2084, is a molecular compound consisting of two nitrogen atoms and four fluorine atoms. To solve stoichiometric problems like this, we rely on molar relationships and atomic masses from the periodic table.<\/p>\n\n\n\n

    For part (a), we wanted to know how many grams of nitrogen are in a given number of moles of N\u2082F\u2084. Since each molecule has two nitrogen atoms, we multiply the atomic mass of nitrogen by two to find the mass of nitrogen per mole of the compound. Then, by multiplying by the number of moles (3.08), we calculate the total grams of nitrogen.<\/p>\n\n\n\n

    In part (b), we worked in reverse. We began with grams and needed to find how many moles of fluorine atoms that represents. First, we calculated the molar mass of the entire compound (N\u2082F\u2084) to convert grams to moles. After that, we looked at the molecular formula again \u2014 each molecule has four fluorine atoms. Therefore, every mole of N\u2082F\u2084 contains 4 moles of fluorine atoms. By multiplying the number of moles of N\u2082F\u2084 by 4, we find the total moles of fluorine.<\/p>\n\n\n\n

    This process is a textbook example of how chemical formulas give us mole ratios, and how we can use those ratios to move between grams, moles, and even atoms if needed. Science magic, baby \ud83d\udd25\ud83e\uddea<\/p>\n\n\n\n

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

    The formula for dinitrogen tetrafluoride is N2F4F. a. How many grams of nitrogen are present in 3.08 moles of dinitrogen tetrafluoride? grams b. How many moles of fluorine are present in 2.23 grams of dinitrogen tetrafluoride? moles The Correct Answer and Explanation is: Given compound:Dinitrogen tetrafluoride \u2192 Formula: N\u2082F\u2084 a. How many grams of nitrogen […]<\/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-41067","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/41067","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=41067"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/41067\/revisions"}],"predecessor-version":[{"id":41069,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/41067\/revisions\/41069"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=41067"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=41067"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=41067"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}