{"id":17285,"date":"2025-06-12T10:53:29","date_gmt":"2025-06-12T10:53:29","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=17285"},"modified":"2025-06-12T10:53:33","modified_gmt":"2025-06-12T10:53:33","slug":"which-reactant-is-limiting-when-5-moles-of-n2-gas-react-with-10-moles-of-h2-gas-to-make-ammonia","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/which-reactant-is-limiting-when-5-moles-of-n2-gas-react-with-10-moles-of-h2-gas-to-make-ammonia\/","title":{"rendered":"which reactant is limiting when 5 moles of N2 gas react with 10 moles of H2 gas to make ammonia"},"content":{"rendered":"\n

which reactant is limiting when 5 moles of N2 gas react with 10 moles of H2 gas to make ammonia?<\/p>\n\n\n\n

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

To determine the limiting reactant<\/strong> in the reaction between nitrogen gas (N\u2082) and hydrogen gas (H\u2082) to form ammonia (NH\u2083)<\/strong>, we first look at the balanced chemical equation<\/strong>: N2+3H2\u21922NH3\\text{N}_2 + 3\\text{H}_2 \\rightarrow 2\\text{NH}_3<\/p>\n\n\n\n

Step 1: Understand the mole ratio<\/h3>\n\n\n\n

From the balanced equation:<\/p>\n\n\n\n

    \n
  • 1 mole of N\u2082<\/strong> reacts with 3 moles of H\u2082<\/strong>.<\/li>\n<\/ul>\n\n\n\n

    Step 2: Compare available moles<\/h3>\n\n\n\n

    We are given:<\/p>\n\n\n\n

      \n
    • 5 moles of N\u2082<\/li>\n\n\n\n
    • 10 moles of H\u2082<\/li>\n<\/ul>\n\n\n\n

      Now, let\u2019s see how many moles of H\u2082 are needed to fully react with the 5 moles of N\u2082: 5 mol N2\u00d73 mol H21 mol N2=15 mol H25 \\text{ mol N}_2 \\times \\frac{3 \\text{ mol H}_2}{1 \\text{ mol N}_2} = 15 \\text{ mol H}_2<\/p>\n\n\n\n

      So, we need 15 moles<\/strong> of H\u2082 to react with 5 moles of N\u2082, but we only have 10 moles<\/strong> of H\u2082.<\/p>\n\n\n\n

      Step 3: Identify the limiting reactant<\/h3>\n\n\n\n

      Since we don\u2019t have enough H\u2082<\/strong>, it will run out first. Therefore, H\u2082 is the limiting reactant<\/strong>.<\/p>\n\n\n\n

      \n\n\n\n

      Explanation (Approx. 300 words):<\/h3>\n\n\n\n

      In chemical reactions, the limiting reactant<\/strong> is the substance that is completely used up first, limiting the amount of product formed. To determine the limiting reactant between nitrogen gas (N\u2082) and hydrogen gas (H\u2082) in the synthesis of ammonia (NH\u2083), we must use the balanced chemical equation: N2+3H2\u21922NH3\\text{N}_2 + 3\\text{H}_2 \\rightarrow 2\\text{NH}_3<\/p>\n\n\n\n

      This tells us that for every 1 mole of nitrogen, 3 moles of hydrogen are required. Given 5 moles of N\u2082 and 10 moles of H\u2082, we calculate how much hydrogen would be needed to react with all the nitrogen: 5 mol N2\u00d73=15 mol H25 \\text{ mol N}_2 \\times 3 = 15 \\text{ mol H}_2<\/p>\n\n\n\n

      However, we only have 10 moles of hydrogen, which is insufficient. Because we don\u2019t have the full 15 moles needed, the reaction cannot consume all 5 moles of nitrogen. Hydrogen will be used up first, stopping the reaction from proceeding further. That makes hydrogen the limiting reactant<\/strong>.<\/p>\n\n\n\n

      Identifying the limiting reactant is important in stoichiometry because it determines the maximum amount of product that can be formed. Even if there\u2019s excess of the other reactant, the reaction stops once the limiting one is gone. In this case, since H\u2082 is the limiting reactant, the amount of ammonia produced depends on the 10 moles of hydrogen available.<\/p>\n","protected":false},"excerpt":{"rendered":"

      which reactant is limiting when 5 moles of N2 gas react with 10 moles of H2 gas to make ammonia? The correct answer and explanation is: To determine the limiting reactant in the reaction between nitrogen gas (N\u2082) and hydrogen gas (H\u2082) to form ammonia (NH\u2083), we first look at the balanced chemical equation: N2+3H2\u21922NH3\\text{N}_2 […]<\/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-17285","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/17285","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=17285"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/17285\/revisions"}],"predecessor-version":[{"id":17286,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/17285\/revisions\/17286"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=17285"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=17285"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=17285"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}