{"id":28747,"date":"2025-06-20T15:03:58","date_gmt":"2025-06-20T15:03:58","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=28747"},"modified":"2025-06-20T15:03:59","modified_gmt":"2025-06-20T15:03:59","slug":"when-ammonia-reacts-with-oxygen-nitrogen-monoxide-and-water-are-produced","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/when-ammonia-reacts-with-oxygen-nitrogen-monoxide-and-water-are-produced\/","title":{"rendered":"When ammonia reacts with oxygen, nitrogen monoxide and water are produced."},"content":{"rendered":"\n<p>When ammonia reacts with oxygen, nitrogen monoxide and water are produced. The balanced equation for this reaction is: 4NH3 (g) + 5O2 (g) \u00e2\u2020\u2019 4NO (g) + 6H2O (g) If 16 moles of ammonia react, the reaction consumes 20 moles of oxygen. The reaction produces 16 moles of nitrogen monoxide and 24 moles of water<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-vivid-green-cyan-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p><strong>Correct Answer:<\/strong><\/p>\n\n\n\n<p>Yes, the reaction consumes 20 moles of oxygen, produces 16 moles of nitrogen monoxide, and produces 24 moles of water when 16 moles of ammonia react.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>Explanation <\/strong><\/p>\n\n\n\n<p>To determine if the numbers are correct, we begin with the balanced chemical equation for the reaction between ammonia and oxygen:<\/p>\n\n\n\n<p><strong>4NH\u2083 (g) + 5O\u2082 (g) \u2192 4NO (g) + 6H\u2082O (g)<\/strong><\/p>\n\n\n\n<p>This equation tells us that 4 moles of ammonia (NH\u2083) react with 5 moles of oxygen (O\u2082) to produce 4 moles of nitrogen monoxide (NO) and 6 moles of water (H\u2082O).<\/p>\n\n\n\n<p>This is a mole ratio. From the equation, for every 4 moles of NH\u2083, we need:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>5 moles of O\u2082<\/li>\n\n\n\n<li>We produce 4 moles of NO<\/li>\n\n\n\n<li>We produce 6 moles of H\u2082O<\/li>\n<\/ul>\n\n\n\n<p>Now, we scale the entire equation up based on the amount of ammonia given in the question, which is 16 moles.<\/p>\n\n\n\n<p>Since 16 moles is 4 times the original 4 moles of NH\u2083 in the balanced equation, we must multiply every other substance in the equation by 4:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>O\u2082: 5 moles \u00d7 4 = 20 moles required<\/li>\n\n\n\n<li>NO: 4 moles \u00d7 4 = 16 moles produced<\/li>\n\n\n\n<li>H\u2082O: 6 moles \u00d7 4 = 24 moles produced<\/li>\n<\/ul>\n\n\n\n<p>So, reacting 16 moles of ammonia would consume <strong>20 moles of oxygen<\/strong>, produce <strong>16 moles of nitrogen monoxide<\/strong>, and produce <strong>24 moles of water<\/strong>.<\/p>\n\n\n\n<p>The quantities in the question match exactly with the stoichiometry of the balanced equation. Therefore, the answer is <strong>correct<\/strong>, and the mole relationships are consistent with the balanced reaction. This example demonstrates how mole ratios from balanced equations can be used to predict the amounts of reactants and products in a chemical reaction.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"852\" height=\"1024\" src=\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-246.jpeg\" alt=\"\" class=\"wp-image-28748\" srcset=\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-246.jpeg 852w, https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-246-250x300.jpeg 250w, https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-246-768x923.jpeg 768w\" sizes=\"auto, (max-width: 852px) 100vw, 852px\" \/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>When ammonia reacts with oxygen, nitrogen monoxide and water are produced. The balanced equation for this reaction is: 4NH3 (g) + 5O2 (g) \u00e2\u2020\u2019 4NO (g) + 6H2O (g) If 16 moles of ammonia react, the reaction consumes 20 moles of oxygen. The reaction produces 16 moles of nitrogen monoxide and 24 moles of water [&hellip;]<\/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-28747","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/28747","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=28747"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/28747\/revisions"}],"predecessor-version":[{"id":28749,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/28747\/revisions\/28749"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=28747"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=28747"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=28747"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}