How many moles of cobalt are in 1.80e22 cobalt atoms?<\/p>\n\n\n\n
The correct answer and explanation is:<\/mark><\/strong><\/p>\n\n\n\n To find how many moles of cobalt<\/strong> are in 1.80 \u00d7 10\u00b2\u00b2 atoms of cobalt<\/strong>, use Avogadro’s number<\/strong>, which is:<\/p>\n\n\n\n 6.022 \u00d7 10\u00b2\u00b3 atoms\/mol<\/strong><\/p>\n\n\n\n Moles of cobalt=Number of atomsAvogadro\u2019s number=1.80\u00d710226.022\u00d71023\\text{Moles of cobalt} = \\frac{\\text{Number of atoms}}{\\text{Avogadro’s number}} = \\frac{1.80 \\times 10^{22}}{6.022 \\times 10^{23}} =0.02989 mol= 0.02989\\ \\text{mol}<\/p>\n\n\n\n Rounded to three significant figures: 0.0299 mol of cobalt\\boxed{0.0299\\ \\text{mol of cobalt}}<\/p>\n\n\n\n A mole<\/strong> is a standard unit in chemistry used to express amounts of a chemical substance. One mole of any element contains 6.022 \u00d7 10\u00b2\u00b3 particles<\/strong> (atoms, molecules, ions, etc.). This number is known as Avogadro\u2019s number<\/strong>.<\/p>\n\n\n\n In this case, the goal is to determine how many moles of cobalt are present in 1.80 \u00d7 10\u00b2\u00b2 atoms<\/strong>. To do this, the number of atoms must be divided by Avogadro\u2019s number. This gives a ratio that tells how many groups of 6.022 \u00d7 10\u00b2\u00b3 atoms are present in the sample. Because the number of atoms given is smaller than Avogadro’s number, the result is less than one mole.<\/p>\n\n\n\n The formula applied is: Moles=Atoms6.022\u00d71023\\text{Moles} = \\frac{\\text{Atoms}}{6.022 \\times 10^{23}}<\/p>\n\n\n\n This method works because the definition of a mole is tied directly to this constant. In practical terms, the result tells that 1.80 \u00d7 10\u00b2\u00b2 cobalt atoms make up about 0.0299 moles<\/strong> of cobalt.<\/p>\n\n\n\n Understanding moles is essential in chemistry for converting between the microscopic world (atoms and molecules) and the macroscopic world (grams and liters). It is especially helpful in stoichiometry, where balanced chemical equations are used to calculate the amounts of reactants and products in a reaction.<\/p>\n","protected":false},"excerpt":{"rendered":" How many moles of cobalt are in 1.80e22 cobalt atoms? The correct answer and explanation is: To find how many moles of cobalt are in 1.80 \u00d7 10\u00b2\u00b2 atoms of cobalt, use Avogadro’s number, which is: 6.022 \u00d7 10\u00b2\u00b3 atoms\/mol Step-by-step Solution: Moles of cobalt=Number of atomsAvogadro\u2019s number=1.80\u00d710226.022\u00d71023\\text{Moles of cobalt} = \\frac{\\text{Number of atoms}}{\\text{Avogadro’s number}} = \\frac{1.80 \\times 10^{22}}{6.022 \\times […]<\/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-34791","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/34791","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=34791"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/34791\/revisions"}],"predecessor-version":[{"id":34792,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/34791\/revisions\/34792"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=34791"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=34791"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=34791"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
\n\n\n\nStep-by-step Solution:<\/h3>\n\n\n\n
\n\n\n\nExplanation (300 words):<\/h3>\n\n\n\n