How many formula units are contained in 23.5g of Sb2S3<\/p>\n\n\n\n
The correct answer and explanation is:<\/strong><\/mark><\/p>\n\n\n\n Let’s solve the problem step-by-step.<\/p>\n\n\n\n How many formula units are contained in 23.5 g<\/strong> of Sb\u2082S\u2083<\/strong> (antimony(III) sulfide)?<\/p>\n\n\n\n Molar mass of Sb\u2082S\u2083 = (2 \u00d7 121.76) + (3 \u00d7 32.06) Number of moles = mass \/ molar mass 1 mole of any substance contains 6.022 \u00d7 10\u00b2\u00b3<\/strong> formula units (Avogadro’s number).<\/p>\n\n\n\n Number of formula units = moles \u00d7 Avogadro’s number 23.5 g of Sb\u2082S\u2083 contains approximately 4.17 \u00d7 10\u00b2\u00b2 formula units.<\/strong><\/p>\n\n\n\n When dealing with compounds like Sb\u2082S\u2083, we often want to know how many discrete units of the compound are present in a certain mass. These discrete units are called formula units<\/strong> for ionic or covalent network compounds, analogous to molecules in molecular substances.<\/p>\n\n\n\n The first step is to determine the molar mass of Sb\u2082S\u2083. This is the mass of one mole of the compound and is found by adding the atomic masses of all the atoms in one formula unit. Antimony (Sb) has an atomic mass of about 121.76 g\/mol, and sulfur (S) has an atomic mass of 32.06 g\/mol. Since Sb\u2082S\u2083 contains 2 atoms of Sb and 3 atoms of S, we multiply accordingly and sum these masses, which results in approximately 339.70 g\/mol.<\/p>\n\n\n\n Next, you find how many moles are in the 23.5 g sample by dividing the sample\u2019s mass by the molar mass. This gives approximately 0.0692 moles. A mole represents a quantity of particles equal to Avogadro’s number (6.022 \u00d7 10\u00b2\u00b3).<\/p>\n\n\n\n Finally, to get the total number of formula units, multiply the number of moles by Avogadro\u2019s number. This conversion allows us to go from macroscopic quantities of a compound to the microscopic number of particles. The result is about 4.17 \u00d7 10\u00b2\u00b2 formula units.<\/p>\n\n\n\n This calculation is useful in chemistry because many reactions and properties depend on the number of formula units or molecules, not just the mass, allowing chemists to understand and predict how substances will behave at the microscopic level.<\/p>\n","protected":false},"excerpt":{"rendered":" How many formula units are contained in 23.5g of Sb2S3 The correct answer and explanation is: Let’s solve the problem step-by-step. Question: How many formula units are contained in 23.5 g of Sb\u2082S\u2083 (antimony(III) sulfide)? Step 1: Find the molar mass of Sb\u2082S\u2083 Molar mass of Sb\u2082S\u2083 = (2 \u00d7 121.76) + (3 \u00d7 32.06)= […]<\/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-21723","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/21723","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=21723"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/21723\/revisions"}],"predecessor-version":[{"id":21724,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/21723\/revisions\/21724"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=21723"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=21723"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=21723"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
\n\n\n\nQuestion:<\/h3>\n\n\n\n
\n\n\n\nStep 1: Find the molar mass of Sb\u2082S\u2083<\/h3>\n\n\n\n
\n
= 243.52 + 96.18
= 339.70 g\/mol<\/strong><\/p>\n\n\n\n
\n\n\n\nStep 2: Calculate the number of moles in 23.5 g of Sb\u2082S\u2083<\/h3>\n\n\n\n
= 23.5 g \/ 339.70 g\/mol
\u2248 0.0692 moles<\/strong><\/p>\n\n\n\n
\n\n\n\nStep 3: Calculate the number of formula units<\/h3>\n\n\n\n
= 0.0692 \u00d7 6.022 \u00d7 10\u00b2\u00b3
\u2248 4.17 \u00d7 10\u00b2\u00b2 formula units<\/strong><\/p>\n\n\n\n
\n\n\n\nFinal answer:<\/h3>\n\n\n\n
\n\n\n\nExplanation (300 words):<\/h3>\n\n\n\n