To calculate the molar mass of Fe\u2082(SO\u2084)\u2083<\/strong>, we need to determine the mass contribution of each element in the formula.<\/p>\n\n\n\n The formula Fe\u2082(SO\u2084)\u2083<\/strong> contains:<\/p>\n\n\n\n Each sulfate ion contains:<\/p>\n\n\n\n Now calculate the total atoms:<\/p>\n\n\n\n Total molar mass = 111.70 + 96.21 + 192.00 = 399.91 g\/mol<\/strong><\/p>\n\n\n\n Avogadro\u2019s number is 6.022 \u00d7 10\u00b2\u00b3 formula units\/mol<\/strong>. The problem gives 4.05 \u00d7 10\u00b2\u00b3<\/strong> formula units. We need to find how many moles this represents.Moles of Fe\u2082(SO\u2084)\u2083=4.05\u00d710236.022\u00d71023=0.6726 mol\\text{Moles of Fe\u2082(SO\u2084)\u2083} = \\frac{4.05 \u00d7 10^{23}}{6.022 \u00d7 10^{23}} = 0.6726 \\text{ mol}Moles of Fe\u2082(SO\u2084)\u2083=6.022\u00d710234.05\u00d71023\u200b=0.6726 mol<\/p>\n\n\n\n Now multiply the number of moles by the molar mass:Mass=0.6726 mol\u00d7399.91 g\/mol=268.9 g\\text{Mass} = 0.6726 \\text{ mol} \u00d7 399.91 \\text{ g\/mol} = 268.9 \\text{ g}Mass=0.6726 mol\u00d7399.91 g\/mol=268.9 g<\/p>\n\n\n\n Rounded to three significant figures, the mass is:269 g Fe\u2082(SO\u2084)\u2083\\boxed{269 \\text{ g Fe\u2082(SO\u2084)\u2083}}269 g Fe\u2082(SO\u2084)\u2083\u200b<\/p>\n\n\n\n Iron(III) sulfate has a complex formula that requires careful accounting of each atom in the compound. We begin by breaking down the molar mass using atomic masses from the periodic table. After summing the contributions of all atoms, we use Avogadro\u2019s number to relate formula units to moles. Finally, multiplying the moles by the molar mass gives the total mass of the compound in grams. The precision of three significant figures matches the input value, which ensures consistency. This approach is fundamental in stoichiometry for converting between particles and measurable mass in chemistry.<\/p>\n\n\n\n Calculate the molar mass of Fe2(SO4)3. Then calculate the mass of iron(III) sulfate of 4.05×10^23 formula units. Answer: 269g Fe2(SO4)3 The Correct Answer and Explanation is: To calculate the molar mass of Fe\u2082(SO\u2084)\u2083, we need to determine the mass contribution of each element in the formula. Step 1: Calculate Molar Mass The formula Fe\u2082(SO\u2084)\u2083 contains: […]<\/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-39947","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/39947","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=39947"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/39947\/revisions"}],"predecessor-version":[{"id":39949,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/39947\/revisions\/39949"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=39947"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=39947"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=39947"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Step 1: Calculate Molar Mass<\/h3>\n\n\n\n
\n
\n
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\n\n\n\nStep 2: Use Avogadro\u2019s Number<\/h3>\n\n\n\n
\n\n\n\nStep 3: Calculate the Mass<\/h3>\n\n\n\n
\n\n\n\nExplanation<\/h3>\n\n\n\n
![\"\"](\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-1197.jpeg\")
<\/figure>\n","protected":false},"excerpt":{"rendered":"