A chemist weighed out 20.0 g of magnesium. Calculate the number of moles of magnesium she weighed out.<\/p>\n\n\n\n
The correct answer and explanation is:<\/strong><\/mark><\/p>\n\n\n\n To calculate the number of moles of magnesium in 20.0 grams, use the mole formula<\/strong>: Moles=Mass (g)Molar Mass (g\/mol)\\text{Moles} = \\frac{\\text{Mass (g)}}{\\text{Molar Mass (g\/mol)}}<\/p>\n\n\n\n The molar mass<\/strong> of magnesium (Mg) is approximately 24.31 g\/mol<\/strong>. Moles of Mg=20.0 g24.31 g\/mol\u22480.823 mol\\text{Moles of Mg} = \\frac{20.0\\ \\text{g}}{24.31\\ \\text{g\/mol}} \\approx 0.823\\ \\text{mol}<\/p>\n\n\n\n In chemistry, the mole<\/strong> is a fundamental unit in the International System of Units (SI) used to express the amount of a substance. One mole of any element contains Avogadro\u2019s number<\/strong> of particles, which is approximately 6.022\u00d710236.022 \\times 10^{23} atoms, molecules, or ions. The molar mass<\/strong> is the mass of one mole of an element or compound, expressed in grams per mole (g\/mol), and is numerically equal to the atomic or molecular weight found on the periodic table.<\/p>\n\n\n\n Magnesium (Mg) is an element with an atomic number of 12 and a molar mass of approximately 24.31 g\/mol<\/strong>. This means that one mole of magnesium weighs 24.31 grams. If a chemist weighs 20.0 grams<\/strong> of magnesium, to determine how many moles this represents, we use the formula: Moles=MassMolar Mass\\text{Moles} = \\frac{\\text{Mass}}{\\text{Molar Mass}}<\/p>\n\n\n\n Substituting the values: Moles=20.024.31\u22480.823\\text{Moles} = \\frac{20.0}{24.31} \\approx 0.823<\/p>\n\n\n\n This tells us that 20.0 grams of magnesium corresponds to approximately 0.823 moles<\/strong> of magnesium atoms.<\/p>\n\n\n\n Understanding how to convert between grams and moles is essential in chemistry for tasks such as preparing solutions, balancing chemical reactions, and calculating yields. It allows chemists to relate a measurable quantity (mass in grams) to the number of particles involved in a reaction, which is critical when performing stoichiometric calculations in laboratory and industrial settings.<\/p>\n","protected":false},"excerpt":{"rendered":" A chemist weighed out 20.0 g of magnesium. Calculate the number of moles of magnesium she weighed out. The correct answer and explanation is: To calculate the number of moles of magnesium in 20.0 grams, use the mole formula: Moles=Mass (g)Molar Mass (g\/mol)\\text{Moles} = \\frac{\\text{Mass (g)}}{\\text{Molar Mass (g\/mol)}} The molar mass of magnesium (Mg) is approximately 24.31 g\/mol. […]<\/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-16263","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/16263","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=16263"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/16263\/revisions"}],"predecessor-version":[{"id":16264,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/16263\/revisions\/16264"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=16263"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=16263"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=16263"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}\u2705 Final Answer: 0.823 moles of magnesium<\/strong><\/h3>\n\n\n\n
\n\n\n\n\u270d\ufe0f Explanation (300 words):<\/h3>\n\n\n\n