calculate the mass of 2*10power 10 molecules of nitrogen gas<\/p>\n\n\n\n
The correct answer and explanation is:<\/strong><\/mark><\/p>\n\n\n\n To calculate the mass of 2\u00d710102 \\times 10^{10}<\/strong> molecules of nitrogen gas (N\u2082)<\/strong>, we will use the following steps:<\/p>\n\n\n\n Avogadro’s number tells us how many molecules are in 1 mole<\/strong> of any substance: NA=6.022\u00d71023 molecules\/molN_A = 6.022 \\times 10^{23} \\text{ molecules\/mol}<\/p>\n\n\n\n The atomic mass of nitrogen (N) is approximately 14.01 g\/mol<\/strong>, so: Molar mass of N2=2\u00d714.01=28.02 g\/mol\\text{Molar mass of N}_2 = 2 \\times 14.01 = 28.02 \\text{ g\/mol}<\/p>\n\n\n\n We are given: Number of molecules=2\u00d71010\\text{Number of molecules} = 2 \\times 10^{10}<\/p>\n\n\n\n To find the number of moles<\/strong>, divide the number of molecules by Avogadro\u2019s number: Moles=2\u00d710106.022\u00d71023\u22483.32\u00d710\u221214 mol\\text{Moles} = \\frac{2 \\times 10^{10}}{6.022 \\times 10^{23}} \\approx 3.32 \\times 10^{-14} \\text{ mol}<\/p>\n\n\n\n Now, multiply the number of moles by the molar mass: Mass=moles\u00d7molar mass\\text{Mass} = \\text{moles} \\times \\text{molar mass} Mass=(3.32\u00d710\u221214)\u00d728.02\u22489.3\u00d710\u221213 g\\text{Mass} = (3.32 \\times 10^{-14}) \\times 28.02 \\approx 9.3 \\times 10^{-13} \\text{ g}<\/p>\n\n\n\n 9.3\u00d710\u221213 grams\\boxed{9.3 \\times 10^{-13} \\text{ grams}}<\/p>\n\n\n\n To determine the mass of a specific number of nitrogen gas molecules, we need to connect microscopic particles (molecules) to macroscopic units (grams). This is made possible by Avogadro’s number<\/strong>, which relates the number of particles in a mole\u2014one of the fundamental units in chemistry.<\/p>\n\n\n\n Avogadro\u2019s number, 6.022\u00d710236.022 \\times 10^{23}, indicates that a mole contains that many molecules. If we are given a much smaller number of molecules, like 2\u00d710102 \\times 10^{10}, we first convert this to moles<\/strong> by dividing it by Avogadro\u2019s number. This gives us a very tiny number of moles (3.32\u00d710\u2212143.32 \\times 10^{-14}), since 2\u00d710102 \\times 10^{10} molecules is just a minuscule fraction of a mole.<\/p>\n\n\n\n Next, we use the molar mass<\/strong> of nitrogen gas (N\u2082), which is about 28.02 g\/mol. This value tells us the mass of one mole of nitrogen gas. By multiplying our small number of moles by this molar mass, we find the actual mass of our sample.<\/p>\n\n\n\n In this case, the final answer is approximately 9.3\u00d710\u2212139.3 \\times 10^{-13} grams\u2014an extremely small quantity, which makes sense given the very small number of molecules. This type of calculation is foundational in chemistry, especially when working with molecular scales in areas such as stoichiometry, gas laws, or molecular biology.<\/p>\n","protected":false},"excerpt":{"rendered":" calculate the mass of 2*10power 10 molecules of nitrogen gas The correct answer and explanation is: To calculate the mass of 2\u00d710102 \\times 10^{10} molecules of nitrogen gas (N\u2082), we will use the following steps: \u2705 Step 1: Use Avogadro\u2019s Number Avogadro’s number tells us how many molecules are in 1 mole of any substance: […]<\/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-20556","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/20556","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=20556"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/20556\/revisions"}],"predecessor-version":[{"id":20557,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/20556\/revisions\/20557"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=20556"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=20556"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=20556"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
\n\n\n\n\u2705 Step 1: Use Avogadro\u2019s Number<\/strong><\/h3>\n\n\n\n
\n\n\n\n\u2705 Step 2: Find the Molar Mass of N\u2082<\/strong><\/h3>\n\n\n\n
\n\n\n\n\u2705 Step 3: Convert Molecules to Moles<\/strong><\/h3>\n\n\n\n
\n\n\n\n\u2705 Step 4: Calculate the Mass<\/strong><\/h3>\n\n\n\n
\n\n\n\n\u2705 Final Answer:<\/strong><\/h3>\n\n\n\n
\n\n\n\n\ud83e\udde0 Explanation (300 words)<\/strong><\/h3>\n\n\n\n