How many liters of gas are found in 0.15 moles of chlorine gas?<\/p>\n\n\n\n
The correct answer and explanation is:<\/strong><\/mark><\/p>\n\n\n\n Correct Answer:<\/strong><\/p>\n\n\n\n At standard temperature and pressure (STP), 0.15 moles of chlorine gas (Cl\u2082)<\/strong> occupy approximately 3.36 liters<\/strong>.<\/p>\n\n\n\n To determine how many liters of chlorine gas are present in 0.15 moles, we use the concept of molar volume of a gas<\/strong> at standard temperature and pressure (STP)<\/strong>.<\/p>\n\n\n\n STP<\/strong> is defined as:<\/p>\n\n\n\n At STP, 1 mole of any ideal gas occupies 22.4 liters<\/strong>.<\/p>\n\n\n\n We are given:<\/p>\n\n\n\n Use the formula: Volume (L)=Moles\u00d7Molar Volume\\text{Volume (L)} = \\text{Moles} \\times \\text{Molar Volume} Volume=0.15\u2009mol\u00d722.4\u2009L\/mol=3.36\u2009L\\text{Volume} = 0.15 \\, \\text{mol} \\times 22.4 \\, \\text{L\/mol} = 3.36 \\, \\text{L}<\/p>\n\n\n\n So, 0.15 moles of Cl\u2082 gas occupy 3.36 liters at STP<\/strong>.<\/p>\n\n\n\n Chlorine gas (Cl\u2082) behaves like an ideal gas under standard conditions. The ideal gas law relates pressure, volume, temperature, and amount of gas. At STP, the molar volume simplifies calculations: PV=nRT\u21d2V=nRTPPV = nRT \\Rightarrow V = \\frac{nRT}{P}<\/p>\n\n\n\n Where:<\/p>\n\n\n\n At STP, these values are constant, leading to the standardized 22.4 L per mole<\/strong>.<\/p>\n\n\n\n This method is widely used in chemistry for quick estimations involving gases when conditions are known to be STP. If the temperature or pressure differs from STP, the ideal gas law must be used with actual values.<\/p>\n","protected":false},"excerpt":{"rendered":" How many liters of gas are found in 0.15 moles of chlorine gas? The correct answer and explanation is: Correct Answer: At standard temperature and pressure (STP), 0.15 moles of chlorine gas (Cl\u2082) occupy approximately 3.36 liters. Explanation (Approx. 300 Words): To determine how many liters of chlorine gas are present in 0.15 moles, we […]<\/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-26684","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/26684","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=26684"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/26684\/revisions"}],"predecessor-version":[{"id":26685,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/26684\/revisions\/26685"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=26684"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=26684"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=26684"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
\n\n\n\nExplanation (Approx. 300 Words):<\/strong><\/h3>\n\n\n\n
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Step-by-Step Calculation:<\/strong><\/h4>\n\n\n\n
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\n\n\n\nWhy This Works:<\/strong><\/h3>\n\n\n\n
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