{"id":11533,"date":"2020-11-30T09:25:18","date_gmt":"2020-11-30T03:55:18","guid":{"rendered":"https:\/\/cbselibrary.com\/?p=11533"},"modified":"2020-11-30T10:43:28","modified_gmt":"2020-11-30T05:13:28","slug":"molar-volume-gas-stp","status":"publish","type":"post","link":"https:\/\/cbselibrary.com\/molar-volume-gas-stp\/","title":{"rendered":"What is the Molar Volume of a Gas at STP?"},"content":{"rendered":"
People also ask<\/strong><\/p>\n 1. What is the volume of 0.4 mole of carbon dioxide gas at STP?<\/strong> 2. Find the number of moles of ammonia gas contained in a sample of 60 cm3<\/sup> of the gas at room conditions. [Molar volume: 24 dm3<\/sup> mol-1<\/sup> at room conditions]<\/strong> The following shows the relationships between the number of moles, number of particles, mass and volume of gases. In most calculations, we first convert other quantities such as the number of particles, mass or volume to the number of moles (refer to Table). 1. What is the volume of 12 g of methane at STP? <\/strong> 2. A sample of 120 cm3<\/sup> of carbon dioxide is collected at room conditions in an experiment. Calculate the mass of the sample of carbon dioxide.<\/strong> 3. How many hydrogen molecules are there in 6 dm3<\/sup> of hydrogen gas at room conditions? [Molar volume: 24 dm3<\/sup> mol-1<\/sup> at room conditions. Avogadro constant, NA: 6.02 \u00d7 1023<\/sup>\u00a0mol-1<\/sup>]<\/strong> 4. Find the volume of nitrogen gas in cm3<\/sup> at STP that consists of 2.408 \u00d7 1023<\/sup> nitrogen molecules. [Molar volume: 22.4 dm3<\/sup> mol-1<\/sup> at STP. Avogadro constant, Na: 6.02 \u00d7 1023<\/sup> mol-1<\/sup>]<\/strong> What is the Molar Volume of a Gas at STP? The Mole and the Volume of Gas It is rather tricky to find the number of moles of a gas by weighing its mass. Chemists determine the number of moles of any gas by measuring its volume. However, this cannot be done for solids and … Read more<\/a><\/p>\n","protected":false},"author":8,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"spay_email":""},"categories":[84],"tags":[4301,4303,4302],"yoast_head":"\n\n
The Mole and the Volume of Gas Problems with Solutions<\/h2>\n
\n[Molar volume: 22.4 dm3<\/sup> mol-1<\/sup> at STP]<\/strong>
\nSolution:<\/strong>
\nGiven the number of moles of carbon dioxide, CO2<\/sub> = 0.4 mol
\nTherefore, the volume of CO2<\/sub> = number of moles of CO2<\/sub> x molar volume at STP
\n= 0.4 x 22.4 dm3<\/sup> = 8.96 dm3<\/sup><\/p>\n
\nSolution:<\/strong>
\n<\/p>\nThe Relationship\u00a0Between Mole, Number of particles, Mass and Volume<\/h2>\n
\n<\/p>\n
\nTable: Summary of steps in calculations involving the number of moles<\/strong><\/p>\n\n\n
\n Conversion<\/strong><\/td>\n Steps<\/strong><\/td>\n<\/tr>\n \n From mass to volume<\/td>\n Mass \u2192 number of moles \u2192 volume<\/td>\n<\/tr>\n \n From volume to mass<\/td>\n Volume \u2192 number of moles \u2192 mass<\/td>\n<\/tr>\n \n From volume to number of particles<\/td>\n Volume \u2192 number of moles \u2192 number of particles<\/td>\n<\/tr>\n \n From number of particles to volume<\/td>\n Number of particles \u2192 number of moles \u2192 volume<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n The Relationship\u00a0Between Mole, Number of particles, Mass and Volume\u00a0Problems with Solutions<\/h2>\n
\n[Relative atomic mass: H, 1; C, 12. Molar volume: 22.4 dm3<\/sup> mol-1<\/sup> at STP]<\/strong>
\nSolution:<\/strong>
\n<\/p>\n
\n[Relative atomic mass: C, 12; O, 16. Molar volume: 24 dm3<\/sup> mol-1<\/sup> at room conditions]<\/strong>
\nSolution:<\/strong>
\nGiven the volume of carbon dioxide, CO2<\/sub>\u00a0= 120 cm3<\/sup> = 120\/1000 dm3<\/sup> = 0.12 dm3<\/sup>
\n
\nTherefore, the mass of CO2<\/sub> = number of moles of CO2<\/sub> \u00d7 molar mass of CO2<\/sub>\u00a0= 0.005 \u00d7 [12 + 2(16)]
\n= 0.005 \u00d7 44
\n= 0.22 g<\/p>\n
\nSolution:<\/strong>
\n<\/p>\n
\nSolution:<\/strong>
\n<\/p>\n","protected":false},"excerpt":{"rendered":"