[{"data":1,"prerenderedAt":-1},["ShallowReactive",2],{"doc-detail-207946-en":3,"doc-seo-207946-105":30,"detail-sidebar-cat-0-en-105":90},{"code":4,"msg":5,"data":6},0,"success",{"doc_id":7,"user_id":8,"nickname":9,"user_avatar":10,"doc_module":4,"category_id":11,"category_name":12,"doc_title":13,"doc_description":14,"doc_content":15,"file_id":16,"file_url":17,"file_type":18,"file_size":19,"view_count":4,"is_deleted":4,"is_public":20,"is_downloadable":20,"audit_status":20,"page_count":21,"language":22,"language_code":23,"site_id":24,"html_lang":23,"table_of_contents":25,"faqs":26,"seo_title":27,"seo_description":14,"update_tm":28,"read_time":29},207946,1374391974468,"Eden","https://ap-avatar.wpscdn.com/davatar_29158cc5080c5b710cf443261637dec0",4,"Exam","AQA GCSE Chemistry - Calculating Mass of Substances - The Mole","Revision notes for AQA GCSE Chemistry focused on calculating mass of substances using the mole concept. Explains that chemical amounts are measured in moles and that one mole contains a fixed number of particles, linked to the Avogadro constant. Covers how to relate moles to particle counts, ions, formula units, and molar mass for elements and compounds. Includes worked examples for determining numbers of particles and calculating mass from given moles, reinforcing the mole–mass relationship.","Head to www.savemyexams. com for more awesome resources  \n AQA GCSE Chemistry  \nCalculating Mass of Substances  \nContents  \n The Mole  \n Amounts of Substances in Equations  Using Moles to Balance Equations  Limiting Reactants  \n Concentrations of Solutions  \nPage 1 of 17  \n© 2015 − 2024 Save My Exams, Ltd. · Revision Notes, Topic Questions, Past Papers  \nYour notes  \nHead to www.savemyexams. com for more awesome resources  \nThe Mole  \nThe mole Higher tier only  \n Chemical amounts are measured in moles  \n The mole, symbol mol, is the SI unit of amount of substance  \n One mole of a substance contains the same number of the stated particles  \n This can be atoms, molecules or ions  \n One mole contains 6 .02 x 1023 particles; this number is known asthe Avogadro Constant  \n For example:  \n  One mole of sodium (Na) contains 6 . 02 x 1023 atoms of sodium  \n One mole of hydrogen (H2) contains 6 . 02 x 1023 molecules of hydrogen  \n One mole of sodium chloride (NaCl) contains 6 . 02 x 1023 formula units of sodium chloride  \n The mass of 1 mole of asubstance is known asthe molar mass  \n For an element, it isthe same asthe relative atomic mass written in grams  \n For a compound, it isthe same asthe relative molecular or formula mass in grams  \nPage 2 of 17  \n© 2015 − 2024 Save My Exams, Ltd. · Revision Notes, Topic Questions, Past Papers  \nYour notes  \nHead to www.savemyexams. com for more awesome resources  \n Worked example  \nFor magnesium chloride, MgCl2 , calculate the number of:􀂋 . Formula units in 1 mole  \n􀂌 . Atoms in 1 mole  \n􀂍 . Chloride ions in 1 mole  \n􀂎 . Magnesium ions in 2 moles Answers:  \n􀂋 . The formula unit is MgCl2 , so 1 mole of MgCl2 is:  \n 1 x 6 . 02 x 1023 = 6 . 02 x 1023 formula units  \n􀂌 . There are 3 atoms in MgCl2 , so 1 mole of MgCl2 contains:  \n 3 x 6 . 02 x 1023 = 18 . 06 x 1023 atoms  \n􀂍 . There are 2 chloride ions in MgCl2 , so 1 mole of MgCl2 contains:  \n 2 x 6 . 02 x 1023 = 12 . 04 x 1023 chloride ions  \n􀂎 . There is 1 magnesium ion in MgCl2 , so 2 mole of MgCl2 contains:  \n 2 x (1 x 6 . 02 x 1023) = 12 . 04 x 1023 magnesium ions  \n Examiner Tip  \nYou need to appreciate that the measurement of amounts in moles can apply to atoms, molecules, ions, electrons, formulae and equations. E. g. in one mole of carbon (C) the number of atoms is the same asthe number of molecules in one mole of carbon dioxide (CO2) .  \nThe mole and atomic mass  \n One mole of any element is equal to the relative atomic mass of that element in grams  \n This is called the molar mass  \n If you had 6 . 02 x 1023 atoms of carbon in your hand, that number of carbon atoms would have a mass of  \n12 g (because theAr of carbon is 12)  \n So one mole of helium atoms would have a mass of 4 g (Arof He is 4) , one mole of lithium would have amass of 7 g (Arof Li is 7) and so on  \n To |nd the mass of one mole of a compound, we add up the relative atomic masses  \n So one mole of water would have a mass of (2 x 1) + 16 = 18 g  \nPage 3 of 17  \n© 2015 − 2024 Save My Exams, Ltd. · Revision Notes, Topic Questions, Past Papers  \nYour notes  \nHead to www.savemyexams. com for more awesome resources  \n Worked example  \nWhat is the mass of 0 .250 moles of zinc?  \nAnswer:  \n From the Periodic Table, the relative atomic mass of Zn is 65  \n So, the molar mass is 65 g / mol  \n The mass is calculated by moles x molar mass:  \n 0.250 mol x 65 g / mol = 16 .25 g  \n Examiner Tip  \nRemember the key link between molesand mass: one mole of any element is equal to that elements atomic mass in grams.  \nPage 4 of 17  \n© 2015 − 2024 Save My Exams, Ltd. · Revision Notes, Topic Questions, Past Papers  \nYour notes  \nHead to www.savemyexams. com for more awesome resources  \nCalculating moles & masses Higher tier only  \n Although elements and chemicals react with each other in molar ratios, in the laboratory we use digital balances and grams to measure quantities of chemicals as it is impractical to try and measure out moles  \n Therefore, we have to be able to convert between molesan","cbCaiczbuFWL6CCi","https://ap.wps.com/l/cbCaiczbuFWL6CCi","pdf",811429,1,17,"English","en",105,"# The Mole\n## Chemical amounts and the mole\n## Avogadro constant and particle counts\n## Molar mass for elements and compounds\n# Calculating moles & masses\n## Converting between moles and grams\n## Worked examples using molar mass\n# Amounts of Substances in Equations\n## Using balanced equations for moles and masses","[{\"question\":\"What is the mole (mol) in GCSE Chemistry?\",\"answer\":\"The mole is the SI unit used to measure the amount of substance. One mole of a substance contains the same number of particles, such as atoms, molecules, ions, or formula units.\"},{\"question\":\"How do you calculate molar mass for an element or a compound?\",\"answer\":\"For an element, molar mass equals its relative atomic mass in grams. For a compound, molar mass equals its relative molecular or formula mass in grams, found by adding the relative atomic masses.\"},{\"question\":\"How do you convert between moles and mass?\",\"answer\":\"Use the relationship mass = moles × molar mass. First find the molar mass from the periodic table (or formula), then multiply by the given number of moles.\"}]","AQA GCSE Chemistry - Calculating Mass of Substances - The Mole | PDF",1788601888,43,{"code":4,"msg":31,"data":32},"ok",{"site_id":24,"language":23,"slug":33,"title":13,"keywords":34,"description":14,"schema_data":35,"social_meta":85,"head_meta":87,"extra_data":89,"updated_unix":28},"aqa-gcse-chemistry-calculating-mass-of-substances-the-mole","",{"@graph":36,"@context":84},[37,53,67],{"@type":38,"itemListElement":39},"BreadcrumbList",[40,44,48,51],{"item":41,"name":42,"@type":43,"position":20},"https://docshare.wps.com","Home","ListItem",{"item":45,"name":46,"@type":43,"position":47},"https://docshare.wps.com/document/","Document",2,{"item":49,"name":12,"@type":43,"position":50},"https://docshare.wps.com/document/exam/",3,{"item":52,"name":13,"@type":43,"position":11},"https://docshare.wps.com/document/aqa-gcse-chemistry-calculating-mass-of-substances-the-mole/207946/",{"url":52,"name":13,"@type":54,"author":55,"headline":13,"publisher":57,"fileFormat":60,"inLanguage":23,"description":14,"dateModified":61,"datePublished":61,"encodingFormat":60,"isAccessibleForFree":62,"interactionStatistic":63},"DigitalDocument",{"name":9,"@type":56},"Person",{"url":41,"name":58,"@type":59},"DocShare","Organization","application/pdf","2026-09-05",true,{"@type":64,"interactionType":65,"userInteractionCount":4},"InteractionCounter",{"@type":66},"ViewAction",{"@type":68,"mainEntity":69},"FAQPage",[70,76,80],{"name":71,"@type":72,"acceptedAnswer":73},"What is the mole (mol) in GCSE Chemistry?","Question",{"text":74,"@type":75},"The mole is the SI unit used to measure the amount of substance. One mole of a substance contains the same number of particles, such as atoms, molecules, ions, or formula units.","Answer",{"name":77,"@type":72,"acceptedAnswer":78},"How do you calculate molar mass for an element or a compound?",{"text":79,"@type":75},"For an element, molar mass equals its relative atomic mass in grams. For a compound, molar mass equals its relative molecular or formula mass in grams, found by adding the relative atomic masses.",{"name":81,"@type":72,"acceptedAnswer":82},"How do you convert between moles and mass?",{"text":83,"@type":75},"Use the relationship mass = moles × molar mass. 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