1.1.2 MOLES & EQUATIONS 0.0 / 5 ? ChemistryATOMSASOCR Created by: upsidedown1004Created on: 16-05-16 11:52 What is relative isotopic mass? the mass of an isotope compared to 1/12 of the mass of an atom of C12 1 of 19 What is an isotope? atoms of an element with the same number of protons and electrons but a different number of neutrons 2 of 19 What is relative molecular mass? the weighted meanness of a molecule compared to 1/12 of an atom of C12 3 of 19 What is relative formula mass? the weighted mean mass of a formula unit compared with 1/12 of the mass of an atom of C12 4 of 19 What is the amount of a substance? mass of a substance that has the same number of particles as 12g of C12 5 of 19 What is Avogadro's constant? number of particles present is one mole of carbon 6 of 19 What is the value of Avogadro's constant? 6.02x10^23 7 of 19 How would you calculate the number of particles present? avogadro's constant x moles 8 of 19 What is molar mass? the mass of 1mol of a substance 9 of 19 What are the units of molar mass? g mol^-1 10 of 19 What is relative atomic mass? Weighted mean mass of an atom compared to 1/12 of the mass of an atom of C12 11 of 19 How would would you calculate the relative atomic mass of a substance when given the percentages of it's isotopes? ((% x mass) + (% x mass)) / 100 12 of 19 What is an empirical formula? simplest whole number ratio of atoms of each element present in a compound 13 of 19 How do you calculate the empirical formula? find n of moles // divide by smallest // create whole number 14 of 19 What is a molecular formula? the actual number of each element present in a molecule 15 of 19 where is the mass of an atom concentrated? in its nucleus 16 of 19 What is the mass of an electron? 1/2000 17 of 19 How do you calculate % yield? actual yield / theoretical yield x 100 18 of 19 When using volume, why is 24 used? 1mol of gas occupies 24dm^3 of mass at RTP 19 of 19
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