713641
| Question | Answer |
| RAM of an isotope | mass of each isotope by its relative abundance added together / relative abundance |
| RFM | RAMs of each atom in molecule added together |
| Empirical formula | List elements, write experimental masses, divide by atomic no., even out |
| molecular formula | find mass of empirical formula, relative molecular mass/ans, empirical formula x empirical unit |
| Masses in a reaction | balanced equation, find RFM of required parts in equation, divide to get one then multiply to get all |
| percentage yield | (actual yield/theoretical yield) x 100 |
| number of moles | mass in g / RAM (or RFM) |
| volume | (mass/RAM) x 24 = dm3 (mass/RAM) x 24000 = cm3 |
| concentration | no. of moles / volume |
| electrolysis | no. of moles = charge / charge of ion x faraday constant (which is 96000) |
| acid + metal | salt + hydrogen |
| metal + water | metal hydroxide + hydrogen |
| less reactive metal + steam | metal oxide + hydrogen |
| iron + oxygen + water (Rusting) | hydrated iron (III) oxide (rust) |
| Production of O2 | 2H2O2 (aq) ---> 2H2O (l) + O2 (g) |
| Alkanes | CnH2n+2 |
| Complete Combustion alkane + oxygen | carbon dioxide + water |
| Incomplete Combustion alkane + oxygen | carbon + carbon monoxide + carbon dioxide + water |
| Alkenes | CnH2n |
| acid + base | salt + water |
| acid + metal oxide | salt + water |
| acid + metal carbonate | salt + water + carbon dioxide |
| acid + insoluble base (making soluble salts) | salt + carbon dioxide + water |
| titration | no. of moles of known substance, according to equation work out no. of mole of unknown substance, work out its concentration |
| rate of reaction | amount of reactant used or amount of product formed / time |
| enthalpy change | total energy absorbed to break bonds - total energy released in making bonds |
| the Haber Process | N2 (g) + 3H2 (g) <-----> 2NH3 (g) (+ heat) |
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