Chemistry Equations / Maths

Georgia B
Flashcards by , created over 5 years ago

GCSE Chemistry Flashcards on Chemistry Equations / Maths , created by Georgia B on 04/03/2014.

Georgia B
Created by Georgia B over 5 years ago
Chemistry Session 1
Diane MAK
Chemistry ATP Quiz
A-Level Physics: Course Overview
Religious Studies - Keywords.
IGCSE Chemistry Revision
organic chemistry
Chemistry General Quiz
Chemistry ATP
Cation, Anion & Flame Tests
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)