The ultimate A level chemistry resource
Electrolysis is a non-spontaneous chemical process powered by electrical energy. The reactions happening at the electrodes in the electrolysis of
Continue readingExplaining the electrolysis of molten ionic salts
In the reaction between peroxodisulphate ions and iodide ions, the iodide ions are oxidised to iodine whilst the peroxodisulphate ions
Much of the chemistry of transition metal ions is a consequence of the fact that the 3d and 4s orbitals
Continue readingExplaining the redox behaviour of transition metals
Group 7 consists of the elements fluorine, chorine, bromine, iodine and astatine, and they are known as the halogens. All
Continue readingExplaining the chemistry of the Group 7, the halogens
Electrolysis uses electricity (energy) to drive a non-spontaneous reaction which is useful for recharging batteries, splitting water to make hydrogen
Fuel cells commonly use the reaction between hydrogen and oxygen to produce a voltage, with water being the only waste
Modern storage cells (batteries) can be divided into the non-rechargeable kind (primary cells) and the rechargeable kind (secondary cells). Primary
The rusting of iron can be summarised by the equation 4 Fe(s) + 3 O2(g) + H2O(l) ⇾ 2 Fe2O3•xH2O(s)
A redox reaction consists of two half reactions – an oxidation and a reduction reaction. If we take a pair
Continue readingPredicting the feasibility of redox reactions using standard electrode potentials
We can link any two half cells together to form an electrochemical cell. A high resistance voltmeter prevents current (electrons)
Continue readingDetermining the potential difference of an electrochemical cell