This question is about the industrial extraction of calcium metal and bromine gas through the electrolysis of molten calcium bromide (CaBr2\text{CaBr}_2CaBr2).
Calcium is deposited at the negative electrode. Describe what happens to calcium ions (Ca2+\text{Ca}^{2+}Ca2+) during this process in terms of electrons.
Write a balanced half-equation to represent the formation of bromine molecules (Br2\text{Br}_2Br2) at the positive electrode from bromide ions (Br−\text{Br}^-Br−).
The overall chemical equation representing this electrolysis process is: CaBr2→Ca+Br2\text{CaBr}_2 \rightarrow \text{Ca} + \text{Br}_2CaBr2→Ca+Br2 Determine the mass, in kg\text{kg}kg, of bromine gas generated when 500 kg500\text{ kg}500 kg of molten calcium bromide is completely decomposed.
Relative atomic masses (ArA_rAr): Ca=40\text{Ca} = 40Ca=40; Br=80\text{Br} = 80Br=80