The melting point of bromine is $-7^{\circ}\text{C}$ and the boiling point is $59^{\circ}\text{C}$.\n\nExplain why bromine remains a solid at $-50^{\circ}\text{C}$.
Describe the arrangement and movement of bromine molecules at $-50^{\circ}\text{C}$.
A sample of liquid bromine has $2.408 \times 10^{25}$ molecules.\n\nOne mole of bromine liquid has $6.02 \times 10^{23}$ molecules.\n\nCalculate the mass of the sample of bromine liquid.
The ionic equation represents bromine reacting with warm concentrated aqueous sodium hydroxide.\n\n$3\text{Br}_2 + 6\text{OH}^- \rightarrow \text{BrO}_3^- + 5\text{Br}^- + 3\text{H}_2\text{O}$\n\nState the oxidation number of bromine in Br$_2$ and in Br$^-$.
Bromine is reduced in the reaction.\n\nExplain why, in terms of electrons.
Bromine reacts with hydrogen in a closed vessel to establish an equilibrium mixture. The forward reaction releases thermal energy to the surroundings.\n\n$\text{Br}_2(g) + \text{H}_2(g) \rightleftharpoons 2\text{HBr}(g)$\n\nThe temperature of the equilibrium mixture is increased while the pressure stays constant.\n\nState and explain what happens to the position of equilibrium.
The pressure of the equilibrium mixture is increased while the temperature stays constant.\n\nState and explain what happens to the position of equilibrium.
A phosphorus bromide contains 7.2% phosphorus by mass.\n\nCalculate the empirical formula of this bromide. Show your working.