i. Calculate the relative molecular mass of anhydrous aluminium chloride vapour at each temperature. R=8.31J/K. ii. What is the probable molecular formula of aluminium chloride vapour at 200^circ c and

To calculate the relative molecular mass of anhydrous aluminium chloride vapor at a given temperature, we can use the ideal gas equation in the form of the molar mass equation:<br /><br />\[ M = \frac{dRT}{P} \]<br /><br />where:<br />- \( M \) is the molar mass,<br />- \( d \) is the density of the gas,<br />- \( R \) is the universal gas constant (\(8.31 \, \text{J/mol K}\)),<br />- \( T \) is the temperature in Kelvin,<br />- \( P \) is the pressure.<br /><br />However, since the problem does not provide specific values for density or pressure, let's assume that you have these values from an experiment or another source to proceed with calculations.<br /><br />For the probable molecular formula of aluminum chloride vapor at \(200^\circ C\):<br /><br />Aluminum chloride (AlCl₃) can exist as a dimer (Al₂Cl₆) in the vapor phase at certain temperatures. At higher temperatures, it tends to dissociate into monomers (AlCl₃).<br /><br />1. Convert the temperature from Celsius to Kelvin:<br /> \[ 200^\circ C = 200 + 273.15 = 473.15 \, \text{K} \]<br /><br />2. If experimental data shows that the calculated molar mass is approximately 267 g/mol, this suggests the presence of the dimer Al₂Cl₆ because:<br /> - The molar mass of AlCl₃ is approximately 133.5 g/mol.<br /> - The molar mass of Al₂Cl₆ is approximately 267 g/mol.<br /><br />Therefore, at \(200^\circ C\), the probable molecular formula of aluminum chloride vapor is Al₂Cl₆.