Experiment 21. Write the equation for the decomposition of the hydrate, MgCl2 MgCl2*XH2O (s) −> MgCl2 (s) + XH2O (g) 2. Record the following masses: a. mass of crucible and hydrate (g) b. mass of the crucible and pure salt (g) The requested information can be found in the following table: Mass of the crucible and hydrate (g) 93,000 g Mass of the crucible and pure salt (g) 90,342 g3. Calculate the following: a. mass of water in hydrate sample (g) b. number of moles of water in the sample c. mass of pure salt in the sample (g) d. number of moles of salt in the sample. water/salt molar ratio in the sample The results of the requested calculations can be found in the following table: Mass of water in the hydrate sample (g) 2.658 g Number of moles of water in the sample .1475 mol Mass of salt pure in the sample (g) 2.342 gNumber of moles of salt in the sample 0.02460 molWater/salt molar ratio in the sample 6 moles of water for 1 mole of salt4. According to your calculations, what is the empirical formula for hydrated magnesium chloride? MgCl2*6H2O (s) −> MgCl2(s) + 6H2O(g)