Determine the empirical formula of the oxide of magnesium. (Think carefully about the precision of each mass that you measured before you do this calculation. How many significant figures are justifled for each mass?) (3 Points) Write correctly balanced chemical equations for the following reactions: (4 points) a. Magnesium with molecular oxygen 2 M9102 2 Ngo b. Magnesium with molecular nitrogen c. Magnesium nitride with water Mga N₂ + 6H₂O →3 Mg(OH)₂ + 2NH3 d. Heating magnesium hydroxide Mg(OH)₂ →→ MgO + H₂O When 0.422 g of phosphorus is burned, 0.967 g of a white oxide is obtained. (3 Points) a. Determine the empirical formula of the oxide b. Write a balanced equation for the reaction of phosphorus and molecular oxygen on the f this empirical formula./n

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