Mass of crucible after the reaction - 76. Mass of crucible with lithium before reaction - 75.500 g Given the experimental data in the table below, what is the empirical formula of lithium nitride? The molar mass of lithium is 6.94 g/mol and that of nitrogen is 14.01 g/mol. Use this as a conversion factor to get 1.596g CuSO4 100 g CuSO4 5H2O 63.92g CuSO4 2. To avoid oxide formation, the reaction is performed under pure nitrogen gas. 159.61g mol1 (159.61 + 5 × 18.015)g mol1 × 100 63.92 CuSO4 This tells you that for every 100 g of copper (II) sulfate pentahydrate, you get 63.92 g of anhydrous copper (II) sulfate. Experiment 2: What was the identity of the precipitate that formed upon the addition of NaOH? Copper hydroxide Lithium is the only metal that reacts with nitrogen gas at room temperature to form lithium nitride. Given that argon is relatively inert, which of the following would you expect if you were to heat pure copper in the presence of argon gas? Copper oxide would not form and the mass would not change. 0.1001 moles Suppose you were to heat the copper in argon gas instead of atmospheric gases. For best accuracy, use the mass measured with the balance during the experiment. How many moles of copper (II) sulfate pentahydrate were used in the reaction? The molar mass of copper (II) sulfate pentahydrate is 249.68 g/mol. 25.000 g What happened when NaOH was added to the copper (II) sulfate pentahydrate solution? A blue precipitate formed. Choose the answer that is closest to yours. Experiment 2: What color was the copper (II) sulfate pentahydrate before heating? Blue How many grams of copper (II) sulfate pentahydrate were added to the beaker? Note: The amount of materials dispensed can vary.
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