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- 1) A sample of blue crystals of copper (II) sulfate pentahydrate was heated to produce the copper(Il)sulfate tetrahydrate. (a) Write the chemical formulas of the copper(II)sulfate pentahydrate and copper(II)sulfate tetrahydrate. (b) Calculate mass percent of water in copper(II)sulfate pentahydrate (c) If 7.491 g of the copper (II) sulfate pentahydrate produces 6.951 g of the copper (II) sulfate tetrahydrate, how many grams of anhydrous copper(I1)sulfate could be obtained? (Cu=63.5 g/mol, S=32.0 g/mol, O=16.0 g/mol, H=1 g/mol)Write the correct net ionic equation for the reaction of lithium carbonate with calcium chloride, which produces the white precipitate pictured below.Write balanced chemical equations for the following reactions. The decomposition of solid ammonium nitrate to produce gaseous dinitrogen oxide and water. The reaction of aqueous sodium phosphate and aqueous copper(II) sulfate to produce solid copper(II) phosphate and aqueous sodium sulfate.
- Copper (II) iodide + silver nitrate --> copper (II) nitrate + silver iodide formulapalladium(III) iodide Express your answer as a chemical formula.A student is given a 1.3002 g of an unknown copper compound. Following isolation by displacement by Mg, 0.4617 g of Cu metal is recovered. What is the percentage of Cu in the sample? You may assume that one mole of the sample contains one mole of copper.