CHM - Exam 2 Review 1. Silver is often extracted from ores...

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Exam 2 Review 1. Silver is often extracted from ores as KAg(CN) 2 and then recovered by the following reaction. What mass of zinc, in grams is required to produce 1 oz (28.35 g) of silver? (Atomic weights: K = 39.10; Ag = 107.87; C = 12.01; N = 14.01; Zn = 65.38). KAg(CN) 2 (aq) + Zn(s) Ag(s) + Zn(CN) 2 (aq) + KCN(aq) 2. Aluminum and sulfur react at elevated temperatures to form aluminum sulfide, Al 2 S 3 . Calculate the mass of aluminum that reacts with 1.00 g of sulfur. (Atomic weights: Al = 26.98; S = 32.06). 3. Write the net ionic equation: Ni(NO 3 ) 2 (aq) + NaOH(aq) 4. Write the net ionic equation: Mg(NO 3 ) 2 (aq)+ Na 2 CrO 4 (aq) NaNO 3 ( ) + MgCrO 4 ( ) 5. Calculate the molarity of a solution of 0.2396 g of RbSO 4 in 15 mL of solution. (Atomic weights: Rb = 85.47, S = 32.06, O = 16.00). 6. Calculate the molarity of a solution of 91 g of MgCl 2 in 2.0 L of solution. (Atomic weights: Mg = 24.30, Cl = 35.45). 7. Determine the mass (g) of solute required to form 275 mL of a 0.4230 M KClO
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CHM - Exam 2 Review 1. Silver is often extracted from ores...

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