A 25.1 g25.1 g sample of magnesium reacts with excess silver nitrate to produce silver metal and magnesium nitrate. The reaction is stopped before all of the magnesium metal has reacted. A total of 61.3 g61.3 g of solid metal is present. Calculate the mass of each metal in the 61.3 g61.3 g mixture.

You have been asked to produce 40.0 g of barium carbonate. You have been given two solutions you can use in this reaction: a 0.160 mol/L solution of potassium carbonate, and a 0.260 mol/L solution of barium nitrate. It is known the reaction between these two compounds has a 72.0% yield of barium carbonate. What is the minimum volume of each solution should you use in this reaction?

You are given 500 mL of a 0.50 M solution of MgCl₂. What is the theoretical yield (g) of Mg metal we could extract from the solution? a. 28g b. 24.3g c. 6.1g d 97.2 g e. 12.2 g Next F

Classify each chemical reaction.

Aqueous solutions barium chloride and potassium sulfate are combined.  1) Predict the products and write the balanced equation showing the states of each substance. 2) The barium chloride solution has a volume of 100.0 mL and contains 10.00 grams of barium chloride.  The molarity of the potassium sulfate solution is 0.574 moles/liter and has a volume of 100.0 mL. Determine the limiting reactant and the mass of each product in grams. 3) Determine how many grams of excess reactant remain. 4) Calculate the molarity of just the potassium ions after the reaction has finished.

56.0 g of sodium sulfate is dissolved in water to make 425 mL of solution. Calculate the molarity of the solution. Express your answer in decimal notation.

In an experiment, a student combines 75.0 mL of a 0.200 M iron (III) chloride solution with 125.0 mL of a 0.250 M sodium carbonate solution. Write a balanced equation for the reaction. What is the limiting reactant? What is the theoretical yield of sodium chloride (in grams)? How many grams of sodium chloride need to be produced in the experiment in order to achieve a yield of 93.75%?

250. mL of water is added to 150. mL of a 2.32 M aqueous solution of glucose. The solution is then heated such that 50.0 mL of water is evaporated. What is the concentration of glucose in the final solution in units of M?

Consider the reaction of solid aluminum iodide and potassium metal to form solid potassium iodide and aluminum metal. Write the balanced chemical equation for the reaction.

A mixture contains Mg(NO3)2 and KBr. A 1.85 g sample of this mixture is dissolved in water and an excess of NaOH is added, producing a precipitate of Mg(OH)2. The precipitate is filtered, dried, and weighed. The mass of the precipitate is 0.365 g. What is the mass percent of Mg(NO3)2 in the original mixture?