Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese(IV) oxide. 4HCl(aq)+MnO2(s)⟶MnCl2(aq)+2H2O(l)+Cl2(g) A sample of 36.7 g MnO2 is added to a solution containing 43.7 g HCl. What is the limiting reactant? HCl MnO2 What is the theoretical yield of Cl2? theoretical yield:_____g Cl2g If the yield of the reaction is 74.9%, what is the actual yield of chlorine? actual yield:_____g Cl2

What mass of precipitate (in g) is formed when 45.5 mL of 0.300 M Li₃PO₄ reacts with 50.5 mL of 0.200 M CrCl₃ in the following chemical reaction? Li₃PO₄(aq) + CrCr₃(aq) → CrPO₄(s) + 3 LiCl(aq)

What mass of precipitate (in g) is formed when 45.5 mL of 0.300 M Li₃PO₄ reacts with 56.0 mL of 0.200 M CrCl₃ in the following chemical reaction? Li₃PO₄(aq) + CrCr₃(aq) → CrPO₄(s) + 3 LiCl(aq)

What mass of precipitate (in g) is formed when 45.5 mL of 0.300 M K₃PO₄ reacts with 54.5 mL of 0.200 M CrCl₃ in the following chemical reaction? K₃PO₄(aq) + CrCl₃(aq) → CrPO₄(s) + 3 KCl₃(aq)

1. A student was asked to react silver nitrate with sodium during a stoichiometry lab. The student react 12.3 g of silver nitrate with 7.83 g of sodium sulfate to produce the following products.  Na2SO4(aq) + 2 AgNO3 (aq) -> Ag2SO4(s) + 2 NaNO3(aq) a) predict the mass of percipitate that the student should obtain.

What mass of precipitate (in g) is formed when 45.5 mL of 0.300 M Li₃PO₄ reacts with 41.5 mL of 0.200 M Cr(NO₃)₃ in the following chemical reaction? Li₃PO₄(aq) + Cr(NO₃)₃(aq) → CrPO₄(s) + 3 LiNO₃(aq)

In the experiment, a student is given 2.94 g of a mixture containing anhydrous MgCl2 and KNO3. To determine the percentage by mass of MgCl2 in the mixture, the student uses excess AgNO3(aq) to precipitate the chloride ion as AgCl(s).    Starting with the 2.94 g sample of the mixture dissolved in water, briefly describe the steps necessary to quantitatively determine the mass of the AgCl precipitate.  The student determines the mass of the AgCl precipitate to be 5.48 g. On the basis of this information, calculate each of the following.(i) The number of moles of MgCl2 in the original mixture  (ii) The percent by mass of MgCl2 in the original mixture

What mass of precipitate (in g) is formed when 69.0 mL of 0.500 M FeCl3 reacts with excess AgNO3 in the following chemical reaction? FeCl3(aq)+ 3 AgNO3(ag) ———> 3 AgCl(s) + Fe(NO3)3(aq)

Fumaric acid is  quite common in the plant world and is added to many foods due to its acidity and fruity flavor.  It has a molar mass of 116.07 g/mol and a formula of C4H4O4. A solution of sodium hydroxide is used to determine the molarity of a fumaric acid acid solution before it is used to prepare some sour gummi worms.     C4H4O4(aq)   + 2NaOH(aq) --> Na2C4H2O4(aq) +2 H2O(l)   Calculate the Molarity of the fumaric acid if 32.08 mL of 0.09973 M NaOH was used to neutralized 75.00 mL of fumaric acid solution.  Assume the fumaric acid is acting as a strong electrolyte acid in this reaction. (It is a weak acid, but a very strong weak electrolyte)     Fumaric acid is  quite common in the plant world and is added to many foods due to its acidity and fruity flavor.  It has a molar mass of 116.07 g/mol and a formula of C4H4O4. A solution of sodium hydroxide is used to determine the molarity of a fumaric acid acid solution before it is used to prepare some sour gummi worms.…