Na2CO3(aq) + CaCl2⋅2H2O → CaCO3(s) + 2NaCl(aq) + 2H2O(aq)  A. how many moles of CaCl2•2H2O are present in 1.50 g of CaCl2•2H2O and then calculate how many moles of pure CaCl2 are present in the 1.50 g of CaCl2•2H2O. B. determine how many moles of Na2CO3 are necessary to reach stoichiometric quantities. From that calculation, determine how many grams of Na2CO3 are necessary to reach stoichiometric quantities

Commercial drain cleaners contain sodium hydroxide and aluminum. When water is added to this mixture, the heat that is generated will melt grease and the gas that is created will stir up the particles that are clogging the drain. If the process proceeds according to the following reaction: 2 Al (s) + 2 NaOH (aq) + 6 H2O (l) → 2 NaAl(OH)­4 (aq) + 3 H2 (g)   If you use 5.6 g of Al (s) and excess sodium hydroxide, how many liters of H2 (g) at 742 mm Hg and 22.0 ˚C are produced?

One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate.Suppose an EPA chemist tests a 250.mL sample of groundwater known to be contaminated with cadmium chloride, which would react with silver nitrate solution like this: CdCl2(aq)+2AgNO3(aq)→2AgCl(s)+CdNO32(aq).  The chemist adds 51.0mM silver nitrate solution to the sample until silver chloride stops forming. She then washes, dries, and weighs the precipitate. She finds she has collected 8.9mg of silver chloride. Calculate the concentration of cadmium chloride contaminant in the original groundwater sample. Be sure your answer has the correct number of significant digits.

In the reaction CrCl3 (aq) + 3 AgNO3 (aq) --> Cr(NO3)3 (aq) + 3 AgCI (s) 4.4 moles of CrClą are reacted with 1 moles of AgNO3. Determine the theoretical yield in mols of the product, silver chloride.

Using the balanced equation: FeCl3(aq) + 3 NaOH (aq) ------> FeOH3 (s) + 3 NaCl (aq), determine the mass of solid product that can be made by starting with 14.0 grams of iron (III) chloride and 9.0 grams of sodium hydroxide.

Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation   MnO2(s)+4HCl(aq)⟶MnCl2(aq)+2H2O(l)+Cl2(g) How much MnO2(s) should be added to excess HCl(aq) to obtain 285 mL Cl2(g) at 25 °C and 95 kPa?

Potassium permanganate reacts with oxalic acid (H2C2O4) in aqueous sulfuric acid according to the following reaction:   2 KMnO4(aq) + 5 H2C2O4(aq) + 3 H2SO4(aq) 2 MnSO4·H2O(s) + K2SO4(aq) + 10 CO2(g) + 6 H2O(l)   The reaction is run a second time and 8.74 g of MnSO4·H2O are obtained. What volume of carbon dioxide gas is collected at 1.01 bar and 23˚C? Answer in L with the correct number of significant figures; do not use scientific notation.

All information listed in question find the limiting reagents in grams.

An excess volume of 0.10 M BaCl2(aq) is mixed with 1.0 L of Na2SO4(aq) and forms 2.33 g of precipitate. What is the net ionic equation for the reaction?   Ba2+(aq) + SO42–(aq) → BaSO4(s)   2 Na+(aq) 2 Cl–(aq)  →      2 NaCl(s)   2 Na+(aq) 2 Cl–(aq) + Ba2+(aq) +  SO42–(aq) → 2 NaCl(s) + BaSO4(s) What is the minimum volume of BaCl2(aq) added to yield the precipitate?   0.001 L   0.01 L   0.10 L

Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation   MnO2(s)+4HCl(aq)⟶MnCl2(aq)+2H2O(l)+Cl2(g) How much MnO2(s) should be added to excess HCl(aq) to obtain 225 mL Cl2(g) at 25 °C and 755 Torr?