Fe2O3 (s) + 3CO(g)→2Fe(s) + 3CO2(g) In a reaction mixture containing 181 g Fe2O3 and 65.4 g CO, CO is the limiting reactant. Part A Calculate the mass of the reactant in excess (which is Fe2O3) that remains after the reaction has gone to completion. Express the mass with the appropriate units. μÅ Value Units ?

Which of the following chemical reactions will produce a precipitate?

A 0.9 g sample of a mixture of KCl and MgCl2 is treated with excess AgNO3(aq). If 2.37 grams of AgCl(s) are obtained, then what is the percentage by mass of KCl in the original mixture? Your answer must be accurate to two significant digits. Keep several extra digits in your calculations and round off only at the end. Do not include the percent sign (%) as part of your answer.   Molar masses (in g mol−1): KCl, 74.55 MgCl2, 95.21 AgCl, 143.35

The useful metal manganese can be extracted from the mineral rhodochrosite by a two-step process. In the first step, manganese(II) carbonate and oxygen react to form manganese(IV) oxide and carbon dioxide: 2MnCO3(s) + O₂(g) → In the second step, manganese (IV) oxide and aluminum react to form manganese and aluminum oxidide: 3 MnO₂ (s) + 4A1(s) 3 Mn (s) + 2 Al₂O3(s) Check 2 MnO₂ (s) + 2 CO₂ (g) Suppose the yield of the first step is 88.% and the yield of the second step is 70.%. Calculate the mass of manganese(II) carbonate required to make 1.0 kg of manganese. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits. 0 0 x10 nin 0 0.0 S Save For Later E OL A S C Submit Assignmen

A sodium sulfate solution is added to a 25.0 mL sample of a solution containing Ba2+ ions until no more precipitate formed.  The precipitate (BaSO4) is collected, dried, and weighed.  If 1.59 g of the precipitate are obtained, what is the concentration (in M) of Ba2+ ions in the 25.0 mL sample? Your answer should have 3 sig. figs. Molar Masses:  (Na2SO4: 142.05 g/mol)  (Ba2+: 137.3 g/mol) (BaSO4: 233.37 g/mol)

Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese(IV) oxide. 4 HCl(aq) + MnO,(s) → MnCl, (aq) + 2 H,O(1) + Cl, (g) > A sample of 34.9 g MnO, is added to a solution containing 43.1 g HCI. What is the limiting reactant? HCl O MnO2 What is the theoretical yield of Cl, ?

For each of the reactions, calculate the mass (in grams) of the product formed when 15.67 g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant. 2K(s)+Cl2(g)−−−−−→2KCl(s) 2K(s)+Br2(l)−−−−−→2KBr(s) 4Cr(s)+3O2(g)−−−−−→2Cr2O3(s) 2Sr(s)−−−−+O2(g)→2SrO(s)

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.

Determine the mass (in g) of AgBr that is produced when 609 mL of a 5.76×10-2 M Na3Ag(S2O3)2 solution completely reacts with 674 mL of a 1.15×10-2 M NaBr solution according to the following balanced chemical equation.Na3Ag(S2O3)2(aq) + NaBr(aq) → AgBr(s) + 2Na2S2O3(aq)