Elemental phosphorus reacts with chlorine gas according to the equationP4(s)+6Cl2(g)→4PCl3(l)A reaction mixture initially contains 45.53 g P4 and 130.9 g Cl2. Once the reaction has reached completion, what mass (in g) of the excess reactant is left?         Express the mass in grams to three significant figures.

For the following reaction, 45.5 grams of iron(II) chloride are allowed to react with 110 grams of silver nitrate. iron (II) chloride (aq) + silver nitrate(aq) → iron(II) nitrate (aq) + silver chloride (s) What is the maximum amount of iron(II) nitrate that can be formed? Mass= What is the FORMULA for the limiting reactant? What amount of the excess reactant remains after the reaction is complete? g Mass=

10 KNO3 (s) + 8 C (s) +3 S (s) → 2 K2CO3 (s) + 3 K2SO4 (s) + 6 CO2 (g) + 5 N2 (g) What is the maximum mass of solid product that can be formed if 74.4 g of each reactant are allowed to react completely. Your answer should be in grams

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 200. mL sample of groundwater known to be contaminated with cadmium chloride, which would react with silver nitrate solution like this: CdCl₂(aq) + 2 AgNO3(aq) → 2 AgCl(s) + Cd(NO3)₂(aq) The chemist adds 75.0 mM silver nitrate solution to the sample until silver chloride stops forming. He then washes, dries, and weighs the precipitate. He finds he has collected 7.0 mg 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. mg L

Thermite is a metal powder mixture used frequently in pyrotechnics and metal construction work. It is composed of highly powderized aluminum and iron(III) oxide and when ignited by a high temperature source (such as burning magnesium ribbon), it reacts according to the following equation. Fe2O3(s) + 2 Al(s) → 2 Fe(l) + Al2O3(s) What mass of powderized Al is required to completely react with 35.3 g Fe2O3?

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) + 4 HCl(aq) → MnCl₂(aq) + 2 H₂O(1) + Cl₂(g) How much MnO₂ (s) should be added to excess HCl(aq) to obtain 395 mL Cl₂(g) at 25 °C and 805 Torr? mass of MnO₂: g

33.5 mL of a 0.117 M Na2CO3 solution completely react with a 0. 150 M HNO3 solution according to the following balanced chemical equation) Na₂CO3(aq) + 2 HNO3(aq) → 2 NaNO3(aq) + CO₂(g) + H₂O(1) What mass (in grams) of carbon dioxide is formed? Express your answer with the appropriate units. mass= 52.3 μÅ g Submit Previous Answers Request Answer

A mixture of barium chloride and sulfuric acid yield the precipitate barium sulfate and hydrochloric acid according to the double replacement reaction: H,SO, (aq) + BaCl, (aq) → Baso4 (s) + 2 HCI (aq) A large quantity of barium chloride is used to ensure that the sulfuric acid is the limiting reactant. If 39.5 grams of barium sulfate are produced, what mass of H2SO4 must be dissolved in the initial aqueous solution? g [Number in standard notation; round your answer to one decimal place] The following molar masses may or may not be needed, but are provided to save you time: • barium sulfate = 233 g/mol • sulfuric acid = 98.0 g/mol

When 32.6 g of Cu metal are reacted with excess AgNO3 (169.87 g/mol), what mass, in g, of Ag metal can theoretically be produced? Cu(s) + 2 AgNO3(aq) → 2 Ag(s) + Cu(NO3)2 Enter a numerical value for your answer; omit the units of g Ag. Your answer should have three significant figures.

Upon reaction of 1.27 g of copper sulfate with excess zinc metal, 0.494 g copper metal was obtained as an experimental result according to the equation: CUSO (aq) + Zn(s) → Cu(s) + ZNSO4(aq) Before the experiment was carried out the theoretical yield calculation was completed to predict the maximum amount of copper that could be isolated. The answer was 0.506 g of Cu. What is the percent yield in standard notation? [report your answer to the tenths place, i.e. one decimal place.]