actual yield of magnesium nitrate formed from 145.7 g145.7 g of magnesium and excess copper(II) nitrate

1. Label each of the following reactions as combination (synthesis), decomposition, single replacement, or double replacement. Then complete and balance the following reactions. Reaction Type of reaction? Redox or nonredox? H2(g) + 02 (g) → K (s) + N2 (g) → C (s) + 02 (g) → H2CO3 (aq) → electrical current H₂O (1) 300°C Au2O3 (s) 300°C Ag2O (s) → NH3 (g) → Pb (s) + Cu(NO3)2 (aq) → Na (s) + HOH (1) -> BaBr2 (aq) + Na3PO4 (aq) → H2SO4 (aq) + NH4OH(aq) → Cl2 (g) + NaI (aq) → Na2S (s) + HCl(aq) → Fe (s) + 02 (g) →

Because of the toxicity of mercury compounds, mercury(I) chloride is used in antibacterial salves. The mercury(I) ion Hg22+ consists of two bound Hg+ ions.How many grams of mercury(I) chloride are needed to saturate 4900 km3 of water (the volume of Lake Michigan)? (Ksp = 1.5 × 10−18) .

Write a balanced chemical equation based on the following description: solid sodium reacts with chlorine gas to produce solid sodium chloride. Na(s)+Cl2(g)_

Octane has a density of 0.703g/ml. Calculate the mass of CO2 produced by burning one gallon of octane. There are 3.79 liters to one gallon.

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 iron(III) chloride, which would react with silver nitrate solution like this: FeCl,(aq) + 3 AgNO,(aq) 3 AgCl(s) + Fe(NO₂),(ag) The chemist adds 21.0 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 3.3 mg of silver chloride. Calculate the concentration of iron(III) chloride contaminant in the original groundwater sample. Be sure your answer has the correct number of significant digits. e -12 D.P C P

Classifying Reactions and Balancing Chemical Equations Part A: For each of the chemical reactions that are listed below, balance the chemical equation and then state the type of chemical reaction. 1. - Cu (s) + O₂(g) → CuO (s) Reaction type: 2.H₂O ()→→O₂ (g) + H₂ (B) Reaction type: 3. Fe (s) + H₂O () Fe₂O3 (s) + H₂(g) Reaction type: 5. 4.H₂S (aq) + AsCl3 (aq) →→As2S3 (s) + HCl(aq) Reaction type: CaCO3 (s) → CO₂(g) + Reaction type: 6. C4H10O (g) + O₂(g) →→CO₂(g) + H₂O (c) Reaction type: 7. S8 (s) + Fe (s)→ FeS (s) Reaction type: CaO (s) 8. H₂SO4 (aq) +Al (s) →→Al2(SO4)3 (aq) + H₂(g) Reaction type: 9. H3PO4 (aq) + NH,OH (aq) Reaction type: (NH4)3PO4 (aq) + stei HOH (c) 2017-

One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe(s) + CuSO (aq) → Cu(s) + FESO,(aq) Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 200. mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 64. mg. Ar Calculate the original concentration of copper(II) sulfate in the sample. Round your answer to 2 significant digits. 10

Which of the following correctly expressed the balanced equation for the following word equation:

When the following molecular equation is balanced using the smallest possible integer coefficients, the values of these coefficients are: O₂ (g) Fe₂03 (s) | Fe (s) +