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- 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)+CuSO4(aq)→Cu(s)+FeSO4(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 350.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 142.mg. Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits.The reaction for producing glucose in plants, called photosynthesis, is 6CO2+6H2O−→−−lightC6H12O6+6O2 6CO2+6H2O→lightC6H12O6+6O2 If a plant produces 7.56 mol C6H12O6,7.56 mol C6H12O6, how many moles of CO2CO2 are needed?The reaction for producing glucose in plants, called photosynthesis, is 6CO2 +6H2O light−−→C6H12O6+6O2 If a plant produces 6.26 mol C6H12O6,how many moles of H2O are needed? moles H2O: mol mol
- 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) + CuSO4 (aq) → Cu (s) + FeSO4 (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 73.mg . Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits.It was invented in 1859 by French physician Gaston Plante and still retains application today, more than 150 years later. There are two reactions that take place during discharge of the lead-acid storage battery. In one step, sulfuric acid decomposes to form sulfur trioxide and water: H₂SO4(1) SO3(9) + H₂O(1) ΔΗ=+113. In another step, lead, lead(IV) oxide, and sulfur trioxide react to form lead(II) sulfate: Pb(s) + PbO2(s) + 2 SO3(g) → 2 PbSO4(s) ΔH = -775 kJ Calculate the net change in enthalpy for the formation of one mole of lead(II) sulfate from lead, lead(IV) oxide, and sulfuric acid from these reactions. Round your answer to the nearest kJ.Give Up? O Resources 9.4% re: Hint 8 > Consider these reactions, where M represents a generic metal. 2 M(s) + 6 HC1(aq) → 2 MCl,(aq) + 3 H, (g) 1. AĦ, = –783.0 kJ HCI(g) HCl(aq) → AH2 = –74.8 kJ H,(g) + Cl, (g) → 2 HCl(g) AH3 = –1845.0 kJ MCI, (s) → MCl, (aq) 4. AH -124.0 kJ Use the given information to determine the enthalpy of the reaction 2 M(s) + 3 Cl,(g) → 2 MCl, (s) S. AH kJ about us privacy policy terme of use contact.ua help en 2. 3.
- 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) + CuSO4 (aq) → Cu (s) + FeSO4 (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 300.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 67.mg . Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits.Sodium hydrogen carbonate (NaHCO3), also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid (HCI), which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl(aq) + NaHCO3(aq) → NaCl(aq) + H2O(l) + CO2(g) ->> The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 100. mL of a 0.089 M HCl solution. What mass of NaHCO3 would he need to ingest to neutralize this much HCI? Round your answer to 2 significant digits. x10 xClassify the following reaction: H2 (g) + 02(g) --> H2O (g) Synthesis or Combination Decomposition Single Displacement or Replacement Double Displacement or Replacement Combustion
- 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) + CuSO4 (aq) → Cu (s) + FeSO4 (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 500.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 76.mg . Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits. gLIn the reaction of magnesium metal with hydrochloric acid, how do you determine when the magnesium metal has reacted completely? Select all that apply. Mg (s) + 2 H* (aq) → Mg²+ (aq) + H2 (g) Select one or more: All of the water has evaporated. The dilute Hcl is gone. The magnesium metal is gone. Gas bubbles are no longer produced.NO+H2→ NH3+H2O balance the following equation and determine how many moles of ammonia are produced when 5.45 moles of hydrogen gas react with excess nitrogen monoxide