Suppose a 250. mL flask is filled with 1.3 mol of SO, and 1.6 mol of SO3. This reaction becomes possible: 250,(3) +0,(g) = 2so,(3) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of 0,. You can leave out the M symbol for molarity. so, 0, so, initial change equilibrium

Suppose a 250. mL flask is filled with 1.3 mol of SO, and 1.6 mol of SO3. This reaction becomes possible: 250,(3) +0,(g) = 2so,(3) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of 0,. You can leave out the M symbol for molarity. so, 0, so, initial change equilibrium

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Phosphoric acid, a mild acid used among other things as a rust inhibitor, food additive, and etching agent for cavity repair by dentists, can be made from elemental phosphorus in a two step process. In the first step, phosphorus and oxygen react to form diphosphorus pentoxide: →+P4s 5O2g 2P2O5g In the second step, diphosphorus pentoxide and water react to form phosphoric acid H3PO4 : →+P2O5g 3H2Ol 2H3PO4l Suppose the yield of the first step is 66.% and the yield of the second step is 62.% . Calculate the mass of phosphorus required to make 2.0kg of phosphoric acid. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.
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.
Complete the table below by deciding whether a precipitate forms when aqueous solutions A and B are mixed. If a precipitate will form, enter its empirical formula in the last column. Does a empirical formula of precipitate precipitate form solution A solution B when A and B are mixed? potassium sulfide ironc1) nitrate Oves O ne ammonium trate potassium acetate O yes O no cadmium ntrate manganese) odide O yes O no
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 NaHCO, neutralizes excess HCI through this reaction: HCl(aq) + NaHCO3(aq) NaCl(aq) + H₂O(1) + 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 200 ml of a 0.050 M HCI solution. What mass of NaHCO, would he need to ingest to neutralize this much HCI? Be sure your answer has the correct number of significant digits. X
A tiny sample of an aqueous solution of two substances R and P is sketched below, as if it was under an imaginary microscope so powerful that individual molecules could be seen. (The water molecules are not shown.) 8 R and P can interconvert. That is, R can turn into P, and P can turn back into R: 113 5 R (aq)=P(aq) R P number of R molecules: number of P molecules: K= The equilibrium constant K for this equilibrium is interconversion reaches equilibrium. $3/1₁ Predict the number of R and P molecules in this sample when the . X
A solution is prepared by dissolving 2.95 g Co2(SO4)3 in enough water to make 1.00 L of red solution; the red color is due to the presence of the cobalt ions. To this solution was added 1.52 g of magnesium powder. A redox reaction occurred, in which the magnesium atoms lose all of their valence electrons and the red color of the solution fades. (a) Write the total reaction that occurs and the net ionic equation for the redox process. (Assume that one of the products of the redox reaction is a metal.) (b) Calculate the initial concentration of cobalt ions, the final concentration of cobalt ions, and the final concentration of magnesium ions.
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.
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
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 x
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. gL
Suppose a 250. mL flask is filled with 1.0 mol of CO, 0.70 mol of H₂O and 2.0 mol of H₂. This reaction becomes possible: CO(g) + H₂O(g) CO₂(g) + H₂(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of CO₂. You can leave out the M symbol for molarity. initial change equilibrium 2 со 0 H₂O CO₂ X H₂ 0 X 5