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All Textbook Solutions for Chemistry: Matter and Change

75A 76A 77A 78A 79A 80A 81A 82A 83A 84A 85A 86A 87A 88A 89A 90A Lead(ll) oxide is obtained by roasting galena, lead(ll) sulfide, in air. The unbalanced equation is: PbS(s)+O2(g)PbO(s)+SO2(g) ) a. Balance the equation, and determine the theoretical yield of PbO if 200.0 g of PbS is heated. b. What is the percent yield if 170.0 g of PbO is obtained?92A 93A 94A 95A 96A 97A Ammonium sulfide reacts With copper(ll) nitrate in a double replacement reaction. What mole ratio would you use to determine the moles of NH4NO3 produced if the moles of CuS are known?Fertilizer The compound calcium cyanamide (CaNCN) is used as a nitrogen source for crops. To obtain this compound, calcium carbide is reacted with nitrogen at high temperatures. CaC2(s)+N2(g)CaNCN(s)+C(s) What mass of CaNCN can be produced if 7.50 mol of CaC2 reacts With 5.00 molOf N2 ?When copper(ll) oxide is heated in the presence Of hydrogen gas, elemental copper and water are produced. What mass of copper can be obtained if 32.0 g of copper(ll) oxide is used?Air Pollution Nitrogen monoxide, which is present in urban air pollution, immediately Converts to nitrogen dioxide as it reacts with oxygen. a. Write the balanced chemical equation for the formation of nitrogen dioxide from nitrogen monoxide. b. What mole ratio would you use to convert from moles of nitrogen monoxide to moles of nitrogen dioxide?Electrolysis Determine the theoretical and percent yield of hydrogen gas if 36.0 g ofwater undergoes electrolysis to produce hydrogen and oxygen and 3.80 g of hydrogen is collected.Iron reacts with oxygen as Shown. 4Fe(s)+3O2(g)2FeO3(s) Different amounts of iron were burned in a fixed amount of oxygen. For each mass of iron burned, the mass Of iron(lll) oxide formed was plotted on the graph shown Figure 11.15. Why does the graph level off after 25.0 g of iron is burned? How many moles of oxygen are present in the fixed amount?Analyze and Conclude In an experiment, you obtain a percent yield of product of 108%. Is such a percent Yield possible? Explain. Assuming that your calculation is correct, what reasons might explain such a result?Observe and Infer Determine whether each reaction depends on a limiting reactant. Explain why or why not, and identify the limiting reactant. a. Potassium chlorate decomposes to form potassium chloride and oxygen. b. Silver nitrate and hydrochloric acid react to produce silver chloride and nitric acid.Design an Experiment Design an experiment that can be used to determine the percent yield of anhydrous copper(ll) sulfate When copper(ll) sulfate pentahydrate is heated to remove water.Apply When a campfire begins to die down and smolder, you can rekindle the flame by fanning the fire. Explain, in terms of stoichiometry, why the fire again begins 10 flare up when fanned.Apply Students conducted a lab to investigate limiting and excess reactants. The students added different volumes of sodium phosphate solution (Na3PO4) to a beaker. They then added a constant volume of cobalt(ll) nitrate solution (CO(NO3)2) stirred the contents, and allowed the beakers to sit overnight. The next day, each beaker had a purple precipitate at the bottom. The students decanted the supernatant from each beaker, divided it into two samples, and added one drop Of sodium phosphate solution to one sample and one drop of cobalt(ll) nitrate solution to the second sample. Their results are shown in Table 11.5. a. Write a balanced chemical equation for the reaction. b. Based on the results, identify the limiting reactant and the excess reactant for each trial.When 9.59 g of a certain vanadium oxide is heated in the presence of hydrogen, and a new oxide of vanadium are formed. This new vanadium oxide has a mass of 8.76 g. When the second vanadium oxide undergoes additional heating in the presence Of hydrogen, 5.38 g of vanadium metal forms, a. Determine the empirical formulas for the two vanadium oxides. b. Write balanced equations for the Steps of the reaction. c. Determine the mass of hydrogen needed to complete the steps of this reaction.110A 111A 112A 113A 114A 115A 116A 117A 118A 119A 120A 1STP 2STP 3STP 4STP 5STP 6STP 7STP 8STP 9STP 10STP 11STP 12STP 13STP 14STP 15STP 16STP 17STP 1PP 2PP 3PP 4PP 5SSC 6SSC 7SSC 8SSC 9SSC 10SSC 11PP 12PP 13PP 14PP 15PP 16PP 17SSC 18SSC 19SSC 20SSC 21SSC 22SSC 23PP 24PP 25SSC 26SSC 27SSC 28PP 29PP 30PP 31SSC 32SSC 33SSC 34SSC 35SSC 34A 35A 36A 37A 38A 39A 40A Baking Explain why the baking instructions on a boxof cake mix are different for high and low elevations.Would you expect to have a longer or a shorter cookingtime at a high elevation?42A 43A 44A 45A 46A 47A 48A 49A 50A 51A 52A 53A 54A 55A 56A 57A 58A 59A 60A 61A 62A 63A 64A 65A 66A 67A 68A 69A 70A 71A 72A 73A 74A 75A 76A 77A 78A 79A 80A 81A 82A 83A 84A 85A 86A 87A 88A 89A 90A 91A 92A 93A 94A 95A 96A 97A 98A 99A 100A 101A 102A 103A 104A 105A 106A 108A 109A 110A 111A 112A 113A What is the ratio of diffusion rates for nitric oxide(NO) and nitrogen tetroxide (N2O4) ? A. 0.326 B. 0.571 C. 1.751 D. 3.066 2STP 3STP Use the figure below to answer Question 4. Hydrogen and nitrogen react as shown to formammonia (NH3) . What is true of this reaction? A. Three ammonia molecules are formed, with zeromolecules remaining. B. Two ammonia molecules are formed, with twohydrogen molecules remaining. C. Six ammonia molecules are formed, with zeromolecules remaining. D. Two ammonia molecules are formed, with twonitrogen molecules remaining.5STP 6STP 7STP 8STP Use the table below to answer Questions 9 and 10. Create a graph to show how bond length varies withbond strength. Place bond strength on the x-axis.10STP 11STP 12STP 13STP 14STP 15STP 1PP 2PP 3PP 4PP 5PP 6PP 7PP 8SSC 9SSC 10SSC 11SSC 12SSC 13SSC 14SSC 15SSC 16SSC 17SSC 18SSC 19SSC 20SSC 21SSC 22SSC 23SSC 24SSC 25SSC 26SSC 27SSC 28SSC 29SSC 30SSC 31SSC 32SSC 33SSC 50A 51A 52A 53A 54A 55A 56A 57A 58A 59A 60A 61A 62A 63A 64A 65A 66A 67A 68A 69A 70A 71A 72A 73A 74A 75A 76A 77A 78A 79A 80A 81A 82A 83A 84A 85A 86A 87A 88A 89A 90A 91A 92A 93A 94A Oxygen Consumption If 5.00 L of hydrogen gas,measured at a temperature of 20.0°C and a pressure of80.1 kPa, is burned in excess oxygen to form water, whatmass of oxygen will be consumed? Assume temperatureand pressure remain constant.96A If 2.33 L of propane at 24°C and 67.2 kPa is completelyburned in excess oxygen, how many moles of carbondioxide will be produced?98A 99A 100A 101A Apply Calculate the pressure of (4.671022) moleculesof CO gas mixed with 2.871024 molecules of N2 gas ina 6.00-L container at 34.8°C.Analyze When nitroglycerin (C3H5N3O9) explodes, itdecomposes into the following gases: CO2 , N2 , NO, and H2O . If 239 g of nitroglycerin explodes, what volumewill the mixture of gaseous products occupy at 1.00 atmpressure and 2678°C?104A 105A 106A 107A 108A 109A 110A 111A 112A 113A 114A 115A 116A 117A 118A 119A 1STP 2STP 3STP 4STP 5STP

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