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All Textbook Solutions for Chemistry: Matter and Change
6STP7STP8STP9STP10STP11STP12STP13STP14STP1PP2PP3PP4PP5PP6PP7PP8PP9PP10PP11PP12PP13PP14SSC15SSC16SSC17SSC18SSC19SSC20PP21PP22PP23PP24PP25PP26PP27PP28PP29PP30PP31SSC32SSC33SSC34SSC35SSC36SSC37SSC38PP39PP40PP41PP42PP43PP44PP45PP46SSC47SSC48SSC49SSC54AWhat is the difference between a solute and a solvent?56A57A58A59A60A61A62A63A64AHow do 0.5M and 2.0M aqueous solutions of NaCl differ?66A67A68A69A70A71A72A73AHow much CaCl2 , in grams, is needed to make 2.0 L ofa 3.5M solution?Stock solutions of HCl with various molarities are frequentlyprepared. Complete Table 14.7 by calculatingthe volume of concentrated, or 12M, hydrochloric acidthat should be used to make 1.0 L of HCl solution witheach molarity listed.76A77A78AIf you dilute 20.0 mL of a 3.5M solution to make100.0 mL of solution, what is the molarity of the dilutesolution?80A81A82A83AWhat is the mole fraction of H 2 S O 4 in a solution containingthe percentage of sulfuric acid and water shownin Figure 14.25?85A86A87A88A89A90A91A92A93A94A95A96A97A98A99AIn the lab, you dissolve 179 g of MgCl2 into1.00 L of water. Use Table 14.6 to find the freezing pointof the solution.Cooking A cook prepares a solution for boiling by adding12.5 g of NaCl to a pot holding 0.750 L of water. Atwhat temperature should the solution in the pot boil?Use Table 14.5 for needed data.102AIce Cream A rock salt (NaCl), ice, and water mixture isused to cool milk and cream to make homemade icecream. How many grams of rock salt must be added towater to lower the freezing point by 10.0°C?Apply your knowledge of polarity and solubility topredict whether solvation is possible in each situationshown in Table 14.9. Explain your answers.105AWhich solute has the greatest effect on the boiling pointof 1.00 kg of water: 50.0 g of strontium chloride (SrCl2) or 150.0 g of carbon tetrachloride (CCl4) ? Justify youranswer.Study Table 14.4. Analyze solubility and temperaturedata to determine the general trend followed by thegases (NH3,CO2,O2) in the chart. Compare this trendto the trend followed by most of the solids in the chart.Identify the solids listed that do not follow the generaltrend followed by most of the solids in the chart.108AIf you prepared a saturated aqueous solution of potassiumchloride at 25°C and then heated it to 50°C, wouldyou describe the solution as unsaturated, saturated, orsupersaturated? Explain.How many grams of calcium nitrate (Ca(NO3)2) wouldyou need to prepare 3.00 L of a 0.500M solution?111A112A113A114AInfer Dehydration occurs when more fluid is lost from the body than is taken in. Scuba divers are advised to hydrate their bodies before diving. Use your knowledge of the relationship between pressure and gas solubility to explain the importance of hydration prior to a dive.Graph Table 14.10 shows solubility data that was collectedin an experiment. Plot a graph of the molarity ofKI versus temperature. What is the solubility of KI at55°C?Design an Experiment You are given a sample of a solid solute and three aqueous solutions containing that solute. How would you determine which solution is saturated, unsaturated, and supersaturated?Compare Which of the following solutions has thehighest concentration? Rank the solutions from thegreatest to the smallest boiling point depression. Explainyour answer. a. 0.10 mol NaBr in 100.0 mL solution b. 2.1 mol KOH in 1.00 L solution c. 1.2 mol KMnO4 in 3.00 L solution119A120A121A122A123A124A125A126A127A128A129A1STP2STP3STP4STP5STP6STP7STP8STP9STP10STP11STP12STP13STP14STP15STP16STP17STP18STP19STP1SSC2SSC3SSC4SSC5SSC6SSC7SSC8SSC9PP10PP11PP12PP13PP14PP15PP16PP17PP18PP19PP20PP21PP22PP23PP24PP25PP26PP27PP28PP29PP30PP31SSC32SSC33SSC34SSC35SSC36PP37PP38PP39SSC40SSC41SSC42SSC43SSC44SSC45PP46PP47PP48SSC49SSC50SSC51SSC52SSC53SSC53A54A55A56A57A58A59A60A61A62A63A64A65A66AMetallurgy A 25.0-g bolt made of an alloy absorbed250 J of heat as its temperature changed from 25.0°C to78.0°C. What is the specific heat of the alloy?68A69A70A71A72A73AHow many joules of heat are lost by 3580 kg of granite asit cools from 41.2°C to -12.9°C? The specific heat ofgranite is 0.803J/(gC) .Swimming Pool A swimming pool measuring 20.0m12.5m is filled with water to a depth of 3.75m. If the initial temperature is 18.4°C, how much heatmust be added to the water to raise its temperature to29.0°C? Assume that the density of water is 1.000 g/mL.How much heat is absorbed by a 44.7-g piece of leadwhen its temperature increases by 65.4°C?77AAlloys When a 58.8-g piece of hot alloy is placed in125 g of cold water in a calorimeter, the temperature ofthe alloy decreases by 106.1°C, while the temperature ofthe water increases by 10.5°C. What is the specific heat ofthe alloy?79A80A81A82AsUse information from Figure 15.24 to calculate howmuch heat is required to vaporize 4.33 mol of waterat 100°C.Agriculture Water is sprayed on oranges during afrosty night. If an average of 11.8 g of water freezes oneach orange, how much heat is released?Grilling What mass of propane (C3H8) must be burnedin a barbecue grill to release 4560 kJ of heat? The Hcomb of propane is -2219 kJ/mol.Heating with Coal How much heat is liberated when5.00 kg of coal is burned if the coal is 96.2% carbon bymass and the other materials in the coal do not react? Hcomb of carbon is -394 kJ/mol.How much heat is evolved when 1255 g of water condensesto a liquid at 100°C?A sample of ammonia (Hsolid=5.66kJ/mol) liberates5.66 kJ of heat as it solidifies at its melting point.What is the mass of the sample?89A90A91A92A93A94A95A96A97A98A99A100A101A102A103AHeat was added consistently to a sample of water to producethe heating curve in Figure 15.26. Identify what is happening in Sections 1, 2, 3, and 4 on the curve.Bicycling Describe the energy conversions that occur when a bicyclist coasts down a long grade, then struggles to ascend a steep grade.Hiking Imagine that on a cold day you are planning to take a thermos of hot soup with you on a hike. Explain why you might fill the thermos with hot water first before filling it with the hot soup.Differentiate between the enthalpy of formation of H2O(l)andH2O(g) . Why is it necessary to specify thephysical state of water in the following thermochemicalequation CH4(g)+2O2(g)CO2(g)+2H2O(lorg)H=?Analyze both of the images in Figure 15.27 in terms ofpotential energy of position, chemical potential energy,kinetic energy, and heat.Apply Phosphorus trichloride is a starting material for the preparation of organic phosphorous compounds.Demonstrate how thermochemical equations a and b can be used to determine the enthalpy change for the reaction PCl3(l)+Cl2(g)PCl5(s) . a. P4(s)+6Cl2(g)4PCl3(l)H=1280kJ b. P4(s)+10Cl2(g)4PCl5(s)H=1774kJCalculate Suppose that two pieces of iron, one with amass exactly twice the mass of the other, are placed in aninsulated calorimeter. If the original temperatures of thelarger piece and the smaller piece are 90.0°C and 50.0°C,respectively, what is the temperature of the two pieceswhen thermal equilibrium has been established? Referto Table R-9 on page 975 for the specific heat of iron.111Asample of natural gas is analyzed and found to be88.4% methane (CH4) and 11.6% ethane (C2H6) bymass. The standard enthalpy of combustion of methaneto gaseous carbon dioxide (CO2) and liquid water (H2O) is -891 kJ/mol. Write the equation for the combustionof gaseous ethane to carbon dioxide and water.Calculate the standard enthalpy of combustion of ethaneusing standard enthalpies of formation from Table R-11on page 975. Using that result and the standard enthalpyof combustion of methane in Table 15.3, calculate theenergy released by the combustion of 1 kg of natural gas.113A114A115A116A117A118A119A120A121A122A123A124A125A126A127A1STP2STP3STP4STP5STP6STP7STP8STP9STP10STP11STP12STP13STP14STP15STP16STP17STP18STP1PP