Bundle: Introductory Chemistry: An Active Learning Approach, 6th + LMS Integrated for OWLv2, 4 terms (24 months) Printed Access Card
6th Edition
ISBN: 9781305717428
Author: Mark S. Cracolice, Ed Peters
Publisher: Cengage Learning
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Chapter 15, Problem 114E
It is a hot summer day, and Chris wants a glass of lemonade. There is none in the refrigerator, so a new batch is prepared from freshly squeezed lemons. When finished, there are
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) The salt potassium perchlorate is soluble in water. When 2.84 g of KClO4 is dissolved in 106.00 g of water, the temperature of the solution decreases from 25.00 to 22.54 °C. Based on this observation, calculate the enthalpy of dissolution of KClO4 (in kJ/mol).Assume that the specific heat of the solution is 4.184 J/g °C and that the heat absorbed by the calorimeter is negligible.
3.56 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70 °C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.184 J/g･ °C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water.
When 8.6 grams of a certain compound is dissolved in 78 grams of water in a calorimeter, the temperature of the calorimeter changes from 25.00ºC to 23.09 ºC. Assuming that the specific heat capacity for the resulting solution is 4.184 J/(g oC), and the heat for this solvation is found as x kJ, what is the value of x?
Chapter 15 Solutions
Bundle: Introductory Chemistry: An Active Learning Approach, 6th + LMS Integrated for OWLv2, 4 terms (24 months) Printed Access Card
Ch. 15 - Prob. 1ECh. 15 - Prob. 2ECh. 15 - Prob. 3ECh. 15 - Prob. 4ECh. 15 - Prob. 5ECh. 15 - Prob. 6ECh. 15 - Prob. 7ECh. 15 - Prob. 8ECh. 15 - Prob. 9ECh. 15 - Prob. 10E
Ch. 15 - Prob. 11ECh. 15 - Prob. 12ECh. 15 - Prob. 13ECh. 15 - Prob. 14ECh. 15 - Prob. 15ECh. 15 - Prob. 16ECh. 15 - Prob. 17ECh. 15 - Prob. 18ECh. 15 - Prob. 19ECh. 15 - Prob. 20ECh. 15 - Prob. 21ECh. 15 - Prob. 22ECh. 15 - Prob. 23ECh. 15 - Prob. 24ECh. 15 - Prob. 25ECh. 15 - Prob. 26ECh. 15 - Prob. 27ECh. 15 - Prob. 28ECh. 15 - Prob. 29ECh. 15 - Prob. 30ECh. 15 - Prob. 31ECh. 15 - Prob. 32ECh. 15 - Prob. 33ECh. 15 - Prob. 34ECh. 15 - Prob. 35ECh. 15 - Prob. 36ECh. 15 - Prob. 37ECh. 15 - Prob. 38ECh. 15 - Prob. 39ECh. 15 - Prob. 40ECh. 15 - Predict which compound, CO2 or CS2, has the higher...Ch. 15 - Prob. 42ECh. 15 - Predict which compound, CH4 or CH3F, has the...Ch. 15 - Prob. 44ECh. 15 - Prob. 45ECh. 15 - Prob. 46ECh. 15 - Prob. 47ECh. 15 - Use the following vapor pressure data to answer...Ch. 15 - Prob. 49ECh. 15 - Prob. 50ECh. 15 - Prob. 51ECh. 15 - Prob. 52ECh. 15 - Prob. 53ECh. 15 - Prob. 54ECh. 15 - Prob. 55ECh. 15 - The molar heat of vaporization of substance X is...Ch. 15 - Prob. 57ECh. 15 - Prob. 58ECh. 15 - Prob. 59ECh. 15 - Prob. 60ECh. 15 - Prob. 61ECh. 15 - Prob. 62ECh. 15 - Prob. 63ECh. 15 - Prob. 64ECh. 15 - Prob. 65ECh. 15 - Prob. 66ECh. 15 - Prob. 67ECh. 15 - Prob. 68ECh. 15 - Prob. 69ECh. 15 - Prob. 70ECh. 15 - Prob. 71ECh. 15 - Prob. 72ECh. 15 - Prob. 73ECh. 15 - Prob. 74ECh. 15 - Prob. 75ECh. 15 - Prob. 76ECh. 15 - Find the quantity of energy released in joules as...Ch. 15 - Prob. 78ECh. 15 - Prob. 79ECh. 15 - What is the energy change when the temperature of...Ch. 15 - Prob. 81ECh. 15 - Prob. 82ECh. 15 - Prob. 83ECh. 15 - Prob. 84ECh. 15 - Prob. 85ECh. 15 - Prob. 86ECh. 15 - Prob. 87ECh. 15 - Prob. 88ECh. 15 - Prob. 89ECh. 15 - Prob. 90ECh. 15 - Prob. 91ECh. 15 - Prob. 92ECh. 15 - Prob. 93ECh. 15 - The following information is given for n-pentane...Ch. 15 - Prob. 95ECh. 15 - Prob. 96ECh. 15 - Prob. 97ECh. 15 - The following information is given for bismuth at...Ch. 15 - Prob. 99ECh. 15 - Classify each of the following statements as true...Ch. 15 - Prob. 101ECh. 15 - Prob. 102ECh. 15 - Prob. 103ECh. 15 - Prob. 104ECh. 15 - Prob. 105ECh. 15 - Prob. 106ECh. 15 - Prob. 107ECh. 15 - Prob. 108ECh. 15 - A calorimeter contains 72.0g of water at 19.2C. A...Ch. 15 - Prob. 110ECh. 15 - Prob. 111ECh. 15 - Prob. 112ECh. 15 - Prob. 113ECh. 15 - It is a hot summer day, and Chris wants a glass of...Ch. 15 - Prob. 15.1TCCh. 15 - Prob. 15.2TCCh. 15 - Prob. 15.3TCCh. 15 - Prob. 15.4TCCh. 15 - Prob. 15.5TCCh. 15 - Prob. 15.6TCCh. 15 - Prob. 15.7TCCh. 15 - Prob. 15.8TCCh. 15 - Prob. 1CLECh. 15 - Prob. 2CLECh. 15 - Prob. 3CLECh. 15 - Prob. 4CLECh. 15 - Prob. 5CLECh. 15 - Prob. 6CLECh. 15 - Prob. 7CLECh. 15 - Prob. 1PECh. 15 - Prob. 2PECh. 15 - Prob. 3PECh. 15 - Prob. 4PECh. 15 - Prob. 5PECh. 15 - Prob. 6PECh. 15 - Prob. 7PECh. 15 - Prob. 8PE
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- Are changes in state physical or chemical changes? Explain. What type of forces must be overcome to melt or vaporize a substance (are these forces intramolecular or intermolecular)? Define the molar heat of fusion and molar heat of vaporization. Why is the molar heat of vaporization of water so much larger than its molar heat of fusion? Why does the boiling point of a liquid vary with altitude?arrow_forward9.91 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70 °C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.184 J/g･ °C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water. my answer -38.99 kJ/mol was wrong.arrow_forwardA constant pressure calorimeter contains 286 g of water at 20.0 °C. A 13.41 g of substance X (molar mass 154 g/mol) at 20.0°C was dissolved in this water. The temperature of the solution increased to 23.5 °C. Assuming the specific heat of the mixture is 4.184 J g‑1°C‑1, and the density of the solution is 1.00 g/cm3, calculate the enthalpy change (in kJ) for the dissolution of 1 mole of X.arrow_forward
- 10.71 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70°C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.184 J/g･°C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water.arrow_forwardA geochemist in the field takes a small sample of the crystals of mineral compound X from a rock pool lined with more crystals of X. He notes the temperature of the pool, 17.° C, and caps the sample carefully. Back in the lab, the geochemist dissolves the crystals in 4.00 L of distilled water. He then filters this solution and evaporates all the water under vacuum. Crystals of X are left behind. The researcher washes, dries and weighs the crystals. They weigh 0.080 kg. Using only the information above, can you calculate the solubility of X in water at 17.° C ? If you said yes, calculate it. Be sure your answer has a unit symbol and the right number of significant digits. O yes O no 0 0 x10 ロ･ロ x 3 00 5arrow_forwardA coffee cup calorimeter was used to measure the heat of solution, the change in enthalpy that occurs when a solid dissolves in water. A 10.0 g sample of an ionic compound with a molar mass of 185.0 g/mol was added to a sample of deionized water to produce 60.0 grams of solution. After stirring and dissolving the solid, the temperature was found to change from 25.00 °C to 23.74 °C. Calculate the enthalpy of solution, AHgoln , per mole of salt dissolved. Assume the specific heat of the solution is 4.12 J/(g.°C) and the heat capacity of the calorimeter is 4.10 J/ °C. Calculate the heat change experienced by the calorimeter contents, Icontents · Icontents J Calculate the heat change experienced by the calorimeter, qcal - Ical = J Calculate the heat change produced by the solution process, Isoln · Activate Windowsarrow_forward
- 3. A 262-mL sample of a sugar solution containing 1.22 g of the sugar has an osmotic pressure of 30.3 mmHg at 35°C. Determine the molar mass of the sugar. (1 mmHg = 0.00131atm) A 4.117-g impure sample of glucose (C&H12O6) was burned in a constant-volume calorimeter having a heat capacity of 19.65 kJ/°C. If the rise in temperature is 3.134°C, calculate the percent by mass of the glucose in the sample. Assume that the impurities are unaffected by the combustion process. b)arrow_forwardPotassium nitrate, KNO3, has a molar mass of 101.1 g/mol. In a constant-pressure calorimeter, 23.4 g of KNO3 is dissolved in 259 g of water at 23.00 °C. H₂O KNO3(s) →→→ K+ (aq) + NO3(aq) The temperature of the resulting solution decreases to 21.20 °C. Assume that the resulting solution has the same specific heat as water, 4.184 J/(g. °C), and that there is negligible heat loss to the surroundings. How much heat was released by the solution? 9soln = kJ What is the enthalpy of the reaction? AHrxn= kJ/molarrow_forwardA coffee cup calorimeter was used to measure the heat of solution, the change in enthalpy that occurs when a solid dissolves in water. A 10.0 g sample of an ionic compound with a molar mass of 145.0 g/mol was added to a sample of deionized water to produce 60.0 grams of solution. After stirring and dissolving the solid, the temperature was found to change from 25.00 °C to 23.71 °C. Calculate the enthalpy of solution, AH30ln , per mole of salt dissolved. Assume the specific heat of the solution is 4.15 J/(g.C) and the heat capacity of the calorimeter is 5.30 J/°C. Calculate the heat change experienced by the calorimeter contents, qcontents - 9contents = J Calculate the heat change experienced by the calorimeter, qcal - 9cal = J Calculate the heat change produced by the solution process, qsoln - Isoln = J Calculate AHsoln , the enthalpy of solution for one mole of solid in kilojoules per mole. ΔΗon= kJ/molarrow_forward
- A geochemist in the field takes a small sample of the crystals of mineral compound X from a rock pool lined with more crystals of X. He notes the temperature of the pool, 30.° C, and caps the sample carefully. Back in the lab, the geochemist dissolves the crystals in 750. mL of distilled water. He then filters this solution and evaporates all the water under vacuum. Crystals of X are left behind. The researcher washes, dries and weighs the crystals. They weigh 0.098 kg. O yes Using only the information above, can you calculate the solubility of X in water at 30.° C7 O no If you sald yes, calculate it. Be sure your answer has a unit symbol and 2 significant digits.arrow_forwardWhen 84.64 grams of fictional compound X is added to water to make 449.6 grams of solution, the temperature increases from 20.93 °C to 52.89 °C. What is the heat of solution for compound X given that the molar mass of compound X is 78.43 g/mol? Assume the specific heat capacity of the solution is 4.18 J/g°C. -60.07 kJ/mol 55.66 kJ/mol -55.66 kJ/mol 18.33 kJ/mol 60.07 kJ/molarrow_forwardDon't provide handwritten sollution ... A metal sample weighing 43.5 g and at a temperature of 100.0 °C was placed in 39.9 g of water in a calorimeter at 25.1 °C. At equilibrium the temperature of the water and metal was 33.5 °C. Using the specific heat of water (4.184 J/g °C), calculate how much heat flowed into the waterarrow_forward
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