Physical Chemistry
2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Wadsworth Cengage Learning,
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Chapter 6, Problem 6.18E
Estimate the boiling point of platinum, Pt, if its
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Substance D has the following properties:
ΔHvap = 30.5 kJ/mol
ΔHfus = 5.9 kJ/mol
Tb = 89.4 °C
Tm = -31.6 °C
Specific Heat (solid) = 4.6 J/g·°C
Specific Heat (liquid) = 2.7 J/g·°C
Specific Heat (gas) = 1.5 J/g·°C
Calculate the energy that must be removed to convert 107.6 g of substance D from a gas at 136.1 °C to a solid at -68.0°C. The molar mass of Substance D is 75 g/mol.
Calculate the heat absorbed when 149 g of liquid ethanol at 25.0°C is converted to gaseous ethanol at 96.0°C. The boiling point of ethanol is 78.4°C, the specific heat of liquid ethanol is 2.44 J/(g °C), the heat of vaporization of ethanol is 3.86 × 104 J/mol, and the specific heat of gaseous ethanol is 1.42 J/(g °C).
Calculate the mass of ice required to cool 181 mL of beverage from 24.6 °C to 0.0 °C. Assume a density of 1.00 g/mL and a specific heat capacity of 4.184 J/g·°C for the beverage. The enthalpy of fusion of ice is 6.01 kJ/mol
Chapter 6 Solutions
Physical Chemistry
Ch. 6 - Prob. 6.1ECh. 6 - Prob. 6.2ECh. 6 - Prob. 6.3ECh. 6 - Prob. 6.4ECh. 6 - Prob. 6.5ECh. 6 - Prob. 6.6ECh. 6 - Prob. 6.7ECh. 6 - Prob. 6.8ECh. 6 - 6.9. Identify and explain the sign on in equation...Ch. 6 - 6.10. Use Hess’s law to prove that .
Ch. 6 - 6.11. Calculate the amount of heat necessary to...Ch. 6 - Prob. 6.12ECh. 6 - Assume that the vapH of an evaporating liquid...Ch. 6 - 6.14. As a follow-up to the previous exercise,...Ch. 6 - Prob. 6.15ECh. 6 - 6.16. What is for isothermal conversion of liquid...Ch. 6 -
6.17. Estimate the melting point of nickel, Ni,...Ch. 6 -
6.18. Estimate the boiling point of platinum, Pt,...Ch. 6 - Prob. 6.19ECh. 6 - Prob. 6.20ECh. 6 - 6.21. What assumption is used in the integration...Ch. 6 - Prob. 6.22ECh. 6 - Sulfur, in its cyclic molecular form having the...Ch. 6 - Prob. 6.24ECh. 6 - 6.25. Phosphorus exists as several allotropes that...Ch. 6 - Prob. 6.26ECh. 6 - 6.27. What is higher for a substance: its normal...Ch. 6 - 6.28. Elemental gallium is another substance whose...Ch. 6 - Prob. 6.29ECh. 6 - Consider the sulfur solid-state phase transition...Ch. 6 - 6.31. If it takes mega bars of pressure to change...Ch. 6 - Prob. 6.32ECh. 6 - Four alcohols have the formula C4H9OH: 1-butanol,...Ch. 6 - Prob. 6.34ECh. 6 - At 20.0C, the vapor pressure of ethanol is...Ch. 6 - Prob. 6.36ECh. 6 - Prob. 6.37ECh. 6 - Ethanol has a density of 0.789g/cm3 and a vapor...Ch. 6 - Prob. 6.39ECh. 6 - Prob. 6.40ECh. 6 - Prob. 6.41ECh. 6 - 6.42. At what pressure does the boiling point of...Ch. 6 - Prob. 6.43ECh. 6 - Prob. 6.44ECh. 6 - Prob. 6.45ECh. 6 - Prob. 6.46ECh. 6 - Prob. 6.47ECh. 6 - 6.48. Explain how glaciers, huge masses of solid...Ch. 6 - Prob. 6.49ECh. 6 - Prob. 6.50ECh. 6 - Prob. 6.51ECh. 6 - Prob. 6.52ECh. 6 - Prob. 6.53ECh. 6 - Prob. 6.54ECh. 6 - Prob. 6.55ECh. 6 - Prob. 6.56ECh. 6 - Prob. 6.57ECh. 6 - Use the phase diagram of water in Figure 6.6 and...Ch. 6 - Prob. 6.59ECh. 6 - Prob. 6.60ECh. 6 - At the triple point of a substance, the vapor...Ch. 6 - Prob. 6.62ECh. 6 - Prob. 6.63ECh. 6 - Prob. 6.64ECh. 6 - Prob. 6.65ECh. 6 - Prob. 6.66ECh. 6 - The phase diagram for elemental sulfur is shown in...Ch. 6 - Consider the phase diagram of sulfur in the...Ch. 6 - Prob. 6.69ECh. 6 - Rearrange the Clausius-Clapeyron equation,...
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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- 1. Which of the following processes requires the largest input of energy as heat? raising the temperature of 100 g of water by 1.0 °C vaporization of 0.10 g of water at 100 °C melting 1.0 g of ice at 0 °C warming 1.0 g of ice from −50 °C to 0 °C (specific heat of ice = 2.06 J/g · K)arrow_forwardThe enthalpy change when 1 mol methane (CH4) is burned is 890 kJ. It takes 44.0 kJ to vaporize 1 mol water. What mass of methane must be burned to provide the heat needed to vaporize 1.00 g water?arrow_forwardBenzene, C6H6, is an organic liquid that freezes at 5.5 C (Figure 11.1) to form beautiful, feather-like crystals. How much energy is evolved as heat when 15.5 g of benzene freezes at 5.5 C? (The enthalpy of fusion of benzene is 9.95 kJ/mol.) If the 15.5-g sample is remelted, again at 5.5 C, what quantity of energy is required to convert it to a liquid?arrow_forward
- The cooling effect of alcohol on the skin is due to its evaporation. Calculate the heat of vaporization of ethanol (ethyl alcohol), C2H5OH. C2H5OH(l)C2H5OH(g);H=? The standard enthalpy of formation of C2H5OH(l) is 277.7 kJ/mol and that of C2H5OH(g) is 235.1 kJ/mol.arrow_forward9.46 The heat of fusion of pure silicon is 43.4 kJ/mol. How much energy would be needed to melt a 5.24-g sample of silicon at its melting point of 1693 K?arrow_forward9.45 What happens to the temperature of a material as it undergoes an endothermic phase change? If heat is added, how can the temperature behave in this manner?arrow_forward
- The enthalpy of combustion of hard coal averages 35 kJ/g, that of gasoline, 1.28105 kJ/gal. How many kilograms of hard coal provide the same amount of heat as is available from 1.0 gallon of gasoline? Assume that the density of gasoline is 0.692 g/mL (the same as the density of isooctane).arrow_forwardEqual masses of liquid A, initially at 100C, and liquid B, initially at 50C, are combined in an insulated container. The final temperature of the mixture is 80C. All the heat flow occurs between the two liquids. The two liquids do not react with each other. Is the specific heat of liquid A larger than, equal to, or smaller than the specific heat of liquid B?arrow_forwardDefine the joule in terms of SI base units.arrow_forward
- Carbon tetrachloride, CCl4, is a liquid used as an industrial solvent and in the preparation of fluorocarbons. What is the heat of vaporization of carbon tetrachloride? CCl4(l)CCl4(g);H=? Use standard enthalpies of formation (Table 6.2).arrow_forwardA 25.0 g sample of benzene at 19.9 °C was cooled to its melting point (5.5 °C). How much heat was given off in this process? The specific heat capacity of liquid benzene is 1.74 J/g K, and its heat of fusion is 127 J/g.arrow_forwardHow much heat energy is required to convert 77.6 g of solid iron at 21 °C to liquid iron at 1538 °C? The molar heat of fusion of iron is 13.8 kJ/mol. Iron has a normal melting point of 1538 °C. The specific heat capacity of solid iron is 0.449 J/(g · °C). q= kJarrow_forward
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