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 6.9E
Identify and explain the sign on
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Calculate the amount of energy in kilojoules needed to change 315 gg of water ice at −−10 ∘C∘C to steam at 125 ∘C∘C
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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- Using the explanation of unbalanced forces as the source of surface tension, justify why it requires energy to increase the surface area of a liquid. Is there any circumstance in which energy is given off when increasing a liquids surface area?arrow_forwardAnswer 6 and 7 pls. Thanksarrow_forwardSuppose that 117.2 J of heat energy is required to completely vaporize 4.3 g of a pure liquid. If the molar mass of the liquid is 80.75 g/mol, what is the molar enthalpy of vaporization of the liquid?arrow_forward
- There are three sets of sketches below, showing the same pure molecular compound (ammonia, molecular formula NH3) at three different temperatures. The sketches are drawn as if a sample of ammonia were under a microscope so powerful that individual atoms could be seen. Only one sketch in each set is correct. Use the slider to choose the correct sketch in each set. You may need the following information: melting point of NH3: -77.7 °C boiling point of NH3: −33.3 °C A B (Choose one) (Choose one) (Choose one) -54. °℃ 3 -94. °℃ 5 29. °C 4 5arrow_forwardIn an experiment, 10.0 g of ice at -20°C is converted into steam with a temperature of 110°C. How much energy is required for this process?(DHvap = 2,260 J/g; DHfus = 334 J/g; cs(ice) = 2.06 J/(g × °C); cs(water) = 4.18 J/(g × °C); cs(steam) = 1.99 J/(g × °C))arrow_forwardHow much heat is required to convert 5.23 g of ice at -10.0 ∘C to water at 23.0 ∘C? (The heat capacity of ice is 2.09 J/(g⋅∘C), ΔHvap(H2O)=40.7kJ/mol, and ΔHfus(H2O)=6.02kJ/mol.) Express your answer with the appropriate units.arrow_forward
- Using 2 mols of ice, a student performed an experiment to determine the molar enthalpy of fusion for water. The percent error for the experiment was 4.5%, and the measured value was larger than the accepted value, AH6.01 How much heat (q), in joules, was absorbed during the experiment? mol a). - 12,561 J O b) + 270 J Oc) + 8374 d) + 12,561 J O e) - 270 Jarrow_forwardHow much energy in kilojoules is released when 28.6 g of ethanol vapor at 82.0 ∘C is cooled to -16.0 ∘C? Ethanol has mp=−114.1∘Cmp=−114.1∘C, bp=78.3∘Cbp=78.3∘C, ΔHvap=38.56kJ/molΔHvap=38.56kJ/mol, and ΔHfusion=4.93kJ/molΔHfusion=4.93kJ/mol. The molar heat capacity is 112.3 J/(K⋅mol)J/(K⋅mol) for the liquid and 65.6 J/(K⋅mol)J/(K⋅mol) for the vapor.arrow_forwardWhen 95.0 grams of ethanol condenses to liquid, how much energy is lost? H(vap) 38.6 kJ/mol and H(fus) 4.60 kJ/mol are the heats of vaporization and fusion, respectively, for ethanol. Ethanol has a molecular weight of 46.arrow_forward
- Calculate the amount of energy in kilojoules needed to change 369 g of water ice at –10 °C to steam at 125 °C. The following constants may be useful: Cm (ice) = 36.57 J mol-1 °C-1 Cm (water) = 75.40 J mol-1 °C-1 Cm (steam) = 36.04 J mol-1 °C-1 Afus H = +6.01 kJ mol-1 Avap H = +40.67 kJ mol- 1arrow_forwardI really need to understand both questionsarrow_forwarda)The table below gives two values of Delta H° for phase changes in molecular iodine. One value is the standard enthalpy of fusion and the other is the standard enthalpy of sublimation. b)Write a thermochemical equation to represent the vaporization of molecular iodine. Estimate the value for the standard enthalpy of vaporization(Show your work to support your quantitative answer to this problem )arrow_forward
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