Physical Chemistry
2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Wadsworth Cengage Learning,
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Textbook Question
Chapter 6, Problem 6.42E
At what pressure does the boiling point of water become
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Coulombs Law describes the interaction between two charges and varies by the magnitude of these
charges and inversely with the distance between them.
For atoms, we'll label the charges as the
nuclear charge and electron charge.
9192
9nuclelec
As you go up in atomic number (Z), the number of protons in the nucleus increases, making the charge
on the nucleus increase, so that in general. qnuc
= Z ·(+1)
However if we think only of the electrons in the outermost shells (valence
electrons), they do not see the full strength of the nuclear charge because it
is partially shielded (or canceled out if you prefer) by the core electrons. So
we define something called effective charge.
Shielding
Experiences
net charge
of about 1+
Nucleus
Effective Charge = # of protons
Zeff = Z – core
# of core electrons
In general, Zeff increases as you go across in the periodic table.
1. Fill out the following table to verify that effective charge increases as you go across a row.
Element
Na
Mg
Al
Si
P
S
CI
Ar…
Q2: Calculate the mole fraction of 15 % (w/w) CeH1206?
1. Where did the R constant in PV=nRT come from, and why must we convert everything to the units of the R constant?
2. Why does the density of water change with its temperature?
3. If all of the gas was not vaporized before taking the mass (some stayed in liquid form), how would that affect the final molar mass calculation?
4. If a sample of ethanol (C2H6O) was determined to have a pressure of 2 atm at a temperature of 25°C, what is its density (in g/L)?
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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- Part C in Liters (L) At 25 °C and 1.0 atm pressure, what is the minimum quantity of dry air needed to combust 1.2 L of CH4 (g) completely to CO2(g)? Remember that oxygen is present in the atmosphere to the extent of 209,480 parts per million. Express your answer using two significant figures.arrow_forwardMass of CO2 formed early = 1.2 x 106 g The world burns approximately 3.8×1012 kg of fossil fuel per year. The previous two statements were either given or solved for in part a of the question. The following is the question asked in part b. The current concentration of carbon dioxide in the atmosphere is approximately 376 ppm (by volume). By what percentage does the concentration increase each year due to fossil fuel combustion? Approximate the average properties of the entire atmosphere by assuming that the atmosphere extends from sea level to 15 km and that it has an average pressure of 381 torr and average temperature of 275 K. Assume Earth is a perfect sphere with a radius of 6371 km. Express your answer to two significant figures and include the appropriate units.arrow_forwardAt a depth of 3,000 m below sea level the ambient pressure is equal to 290 atm. At these depths, near the Galapagos Islands, there are hydrothermal vents that release H2O at 350 oC. Which of the following alternatives is true about the water coming out of these vents? Water will freeze Water is released as water vapor, but will condense quickly Liquid water and ice will coexist in equilibrium The water will remain in a liquid state The water molecule is destroyed at this deptharrow_forward
- Sulfur is NOT ductile, and NOT malieable. Is sulfur a metal, non metal, or metalloid?arrow_forwardShow your full solution and explanation. 1. Two (2.00) liters of hydrogen, originally at 25 degree celsius and 750 mm of mercury are heated until a volume of 20 liters and a pressure of 3.50 atmosphere is reached. What is the new temperature? 2. Seventy three (73.0) mL of nitrogen at STP is heatef to 80 degree celsius and the volume increase to 4.53 L. What is the pressure.arrow_forwardHow would you answer these questions?arrow_forward
- bha Please don't provide handwritten soluttionarrow_forward-Volume of trapped gas = 88.57 mL - moles of O2 = 0.00359- Pressure of trapped gas = 756 mmHg- Partial pressure collected O2 =732.2 mm Hg. - temperature = 298.15 Kd. From these results, calculate an experimental value for the ideal gas constant,R in L atm mol–1 K–1. e. Using 0.0821 as the true value for the gas constant, calculate the % error ofthe experiment to the nearest whole number.arrow_forwardWhat is the mass of 50.0L of CO2 at STP? * 1 point 49,300g 19.7g 25.5g 98.2g What is the volume of 27.3g of H2O vapor at STP? * 1 point 14.8L O 21.9L O 11,000L 34.0L What is the mass of 1.34x10^25molecules of Magnesium? * 1 point O 204g hp 2$ & 4. 7 8 9.arrow_forward
- What possible uses exist for the natural gas liquids that are removed from natural gas during its processing?arrow_forward4. List major sources (biogenic and anthropogenic) of ammonia in the air What happen to ammonia when it interacts with water?arrow_forwardIn this figure, a polar stratospheric cloud (PSC) ice crystal is displayed. Chemical reactions that lead ultimately to ozone destruction occur within the thin aqueous layer present at the surface of the crystal. CIONO, B HCI A1 crystal aqueous layer For the reaction labeled as A, the CIONO2 reacts with the aqueous surface layer. Identify species A1 and A2 (note: you only need to identify the species; the order listed is not important). Note: If a species is charged, be sure to include the charge. You do not have to subscript/superscript. For example, NO2 would be written NO2-. А1:arrow_forward
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Intermolecular Forces and Boiling Points; Author: Professor Dave Explains;https://www.youtube.com/watch?v=08kGgrqaZXA;License: Standard YouTube License, CC-BY