Textbook Question
Calculate the pressure that CCl4 will exert at 80 °C if 1.00 mol occupies 33.3 L, assuming that (c) Which would you expect to deviate more from ideal behavior under these conditions, Cl2 or CCl4? Explain.
Ch.10 - Gases
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 10, Problem 94b
Calculate the pressure that CCl4 will exert at 80 °C if 1.00 mol occupies 33.3 L, assuming that (a) CCl4 obeys the ideal-gas equation (b) CCl4 obeys the van der Waals equation. (Values for the van der Waals constants are given in Table 10.3.)
Verified step by step guidance1
Convert the temperature from Celsius to Kelvin by adding 273.15 to the given temperature (80 °C).
Use the ideal gas law equation, \( PV = nRT \), where \( P \) is pressure, \( V \) is volume, \( n \) is the number of moles, \( R \) is the ideal gas constant (0.0821 L·atm/mol·K), and \( T \) is the temperature in Kelvin, to calculate the pressure assuming CCl4 behaves as an ideal gas.
For the van der Waals equation, use the formula \( \left( P + \frac{an^2}{V^2} \right)(V - nb) = nRT \), where \( a \) and \( b \) are the van der Waals constants for CCl4. Substitute the known values into this equation.
Solve the van der Waals equation for pressure \( P \) by rearranging the terms and substituting the values for \( a \), \( b \), \( n \), \( V \), and \( T \).
Compare the pressures obtained from the ideal gas law and the van der Waals equation to understand the effect of intermolecular forces and molecular volume on the behavior of CCl4.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Ideal Gas Law
The Ideal Gas Law is a fundamental equation in chemistry that relates the pressure, volume, temperature, and number of moles of a gas. It is expressed as PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature in Kelvin. This law assumes that gas particles do not interact and occupy no volume, making it applicable under many conditions but not all.
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Ideal Gas Law Formula
Van der Waals Equation
The Van der Waals equation is an adjustment of the Ideal Gas Law that accounts for the volume occupied by gas molecules and the attractive forces between them. It is expressed as (P + a(n/V)²)(V - nb) = nRT, where 'a' and 'b' are constants specific to each gas. This equation provides a more accurate description of real gas behavior, especially at high pressures and low temperatures, where deviations from ideality are significant.
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Pressure Units and Conversion
Pressure is a measure of force exerted per unit area and is commonly expressed in units such as atmospheres (atm), pascals (Pa), or mmHg. In calculations involving gases, it is crucial to ensure that pressure is in the correct units that correspond with the other variables in the gas equations. Conversions may be necessary, for example, converting mmHg to atm by using the conversion factor 1 atm = 760 mmHg.
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Related Practice
Textbook Question
Table 10.3 shows that the van der Waals b parameter has units of L/mol. This means that we can calculate the sizes of atoms or molecules from the b parameter. Refer back to the discussion in Section 7.3. Is the van der Waals radius we calculate from the b parameter of Table 10.3 more closely associated with the bonding or nonbonding atomic radius discussed there? Explain.
Textbook Question
Based on their respective van der Waals constants( Table 10.3), is Ar or CO2 expected to behave more nearlylike an ideal gas at high pressures?
Textbook Question
Which statement concerning the van der Waals constants a and b is true? (a) The magnitude of a relates to molecular volume, whereas b relates to attractions between molecules. (b) The magnitude of a relates to attractions between molecules, whereas b relates to molecular volume. (c) The magnitudes of a and b depend on pressure. (d) The magnitudes of a and b depend on temperature.
Textbook Question
Torricelli, who invented the barometer, used mercury inits construction because mercury has a very high density,which makes it possible to make a more compact barometerthan one based on a less dense fluid. Calculate the densityof mercury using the observation that the column ofmercury is 760 mm high when the atmospheric pressure is1.01 * 105 Pa. Assume the tube containing the mercury isa cylinder with a constant cross-sectional area.