Textbook Question
Based on their respective van der Waals constants
( Table 10.3), is Ar or CO2 expected to behave more nearly
like an ideal gas at high pressures?
993
views
Ch.10 - Gases
Chapter 10, Problem 94c
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.
Verified step by step guidance1
To calculate the pressure exerted by CCl4, we can use the Ideal Gas Law, which is expressed as PV = nRT. Here, P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
First, convert the temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature: T(K) = 80 + 273.15.
Next, identify the values for each variable: n = 1.00 mol, V = 33.3 L, and R = 0.0821 L·atm/(mol·K) (the ideal gas constant).
Rearrange the Ideal Gas Law to solve for pressure (P): P = nRT / V.
For the second part of the question, consider the factors that cause deviation from ideal gas behavior. Larger, more complex molecules like CCl4 are more likely to deviate from ideal behavior compared to smaller, simpler molecules like Cl2. This is due to stronger intermolecular forces and larger molecular size in CCl4, which can lead to greater deviations from the assumptions of the Ideal Gas Law.
Verified Solution
Video duration:
1m
This video solution was recommended by our tutors as helpful for the problem above.Was this helpful?
Related Practice
Open Question
In Sample Exercise 10.16, we found that one mole of Cl2 confined to 22.41 L at 0 °C deviated slightly from ideal behavior. Calculate the pressure exerted by 1.00 mol Cl2 confined to a smaller volume, 5.00 L, at 25 °C. (a) Use the ideal gas law for the calculation. (b) Then use the van der Waals equation for your calculation. (Values for the van der Waals constants are given in Table 10.3.) (c) Why is the difference between the result for an ideal gas and that calculated using the van der Waals equation greater when the gas is confined to 5.00 L compared to 22.41 L?
Textbook Question
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.)
631
views
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.
1152
views
Textbook Question
Torricelli, who invented the barometer, used mercury in
its construction because mercury has a very high density,
which makes it possible to make a more compact barometer
than one based on a less dense fluid. Calculate the density
of mercury using the observation that the column of
mercury is 760 mm high when the atmospheric pressure is
1.01 * 105 Pa. Assume the tube containing the mercury is
a cylinder with a constant cross-sectional area.
816
views
Textbook Question
A gas bubble with a volume of 1.0 mm3 originates at the bottom of a lake where the pressure is 3.0 atm. Calculate its volume when the bubble reaches the surface of the lake where the pressure is 730 torr, assuming that the temperature does not change.
691
views