7. Gases

Van der Waals Equation

7. Gases

Van der Waals Equation

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Van der Waals Equation

Van der Waals Equation

Van der Waals Equation Example 1

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Real Gases and the van der Waals Equation Explained

15:09

Real Gases and the van der Waals Equation Explained

van der Waal's Equation for NON-Ideal Gases

0048 - van der Waals Equation of State

Real vs Ideal Gases & the van der Waals Equation - AP Chemistry Complete Course - Lesson 24.4

Van der Waals Equation of State

Non-Ideal Gases and the Van der Waals Equation

Professor Dave Explains

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03:32

The van der Waals equation explained

Oxford Academic (Oxford University Press)

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Practice this topic

Multiple Choice

Which gaseous compound is expected to have the largest value for the Van der Waals constant b?

The graph below shows the change in pressure as the temperature increases for a 1-mol sample of a gas confined to a 1-L container. The four plots correspond to an ideal gas and three real gases: CO2, N2, and Cl2. (a) At room temperature, all three real gases have a pressure less than the ideal gas. Which van der Waals constant, a or b, accounts for the influence intermolecular forces have in lowering the pressure of a real gas?

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Textbook Question

The graph below shows the change in pressure as the temperature increases for a 1-mol sample of a gas confined to a 1-L container. The four plots correspond to an ideal gas and three real gases: CO2, N2, and Cl2. (b) Use the van der Waals constants in Table 10.3 to match the labels in the plot (A, B, and C) with the respective gases 1CO2, N2, and Cl22.

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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.

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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?

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Textbook Question

Use the van der Waals equation and the ideal gas equation to calculate the volume of 1.000 mol of neon at a pressure of 500.0 atm and a temperature of 355.0 K. Explain why the two values are different. (Hint: One way to solve the van der Waals equation for V is to use successive approximations. Use the ideal gas law to get a preliminary estimate for V.)

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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.)

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Textbook Question

Use the van der Waals equation and the ideal gas equation to calculate the pressure exerted by 1.000 mol of Cl2 in a volume of 5.000 L at a temperature of 273.0 K. Explain why the two values are different.

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.

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Textbook Question

Consider the following gases, all at STP: Ne, SF₆, N₂, CH₄. (g) Which one would have the largest van der Waals b parameter?

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Textbook Question

Consider the following gases, all at STP: Ne, SF₆, N₂, CH₄. (d) Which one has the highest total molecular volume relative to the space occupied by the gas?

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Textbook Question

It turns out that the van der Waals constant b equals four times the total volume actually occupied by the molecules of a mole of gas. Using this figure, calculate the fraction of the volume in a container actually occupied by Ar atoms (b) at 20.27 MPa pressure and 0 °C. (Assume for simplicity that the ideal-gas equation still holds.)

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Textbook Question

Large amounts of nitrogen gas are used in the manufacture of ammonia, principally for use in fertilizers. Suppose 120.00 kg of N21g2 is stored in a 1100.0-L metal cylinder at 280 °C. (b) By using the data in Table 10.3, calculate the pressure of the gas according to the van der Waals equation.

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Textbook Question

A steel container with a volume of 500.0 mL is evacuated, and 25.0 g of CaCO3 is added. The container and contents are then heated to 1500 K, causing the CaCO3 to decompose completely, according to the equation CaCO31s2¡CaO1s2 + CO21g2. (b) Now make a more accurate calculation of the pressure inside the container. Take into account the volume of solid CaO 1density = 3.34 g/mL2 in the container, and use the van der Waals equation to calculate the pressure. The van der Waals constants for CO21g2 are a = 3.59 1L2 # atm2>mol2 and b = 0.0427 L>mol.