07:12Real vs Ideal Gases & the van der Waals Equation - AP Chemistry Complete Course - Lesson 24.4Jeremy Krug397views
Multiple ChoiceWhich gaseous compound is expected to have the largest value for the Van der Waals constant b?a) O2b) CH3CH3c) HBrd) S8e) Ne449views1rankHas a video solution.
Textbook QuestionThe 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? 628viewsHas a video solution.
Textbook QuestionThe 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. 631viewsHas a video solution.
Textbook QuestionWhich 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.1693viewsHas a video solution.
Textbook QuestionBased 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?906viewsHas a video solution.
Textbook QuestionUse 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.)3437viewsHas a video solution.
Textbook QuestionCalculate 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.)567viewsHas a video solution.
Textbook QuestionUse 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.2288views1rankHas a video solution.
Textbook QuestionTable 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.1026viewsHas a video solution.
Textbook QuestionConsider the following gases, all at STP: Ne, SF6, N2, CH4. (g) Which one would have the largest van der Waals b parameter?624viewsHas a video solution.
Textbook QuestionConsider 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?569viewsHas a video solution.
Textbook QuestionIt 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.)1316viewsHas a video solution.
Textbook QuestionLarge 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.876viewsHas a video solution.
Textbook QuestionA 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.434viewsHas a video solution.
Textbook QuestionThe Rankine temperature scale used in engineering is to the Fahrenheit scale as the Kelvin scale is to the Celsius scale. That is, 1 Rankine degree is the same size as 1 Fahrenheit degree, and 0 °R = absolute zero. (b) What is the value of the gas constant R on the Rankine scale in 1L ~ atm2>1°R ~ mol2? (c) Use the van der Waals equation to determine the pressure inside a 400.0-mL vessel that contains 2.50 mol of CH4 at a temperature of 525 °R. For CH4, a = 2.253 1L2 ~ atm2>mol2 and b = 0.04278 L>mol.537viewsHas a video solution.
Open QuestionWhich statement(s) concerning the van der waals constants a and b is true?185viewsHas a video solution.
Open QuestionA real gas differs from an ideal gas because the molecules of real gas have116views1commentsHas a video solution.