The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to predict the relationship between pressure p, volume V and temperature T for gases better than the Ideal Gas Law does: p+a (V-nb)=nRT The van der Waals equation of state. R stands for the gas constant and n for moles of gas. The parameters a and b must be determined for each gas from experimental data. Use the van der Waals equation to answer the questions in the table below. 0 For carbon dioxide the numerical value of a is 3.592 and the numerical value of b is 0.0429. ? atm Use the van der Waals equation to calculate the pressure of a sample of carbon dioxide at 95.0 °C with a molar volume of 0.257 L/mol. Round your answer to the correct number of significant digits. Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round your answer to the correct number of significant digits. O atm x10 X 5

The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to predict the relationship between pressure p, volume V and temperature T for gases better than the Ideal Gas Law does: p+a (V-nb)=nRT The van der Waals equation of state. R stands for the gas constant and n for moles of gas. The parameters a and b must be determined for each gas from experimental data. Use the van der Waals equation to answer the questions in the table below. 0 For carbon dioxide the numerical value of a is 3.592 and the numerical value of b is 0.0429. ? atm Use the van der Waals equation to calculate the pressure of a sample of carbon dioxide at 95.0 °C with a molar volume of 0.257 L/mol. Round your answer to the correct number of significant digits. Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round your answer to the correct number of significant digits. O atm x10 X 5

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to predict the relationship between pressure p, volume V and temperature T for gases better than the Ideal Gas Law does: |(V-nb) =nRT The van der Waals equation of state. R stands for the gas constant and n for moles of gas. p+a The parameters a and b must be determined for each gas from experimental data. Use the van der Waals equation to answer the questions in the table below. What are the units of a? What are the units of b? ? For ammonia the numerical value of a is 4.169 and the numerical value of b is 0.0371. Use the van der Waals equation to calculate the pressure of a sample of ammonia at 170.0 °C with a molar volume of 2.56 L/mol. Round your answer to the correct number of significant digits. atm Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round your answer to the correct number of significant digits. atm
The ideal gas law is a limiting law, in that it is expected to hold as pressure approaches zero. Suppose the following measured values have been obtained for oxygen gas at 273.15K. Based on the data, calculate R for each pressure value and create a table of pressure and R values (i.e. you are treating R as a variable rather than a constant at this point). Then create a plot R vs p and find the “best value” of R by determining the y-intercept of a straight line fit. (Be sure to label your axes including units).
The number of moles of CO2 in that last equation was 0.119 moles.
The ideal gas law describes the relationship among the pressure P, volume V, number of moles n, and absolute temperature T of an ideal gas. Here is the relationship expressed mathematically: PV = nRT where R is a proportionality constant. The units of R are determined by the units of pressure and volume used in the equation. When bar used for pressure and L for volume, the appropriate R value is 0.08314 L bar mol-¹ K-¹. Part A How many air molecules are in a 4.05 x 3.66 x 3.05 m³ room? Assume atmospheric pressure of 1.00 bar, a room temperature of 20.0 °C, and ideal behavior. Express your answer using three significant figures. ► View Available Hint(s) VE ΑΣΦ + Review | Constants | molecules
The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to predict the relationship between pressure p, volume V and temperature T for gases better than the Ideal Gas Law does: p+a- |(V-nb) = nRT The van der Waals equation of state. R stands for the gas constant and n for moles of gas. The parameters a and b must be determined for each gas from experimental data. Use the van der Waals equation to answer the questions in the table below. Ar What are the units of a? What are the units of b? For water the numerical value of a is 5.464 and the numerical value of b is 0.0305. Oat ||atm Use the van der Waals equation to calculate the pressure of a sample of water at 430.0 °C with a molar volume of 4.03 L/mol. Round your answer to the correct number of significant digits. Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round your answer to the correct number of significant digits. atm
Hydrogen gas is produced by the reaction between metallic aluminum and aqueous hydrochloric acid. 2 Al(s) + 6 HC1(aq) 2 AICI, (aq) + 3 H, (g) > The hydrogen gas produced by this reaction is typically collected via water displacement. During this process, the hydrogen gas becomes saturated with water vapor. If 234.0 mL of gas with a total pressure of 1.03 atm is collected via water displacement at 29.4 °C, what is the partial pressure of the hydrogen gas in the sample? The vapor pressure of water at 29.4 °C is 30.75 torr. PH, atm How many grams of aluminum must have reacted to produce this quantity of hydrogen gas? mass of aluminum: II
Water vapor is a polar gas molecule. Because of this it has fairly strong interactions with itself in the gas phase that can make it behave less like an ideal gas that other gases under similar conditions. What is the difference between the calculated pressures found using the ideal gas law and found using the van der Waals gas equation for 1 mole of water vapor at -100°C in a 1.00L container. (van der Waals constants for water are a = 5.464 L2 atm mol-2, b = 0.03049 L mol-1) i atm
The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to predict the relationship between pressure p, volume V and temperature T for gases better than the Ideal Gas Law does: (p+a n2/V2) (V-nb) =nRT The van der Waals equation of state. R stands for the gas constant and n for moles of gas. The parameters a and b must be determined for each gas from experimental data. Use the van der Waals equation to answer the questions in the table below. What are the units of a? What are the units of b? For argon the numerical value of a is 1.337 and the numerical value of b is 0.0320. Use the van der Waals equation to calculate the pressure of a sample of argon at −110.0°C with a molar volume of 0.384/Lmol. Round your answer to 3 significant digits. = atm Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round this answer to 3 significant digits also. =…
c) This relationship is known as Graham's Law of Effusion. Since both gases are at te same temperature, they must have the same average kinetic energy (½ mv²), where m is mass and v is velocity (like speed). Since both gases have the same average kinetic energy, you can state that ½ muvL2 = v ². Multiplying both sides by 2 gives you m v 2 y ². Rearranging the equation to get H H LL H H 2 m = m both masses on the same side of the equation will give you mu/mH = V 2/VL2. In 3a and 3b, you probably noticed that the heavy gas particles took twice as long to diffuse as the light gas particles. This means that the light gas particles are moving twice as fast, VH/VL = ½. Therefore, V 2/VL2 = ¼. How many times heavier is the heavy gas compared to the light gas? d) If the light gas was Ne, what would be a reasonable identity for the heavy gas?
|(V-nb)=DnRT The van der Waals equation of state. R stands for the gas constant and n for moles of gas. p+a- v2 The parameters a and b must be determined for each gas from experimental data. Use the van der Waals equation to answer the questions in the table below. What are the units of a? What are the units of b? For argon the numerical value of a is 1.337 and the numerical value of b is 0.0320. atm Use the van der Waals equation to calculate the pressure of a sample of argon at -90.0 °C with a molar volume of 0.192 L/mol . Round your answer to 3 significant digits. Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round this answer to 3 significant digits also. atm
According to the ideal gas law, a 1.024 mol sample of xenon gas in a 1.047 L container at 272.4 K should exert a pressure of 21.86 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For Xe gas, a = 4.194 L2atm/mol2 and b = 5.105×10-2 L/mol.
The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to predict the relationship between pressure p, volume V and temperature T for gases better than the Ideal Gas Law does: ( p+a |(V-nb)=nRT The van der Waals equation of state. R stands for the gas constant and n for moles of gas. The parameters a and b must be determined for each gas from experimental data. Use the van der Waals equation to answer the questions in the table below. What are the units of a? What are the units of b? For ammonia the numerical value of a is 4.169 and the numerical value of b is 0.0371. | atm Use the van der Waals equation to calculate the pressure of a sample of ammonia at 170.0 °C with a molar volume of 5.01 L/mol. Round your answer to 3 significant digits. Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round this answer to 3 significant digits also. O atm APR 24 w A olo