The real gases do not follow the ideal gas law of PV = nRT, where P is the pressure, V is the volume, n is the amount of gas, R is the Universal gas constant, and T is the absolute temperature. (a) Identify the variables in the ideal gas that are responsive for the deviation and draw their respective diagrams.

The real gases do not follow the ideal gas law of PV = nRT, where P is the pressure, V is the volume, n is the amount of gas, R is the Universal gas constant, and T is the absolute temperature. (a) Identify the variables in the ideal gas that are responsive for the deviation and draw their respective diagrams.

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...

See similar textbooks

Similar questions

EXERSICE 7 (A) Let A and B be two ideal gases at the same temperature. If mÃ>m³ (where mÃ, m³ are the masses of molecules of gases A and B, respectively) and EA, E, the average kinetic energies of the two gases, choose the correct phrase, giving a justification. (1) EA = EB (ii) EA > EB (iii) EA < EB (iv) Data are insufficient to compare EA, EB.
A gas mixture contains 4.5 mol Br, and 33.1 mol F,. (a) Compute the mole fraction of Br, in the mixture. (b) The mixture is heated above 150°C and starts to react to give BrFs: Br2(g) + 5 F2(g) –→ 2 BrF;(g) At a certain point in the reaction, 2.2 mol BrF5 is present. Determine the mole fraction of Br2 in the mixture at that point.
A 0.516 g sample of a metal, M, reacts completely with sulfuric acid according to M(s) + H,SO,(aq) MSO,(aq) + H,(g) A volume of 223 ml. of hydrogen is collected over water; the water level in the collecting vessel is the same as the outside level. Atmospheric pressure is 756.0 Torr, and the temperature is 25 "C. The vapor pressure of water at 25 "C is 23.8 Torr. Calculate the molar mass of the metal. g/mol molar mass:
The ideal gas law describes the relationship among the volume of an ideal gas (V), its pressure (P), its absolute temperature (T), and number of moles ( n): PV = nRT Under standard conditions, the ideal gas law does a good job of approximating these properties for any gas. However, the ideal gas law does not account for all the properties of real gases such as intermolecular attraction and molecular volume, which become more pronounced at low temperatures and high pressures. The van der Waals equation corrects for these factors with the constants a and b, which are unique to each substance: (P+ ²) (V-nb) = nRT an² The gas constant R is equal to 0.08206 L.atm/(K-mol). Part A A 3.00-L flask is filled with gaseous ammonia, NH3. The gas pressure measured at 16.0 °C is 2.45 atm . Assuming ideal gas behavior, how many grams of ammonia are in the flask? Express your answer to three significant figures and include the appropriate units. View Available Hint(s) mass of NH3 = Submit ▾ Part B HÅ…
Calculate the density of sulfur hexafluoride gas at 410 torr and 34 °C.
2. (a) A helium gas (He) leak resulted in a rectangular vessel (200 cm x 20 cm x 10 cm) becoming pressurized at a temperature of 20 °C with 400 g of helium. Given that the van der Waals constants for helium (He) are: a (L² atm mol?) = 0.0341 b (L mol') = 0.02370 (i) Calculate the pressure exerted by the helium gas in the vessel. (ii) Calculate the root mean square speed of a He atom at 20 °C.
(a) (c) A column of water in a buret is 336 mm Hg high. How high would that column be if it were mercury instead of water? (d) In order for the pressures to be equal, density and height of a column are inversely proportional, therefore the following relationship applies: (denHg)(hHg) = (denH20)(hH20) Note: the density of mercury is 13.6 g/mL and the density of water is 1.00 g/mL. An electrolysis experiment was run for 15 minutes and 45 seconds at an average current of 189 milliamps (mA). The mass lost by the copper anode was 0.0589 grams. (b) Calculate the number of coulombs transferred. (Remember: coulomb = amps x sec) Show full calculation of the height in mercury (remember to use proper significant figures.) Calculate the moles of copper lost from the anode. Based on the moles of copper lost determined in 1c, calculate the moles of electrons transferred. Remember, the reaction at the copper anode is: Cu(s)---> Cu¹² (aq) + 2 e
Decide whether each one of the following statement is correct, not correct, or conditionally correct. Justify your answers in each case. (a) As the pressure increases, a gas molecule travels a shorter distance before it collides with a neighbor. (b) Mean free path of a benzene molecule is larger than that of He.
Use the following (unbalanced) chemical equation to answer the following questions: This equation corresponds to the reaction of gasoline (octane) with oxygen (combustion) that occurs in a car engine. We assume that all gases behave as ideal gases. If T= 0.00°C and P= 1.00 atm, when 4.00 L of octane (2,794.48 g) are consumed, how many liters of O2 are consumed and how many liters of CO2 are produced? The molar mass of octane is 114.2285 g/mol..
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