None The van der Waalsequation of state(P + ñ³ ³) (V - nb) = nRT(A) 10 cm³.mol'.(C)1 cm³.mol'contains a term representing a “molecular size". Theapproximate magnitude of this term is(B) 10°³ cm³ -mol'.(D)10³ cm³.mol'.

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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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2 dN F (V )dV = N M 4 7 (- 2 ART MV 3/2y ? exp( 2 RT where dN, the number of particles having a velocity between v and v+dV, V velocity of molecules, M moleculer mass of gase, T temperature = |V ² † (V )dV =? 2-
3. (a) jf 10.0 mjL of H2jSO4 (sp. jr. 1.50, containing 48.7% of combined SO3 by weight) is diluted to 400 mL, what is the normality of the solution as an acid? (b) What volume of 6.00 M H2SO4 should be added to this in order to make the resulting mixture 1.00N as an acid? FW's : H2SO4 = 98; SO3 = 80 %3D
1.3 (a) To what temperature must a 1.0 L sample of a perfect gas be cooled from 25 °C in order to reduce its volume to 100 cm³?
1. At an altitude of 150 km, the pressure is about 2.7 x 10-⁹ bar and T≈ 500 K. (a) Assuming for simplicity that the air consists entirely of nitrogen, calculate the mean free path (in m) under these conditions. For N₂ molecules o=4.50 × 10-19 m². (b) What is the average collision frequency (in sec-¹) between N₂ molecules?
(a) Use the following data for NH3 (g) at T = 273 K to evaluate B2P (T). (Here Z is the compressibility factor, PV/RT). P (bar) 0.10 0.20 0.30 0.40 0.50 0.60 0.70 Note: You will need to fit this data to a least-squares line. (b) At standard temperature (273.15 K), the density of O₂ varies with pressure as indicated in the table below: P (bar) 0.25331 0.50663 0.75994 1.01325 Z-1 1.519 x 10-4 3.038 x 10-4 4.557x 10-4 6.071 x 10-4 7.583 x 10-4 9.002 x 10-4 1.0551 x 10-3 2 p(g/L) 0.356985 0.714154 1.071485 1.428962 Use this data to find the second virial coefficient, B2v, of oxygen. Note that mo2 = 31.9988 Daltons. (Hint: It will be useful to determine the molar volume from each value of p.)
20. A mixture consisting of 6 kg of O, and 9 kg of N, has a pressure of 3 bar and temperature of 20°C. For the mixture determine the following : (i) The mole fraction of each component ; (iii) The specific gas constant; (v) The partial pressures and partial volumes. (ii) The average molecular weight ; (iv) The volume and density; [Ans. (i) 0.3684, 0.6315 ; (iüi) 29.475 ; (iii) 0.282 kJ/kg K ; (iv) 4.13 m?, 3.629 kg/m² ; (v) 1.1 bar, 1.894 bar ; 1.52 m², 2.61 m²)
(a) For liquid benzene β = 9.30 x 10-5 atm-1 at 20 °C and 1 atm pressure. Utilizing the equation derived ln(v2/v1)=α(T2-T1)-β(P2-P1) and assuming β to be independent of pressure, find the percentage change in volume of a sample of benzene on being compressed at constant temperature from a pressure of 1 atm to a pressure of 11 atm. (b) What would be the percentage change in volume of an ideal gas compressed over the same pressure interval at constant temperature?
4. (a) Determine the reduced pressure (P,), volume (V,), and temperature (T, ) for a 50 L sample of water at 23 bar and 400 K. For H2O gas, Te = 647.14 K, P. = 220.64 bar, and Vc=55.95 L. (b) Determine the pressure, volume and temperature for a sample of hydrogen which is in a corresponding state with the H2O in part (a). For hydrogen, Te = 32.98 K, Pc = 12.93 bar and mc =64.20 L.
+ |/ 00 %24 D. Two bulbs are connected by a stopcock. The 7.50 L bulb contains nitric oxide (NO) at a pressure of 0.340 bar, and the 2.50 L bulb contains oxygen (O,) at a pressure of 0.510 bar. 02 ON After the stopcock is opened, the gases mix and react to produce nitrogen dioxide (CON) 2 NO(g) + 0,(g) – 2 NO,(g) Considering that the volume remains unchanged during the experiment, how does the total pressure in the bulbs change if the reaction is allowed to go to completion? The total pressure will remain constant. O There is not enough information to determine how the total pressure will change. O The total pressure will decrease. O The total pressure will increase. MacBook Pro ( The %23 %24 7. 4. 5. 3. R %3D K. H. B C. option command MOSISO
(c) The Cp of a sample of a perfect gas is related to the temperature as shown below: Cp/(J.K-1) = 38.77+1.52| Calculate q, w, AU, and AH when the temperature is raised from 8°C to 124°C (i) at constant pressure, (ii) at constant volume. (8)
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.
(5) Using the data in Table 1C.3 (from the textbook), calculate the pressure that 2.500 moles of carbon dioxide confined in a volume of 1.000 L at 450 K exerts. Compare the pressure with that calculated assuming ideal-gas behavior.

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The van der Waals equation of state (P + ñ³ ³) (V - nb) = nRT (A) 10 cm³.mol'. (C) 1 cm³.mol' contains a term representing a “molecular size". The approximate magnitude of this term is (B) 10°³ cm³ -mol'. (D) 10³ cm³.mol'.