* Quesbon Moving to another question will save this response. Quèstion 3 For a real gas, when intermolecular attraction forces are dominant The internal pressure T=0, the internal energy U is constant and the compression factor Z=1 Oa. The internal pressure AT>0, the internal energy Uf and the compression factor Z<1 Ob. The internal pressure T>0, the internal energy UI and the compression factor Z<1 Oc. The internal pressure AT=0, the internal energy U ↑ and the compression factor Z=1 %3D Od. Moving to another question will save this response. arch

* Quesbon Moving to another question will save this response. Quèstion 3 For a real gas, when intermolecular attraction forces are dominant The internal pressure T=0, the internal energy U is constant and the compression factor Z=1 Oa. The internal pressure AT>0, the internal energy Uf and the compression factor Z<1 Ob. The internal pressure T>0, the internal energy UI and the compression factor Z<1 Oc. The internal pressure AT=0, the internal energy U ↑ and the compression factor Z=1 %3D Od. Moving to another question will save this response. arch

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

The van der Waals coefficents of mnatomic argon gas are a=0.1345m6 Pa/mol2 and b=32.19 x 106 m/mol . What is the change in temprature ΔT when one mole of argon gas undergoes a Joule free expansion from 0.1 L to 10L ? a. ΔT = -107k b. ΔT = 107k c. ΔT =54k d. ΔT = -54k
218
A vessel of 240 ml capacity contains a certain amount of gas at 35 C and 2 bar pressure. The gas is transferred to another vessel of volume 120 mL at 35C. What would be its pressure in bar? R=8.413 x10-2 L bar/Kmol
One type of gas mixture used in anesthesiologyis a 50%/50% mixture (by volume) of nitrous oxide (N2O) and oxygen(O2), which can be premixed and kept in a cylinder for later use.Because these two gases don’t react chemically at or below 2000 psi, attypical room temperatures they form a homogeneous single gas phase,which can be considered an ideal gas. If the temperature drops below-6C, however, N2O may begin to condense out of the gas phase. Thenany gas removed from the cylinder will initially be nearly pure O2; asthe cylinder empties, the proportion of O2 will decrease until the gascoming from the cylinder is nearly pure N2O. In another test, the valve of a 500 L cylinder full of the gas mixture at 2000 psi (gauge pressure) is opened wide so that the gas rushes out of the cylinder very rapidly. Why might some N2O condense during this process? (a) This is an isochoric process in which the pressure decreases, so the temperature also decreases. (b) Because of the rapid expansion, heat is…
A 0.210 g sample of a metal, M, reacts completely with sulfuric acid according to the reaction M(s)+H2SO4(aq)⟶MSO4(aq)+H2(g) A volume of 219 mL of hydrogen gas is collected over water; the water level in the collecting vessel is the same as the outside level. Atmospheric pressure is 1.0079 bar and the temperature is 25 °C. The vapor pressure of water at 25 °C is 0.03167 bar. Calculate the molar mass of the metal.
Determine the number of degrees of freedom (trans + rot) for each of the following gases; Ne, CO2, H2O. Then calculate the average total kinetic energy (per mole) at 25 celsius for each gas. (R=8.314J K-1 mol-1)
Everything needed is included. An empty 1.0-liter cylinder is filled with 48.0 grams of methane (CH4 ) at 273 K. 2a. Predict (calculate) the pressure, assuming methane behaves as an ideal gas. 2b. Suppose the pressure is measured and is found to actually be 56 atm. Determine the compression factor Z, and indicate whether attractive or replusive intermolecular forces are dominant in methane under these conditions.
The ideal gas constant R is: R = 8.314 J / K*mol What is the value of R expressed in units of L bar K-1 mol-1 ? Express your answer with four significant digits.
A gas cylinder is filled with 4.00 moles of oxygen gas at 300.0 K. The piston is compressed to yield a pressure of 400.0 kPa. What is the volume inside the cylinder? R = 8.31 kPa • dm3 moles • K
given: A real gas has the equation of state Z = 1 + B’ p + C’ p2 at 270 K where B’ = - 0.04135 atm-1 and C’ = 0.00062465 atm-2 Plot the compression factor Z as a function of p in the range between p = 0 atm and p = 200 atm. how to make the table and the plot and also need to show correct units. Determine the value of the pressure (in atm) in that the compression factor Z would change from Z < 1 to Z > 1?
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: n (p+₁ +²2) (v- (V-nb)=nRT 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? The van der Waals equation of state. R stands for the gas constant and n for moles of gas. What are the units of b? For ethane the numerical value of a is 5.507 and the numerical value of b is 0.0651. Use the van der Waals equation to calculate the pressure of a sample of ethane at 105.0 °C with a molar volume of 5.27 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. 0 0 atm atm x10 DO X ロ・ロ

1 k-mol of methane (CH.) is combusted with theoretical air. The products of combustion are at a pressure of 100 kPa. The balanced reaction is given below. CH, + 2[O; + 3.76N:] → CO2 +2H¿0 + 7.52N2 If the products are at T= 40°C, how many k-mols of water are in the liquid phase? (Assume 40°C < Tao) Answer: 1.321 kmol