![Physical Chemistry](https://www.bartleby.com/isbn_cover_images/9781133958437/9781133958437_largeCoverImage.gif)
Interpretation:
Liquid nitrogen comes in large cylinders that required special tank carts and hold 120 L of liquid at 77 K. Given the density of liquid nitrogen of 0.840 g/cm3, using the van der Waals equation, the volume of the nitrogen gas after it evaporates at 77 K and atmospheric pressure is to be estimated.
Concept introduction:
The
![Check Mark](/static/check-mark.png)
Trending nowThis is a popular solution!
![Blurred answer](/static/blurred-answer.jpg)
Chapter 1 Solutions
Physical Chemistry
- Consider Argon (Ar) gas at a pressure of 1 bar and temperature of 300 K. The equivalent hardsphere radius (known as the Van Der Waal radius) of an Argon molecule is 188 picometers (pm)and its atomic mass is 39.948u. Note that 1u = 1.6605 x 10-27kg. a)How many molecules are contained in a cube 1 cm by 1 cm by 1 cm? b)Estimate the mean free path. At scales much larger than this, a continuum description holds. c)What is the density of the gas? d)Estimate the "root mean squared" molecular speed, i.e. SQRT( (V^2) ) e)Estimate the dynamic and kinematic viscosities. Compare these with literature values, forexample from webbook.nist.edu. f) Plot the variation of dynamic viscosity with temperature in the range between 300K and3000K at a fixed pressure of 1 bar. Use Matlab, Python, Mathematica, or any other softwareyou may choose.arrow_forwardHelpppparrow_forwardShow complete solutions and enclose all final answers in a box. Round off final answers to 4 decimal places and use floating values for intermediate answers. A gas column is separated into two segments by a non-permeable partition. On the first segment is 1.63 moles of Helium with volume V1 and on the second segment is 3.84 moles of Oxygen gas with volume V2. Consider both gases to be ideal and at the same pressure P and temperature T. If the partition is removed, calculate the change in entropy of the gaseous system.arrow_forward
- Some N2 gas is mixed with some O2 gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured, and found to be 0.130 kPa. key carbon hydrogen nitrogen sulfur oxygen chlorine Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 3 significant digits. You may assume each gas behaves as an ideal gas. gas mole fraction partial pressure ☐ x10 N2 ||] ☐ kPa ☑ 02 ☐ ☐ kPaarrow_forward+ |/ 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 MOSISOarrow_forwardDirections: To better understand the relationship among temperature, pressure, and volume of ideal gases, we can use the virtual simulation titled “Gas Law Simulator” which can be accessed at http://ch301.cm.utexas.edu/simulations/js/idealgaslaw. Using the virtual simulator, determine the relationships between the properties of gases by recording the pressure, temperature, and volume of the unknown gas. To accomplish this task, complete the following table. NOTE: DO NOT ERASE THE GIVEN QUANTITIES. To calculate the number of moles of the gas, use the ideal gas equation. Attach your solutions on another sheet of paper or digitally write. TEMPERATURE PRESSURE VOLUME 120 K 150 L 120 K 300 L 300 K 150 L 300 K 300 L Answer the following questions: 1.What conditions increase the kinetic energy of the particles of Gas A? 2. What conditions decrease the kinetic energy of the particles of Gas A? 3. What conditions increase the kinetic…arrow_forward
- The amount of NH3 in a smoggy atmosphere was measured to be 33.9 ppm. The barometric pressure was 0.9678 bar. Compute the partial pressure of NH3 in atmospheres. Enter your answer in accordance with the question statementarrow_forwardQ6. (a)The vander waals equation is used to describe the behaviour of real gases but still not so useful in many industrial applications. Explain why?(3) (b)In kinetic molecular theory of gases it is assumed that The molecules of the gases occupy negligible volume as compared to the total volume of the gas' which factor can be actually described by this postulate?(2)arrow_forward6. Calculate the stoichiometric amount of anhydrous ammonia (kg NH3/day) needed to reduce 800 ppm NO2 to 250 ppm NO2 in a flue gas. The actual flow rate is 3,000 m’/min at 700°C and 1 atm.arrow_forward
- P 1) Pinte X A ACTIVITY X EX_FjXNtRGOvhgYzM_rMIZzEwnvfJ17evaEjsK94/edit# Last edit was 2 minutes ago 11 BIUA 田回▼ 1三 ニ=,E▼E ... .. 1. Calculations A. Direction: Calculate the given problems and use the gas laws to determine pressure, volume, or temperature of a gas under certain conditions of change. Show your solutions. Encirce your final answer. 1. The gas inside the tire has a volume of 20.00 L at a pressure of 5.00 atm. Calculate the pressure of the gas if its volume is reduced to 10.0 at the same temperature. 2. If 150.00 mL of N2 gas was collected at 760 torr, what is the new volume of the gas when the pressure is compressed to 740 torr at the same temperature? 3. At 300 K, the given amount of fluorine gas has a volume of 30.0 L. What will be the temperature if the gas occupies a volume of 25 L at constant pressure? 4. A certain gas sample has a volume of 40.00 L at 273 K. At constant pressure. the volume increase to 50 00 L What will be the final temperature of the gas? 5 At…arrow_forwardP total=P1+P2+P3 P container A =3x287kPa =861 kPa P container B= 1/3*429kPa = 143 kPa P total=861 kPa+143 kPa = 1004 kPa Apply the significant figure rule to the final answer.arrow_forward2. Evaluate the following integrals. ● -5 dx 5x • S√1 + x dx 3. The pressure of one mole of a van der Waals gas is a function of volume and temperature. Determine if dP is an exact or inexact differential. P ---- RT V-b a V2arrow_forward
- Physical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,Chemistry for Engineering StudentsChemistryISBN:9781285199023Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
![Text book image](https://www.bartleby.com/isbn_cover_images/9781133958437/9781133958437_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781285199023/9781285199023_smallCoverImage.gif)