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:
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Chapter 1 Solutions
Physical Chemistry
- + |/ 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_forwardConsider 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_forwardThe 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_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_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_forwardPressure (A) Explain the term pressure and state its S.I. unit. (B) Explain Henry’s law. (C)A bottle of H2 has just been received by the technicians in DkIT for use in the instrumentation lab. It is a 47 litre cylinder at a pressure of 50 atmospheres. The normal working pressures is 2 bar. (i) To what volume of gas will that equate at the working pressure? (ii) For how many hours will the gas last if it used at the rate of 0.5dm3 per hour? D)You see your best friend at the bar and you walk up behind her. You accidentally startle her and she takes a step backwards. Unfortunately, she is wearing high heels and her heels come down on your foot. She weighs only 55kg but the size of her heel is 6mm by 6mm.Determine the pressure that she applies on your foot. (E) If a diver dives to a depth of 35 m what will be: (i) the pressure in Pascals due the water column? (3 marks) (ii) the pressure of the air in…arrow_forward
- Thank youarrow_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_forward1.1 (a) A sample of air occupies 1.0 L at 25 °C and 1.00 atm. What pressure is needed to compress it to 100 cm’ at this temperature? 1.2(a) A perfect gas undergoes isothermal compression, which reduces its volume by 2.20 dm³. The final pressure and volume of the gas are 5.04 bar and 4.65 dm', respectively. Calculate the original pressure of the gas in (a) bar, (b) atm. 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? 1.4(a) A sample of 255 mg of neon occupies 3.00 dm at 122 K. Use the perfect gas law to calculate the pressure of the gas. 1.7(a) In an attempt to determine an accurate value of the gas constant, R, a student heated a container of volume 20.000 dm³ filled with 0.251 32 g of helium gas to 500°C and measured the pressure as 206.402 cm of water in a manometer at 25°C. Calculate the value of R from these data. (The density of water at 25°C is 0.997 07 g cm; the construction of a manometer is…arrow_forward
- Q6. (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_forward5) In some system with a constant composition, U is a function of V and T. Write the differential for U.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
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