Estimate the behavior of the real gas using the van der Waals equation of state. To prevent gas tank rupture in cases of fire, an engineering team is studying the effect of temperature on gases confined to small volumes. What is the pressure of 3.60 mol of gas D measured at 251 °C in a 1.75-L container assuming real behavior? Express your answer in bar. The error margin is 1%. Provide your answer with 3 significant figures. View Available Hint(s) P = Submit G| ΑΣΦΑΦ Previous Answers ? bar

Estimate the behavior of the real gas using the van der Waals equation of state. To prevent gas tank rupture in cases of fire, an engineering team is studying the effect of temperature on gases confined to small volumes. What is the pressure of 3.60 mol of gas D measured at 251 °C in a 1.75-L container assuming real behavior? Express your answer in bar. The error margin is 1%. Provide your answer with 3 significant figures. View Available Hint(s) P = Submit G| ΑΣΦΑΦ Previous Answers ? bar

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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ntArea/ContentArea.aspx?LocationID=D45454&Location Type=1 E 21 SC R Home E Q E O b O E brary Follow-up and reports 360° repats Overview Plans Resources More - 9 Gases Quiz 6 7 89 10 11- 20 21- 25 Question 2 If a mixture of gases have a pressure of 10 atm and the first gas exerts a partial pressure of 3 atm and the second gas exerts a pressure of 5 atm, what is the pressure of the third gas? Your answer: 10 atm O O atm O 3 atm O 2 atm Clear answer Pause test Back Next Reports/45454/IndividualReport/418373 US O
The ideal gas law is a limiting law, in that it is expected to hold as pressure approaches zero. Suppose the following measured values have been obtained for oxygen gas at 273.15K. Based on the data, calculate R for each pressure value and create a table of pressure and R values (i.e. you are treating R as a variable rather than a constant at this point). Then create a plot R vs p and find the “best value” of R by determining the y-intercept of a straight line fit. (Be sure to label your axes including units).
A flask contains a mixture of two gases: NO2 and Ne. The flask holds 0.519 mol of NO2 and an unknown amount of Ne. If the partial pressure of Ne is 0.43 bar and the total pressure in the flask is 0.83 bar, calculate the mass of Ne in the flask (in g). TIP: You don't need the volume of the flask nor the temperature to solve this problem. Express answer in 2 significant figures.
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+ ou add to the document will 1. At 18°C and 102.0 kPa, 1.29 L of a gas weighs 2.71 g. Calculate the approximate molar mass of the gas. 2. Determine the volume occupied by 4.00 g of oxygen gas at STP. 3. What volume would 15.0 g of argon occupy at 90°C and 735 mm of mercury? 4. Compute the approximate density of methane CH4, at 20°C and 5.00 atm. 5. If the density of carbon monoxide is 3.17 g/L at -20°C and 238 kPa, what is its approximate molar mass? 6. If 200 mL of a gas weighs 0.268 g at STP what is its molar mass? 7. Compute the volume of 11.0 g of nitrous oxide, N₂O, at STP. 8. What volume will 1.216 g of SO, gas occupy at 18°C and 100.6 kPa? 9. Compute the mass of one litre of ammonia gas at STP. 10. Determine the density of H₂S gas at 27°C and 2.00 atm. 11. A 1.225 g mass of volatile liquid is vapourized giving 400 mL of vapour when measured over water at 30°C and 102.6 kPa. The vapour pressure of water at 30°C is 4.27 kPa. What is the molar mass of the liquid. 12. Find the…
One way to measure temperature in some applications is to monitor the gas pressure in a rigid, closed container. What is the temperature (in °C) of such a vessel, calibrated to read 1.00 atm at STP, if the pressure reads 1.14 atm?
Real gases can exist under conditions other than STP. True O False
The rate of effusion of a particular gas was measured and found to be 26.0 mL/min. Under the same conditions, the rate of effusion of pure methane () gas is 47.8 mL/min. What is the molar mass of the unknown gas? Mass = g/mol
Use the van der Waals equation of state to calculate the pressure of 2.00 mol of CH, at 469 K in a 5.90 L vessel. Van der Waals constants can be found in the van der Waals constants table. P = atm Use the ideal gas equation to calculate the pressure under the same conditions. P = atm Under these conditions, would you expect CH, or CCI, to deviate more from ideal behavior? Why? CCI because it occupies a smaller volume and it has greater dispersion forces between molecules. O CH, because it occupies a smaller volume and it has greater dispersion forces between molecules. CH because it occupies a smaller volume and it has smaller dispersion forces between molecules. CCI because it occupies a larger volume and it has smaller dispersion forces between molecules. O CH because it occupies a larger volume and it has smaller dispersion forces þetween molecules. O CCI, because it occupies a larger volume and it has greater dispersion forces between molecules. O O O C O0
KActivity 6 Simulation - Kinetic Molecular Theory View Available Hint(s)
Several years ago there was a big controversy in football that needed chemistry tosolve it! In “Deflategate”, the problem was a lack of understanding of the ideal gaslaw. Use the following data to determine the final gauge pressure of one of thefootballs from that event. If the football was initially inflated to 12.50 psig in thelocker room at 69.0 F, what gauge pressure would it be when the football wastaken to the field at 48.0 F? Atmospheric pressure = 12.30 psi that day.
Consider the two flasks joined together with a stopcock (shown in the diagram below). Calculate the final partial pressure contributed by each gas to the mixture when the stopcock connecting the flasks is opened. (Assume the total volume is 6 L). 4 1 L of N₂ at 303000 Pa 5 L of H₂ at 101000 Pa a. рH₂= 84167 Pa, pN₂ = 50500 Pa = рн₂ 101000 Pa, pN₂= 101000 Pa рH₂=50500 Pa, pN₂ = 84167 Pa рн₂= 134667 Pa, pN₂ = 50500 Pa e. рH₂= 84167 Pa, pN₂ = 134667 Pa оооо O b. OC. O d.