One mol of O2(g) undergoes a transformation from the initial state T 300 K and %D V1 20.0 L to the final state T2 400 K and V2 2.0 L. In this regime O2(g) is reasonably well described by the van der Waals equation of state, with constants 1.364 atm L? mol-2 and b = 3.19 × 10–2 L mol¬'. Also in this temperature range the molar heat capacity at constant volume of O2(g) has the approximately constant value 20.8 J K-l mol-1. Recalling that for a van der Waals gas n? a V? Ae T what is the internal energy change AU of the gas in the transformation (T1, V1) → (T2, V2)?

One mol of O2(g) undergoes a transformation from the initial state T 300 K and %D V1 20.0 L to the final state T2 400 K and V2 2.0 L. In this regime O2(g) is reasonably well described by the van der Waals equation of state, with constants 1.364 atm L? mol-2 and b = 3.19 × 10–2 L mol¬'. Also in this temperature range the molar heat capacity at constant volume of O2(g) has the approximately constant value 20.8 J K-l mol-1. Recalling that for a van der Waals gas n? a V? Ae T what is the internal energy change AU of the gas in the transformation (T1, V1) → (T2, V2)?

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

Please don't provide handwritten solution ...
You have a perfect gas that undergoes thermal compression (constant temperature) which reduces its volume by 2.50 dm³. The final pressure and volume are 2.01 bar and 1.98 dm³, respectively. Calculate the original pressure in torr.
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).
(no subject) - ftar X с < 71″F OPA ! 1 2 app.101edu.co F1 o Mail- Francesca X 2 W F2 #m A sample of gas contains 5.25 moles at 37.8 °C in a volume of 3.61 L. If 0.530 moles of gas are removed from the initial 5.25 moles and the temperature increased to 52.8 °C while pressure is held constant, then what is the new volume of the gas, in liters? 3 E Homepage - CHI X 4 O $ 3 Aktiv Chemistry X R DII F5 % 5 G molar mass of o X T A 6 F6 Question 34.c of 34 Y University of Dela X * & 7 PrtScn FB 8 Online Payment Home 9 ✔ End F10 Sign In 1 4 7 +/- PgUp 0 2 50 8 F11 + 6 9 0 PgDn
A sealed container holding 0.0255 L0.0255 L of an ideal gas at 99.526 kPa99.526 kPa and 73 °C73 °C is placed into a refrigerator and cooled to 37 °C37 °C with no change in volume. Calculate the final pressure of the gas.
9.26 mol of argon gas is admitted to an evacuated 4,546.84 cm3 container at 38.34oC. The gas then undergoes an isochoric heating to a temperature of 293.66oC. What is the final pressure?
A moture of gaseous reactants is put nto a cyinder, where a chemical reaction turns them nto gaseous products. The cyinder has a pton that moves in or out, as necessary, to keep a constant pressure on the moture of 1 am. The cyinder is aso submerged in a large insulated water bath. (See sketch at nght) From previous expermenes, this chemicai reacton is known to release 136. of erergy. The postion of the pston is monitored, andRs determined from ts data that the pston does 366. of work on the system duning the reacon he en eemicer endtermic endthem Csthe tamwef the ater bah e Ooes the piton move in or o Des heat fon i t ut the as miue much heat fows beure your aner ha he camect umber of gnicant digits
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.
An average gas fireplace uses about 200 gallons (760,000 cm3) of propane gas per year. Assume that the propane, C3H8, behaves as a perfect gas for the conditions of this problem, which are 1.00 atm and 22°C. What is the mass of gas used?
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: p+a n #2²7) (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 water the numerical value of a is 5.464 and the numerical value of b is 0.0305. Use the van der Waals equation to calculate the pressure of a sample of water at 430.0 °C with a molar volume of 1.92 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. 1 0 П atm atm x10 H X ロ・ロ S
A piece of dry ice (solid carbon dioxide) with a mass of 5.49 gg is placed in a 10.0-LL vessel that already contains air at 709 torr and 25 ∘C a. After the carbon dioxide has totally sublimed, what is the partial pressure of the resultant CO2 gas in the container at 25 ∘C? b. After the carbon dioxide has totally sublimed, what is the total pressure in the container at 25 ∘C? Express your answers in atmospheres to three decimal places.
Based on their respective van der Waals constants, which of these two gases: Xe (a = 4.137 L² atm mol-2, b = 0.0516 L mol-1) or CO2 (a = 3.610 L²atm mol-2, b = 0.0429 L mol-1) is expected to behave more nearly like an ideal gas at high pressures? Explain.