If pressure is expressed in atmospheres and volume is expressed in liters, PAV has units of Latm (liters x atmospheres). Rememberthat 1 atm = 101,325 Pa, and that 1 L = 1 dm3. Use this information to determine the number of joules corresponding to 4 L atm.eTextbook and MediaSave for LaterAttempts: 0 of 1 usedSubmit Answerasus COLLECTIONpri sc1121719VIZI&34.78.R.YU

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If pressure is expressed in atmospheres and volume is expressed in liters, PAV has units of Latm (liters x atmospheres). Remember that 1 atm = 101,325 Pa, and that 1 L = 1 dm³3. Use this information to determine the number of joules corresponding to 4 Latm. eTextbook and Media Save for Later Attempts: 0 of 1 used Submit Answer asus COLLECTION prt sc 120 17 & 7\ %23 4. 6. 8. E R T Y. P

If pressure is expressed in atmospheres and volume is expressed in liters, PAV has units of Latm (liters x atmospheres). Remember that 1 atm = 101,325 Pa, and that 1 L = 1 dm³3. Use this information to determine the number of joules corresponding to 4 Latm. eTextbook and Media Save for Later Attempts: 0 of 1 used Submit Answer asus COLLECTION prt sc 120 17 & 7\ %23 4. 6. 8. E R T Y. P

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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colle com/course.html?courseld3D169856748OpenVellumHMAC=Da46387336edc299b16e49c591bf9ad36#10001 For Practice 10.5 - Enhanced - with Feedback I Review | Constants | Periodic Table An 8.45 L tire contains 0.532 mol of gas at a temperature of 320 K. You may want to reference (Pages 425 - 430) Section 10.5 while completing this problem. Part A What is the pressure (in atm) of the gas in the tire? Express the pressure to three significant figures and include the appropriate units. HA ? Value Units Submit Request Answer Next > Provide Feedback P Pearson 11:17 AM A a O (x a 12/10/2021 75°F Partly sunny arch BHJC04Z022B01 E7 O010ahotmai) com 远

At STP, 9.00 mol of gas occupies approximately what volume in liters?
4.Initial Pressure = 95 kPa, Initial Volume = 4.0 L, Final Pressure = 101 kPa, Final Volume = 6.0 L and Final Temperature = 471 K. Solve for Initial Temperature. (x10^ due to SF) Answer: _x10^_ Unit: _
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D Question 33 A large evacuated flask initially has a mass of 134,567 g. When the flask is filled with a gas of unknown molar mass to a pressure of 735 torr at 31 °C, its mass is 137.456 g. when the flask is evacuated again and then filled with water at 31 °C, its mass is 1067.9 g (d H2O = 0.997 g/mL). Assuming the ideal gas %3D equation applies, calculate the molar mass of the gas. O 69.6 g/mol 36.3 g/mol O 1.3 g/mol O 45.2 g/mol
ere's the second problem. You are doing an experiment in a laboratory that is 30.ºC and 1.080 atm of pressure. You take a 0.240L flask that weighs 98.005g and fill it with CO₂. After it is filled it weighs 98.206g. Calculate the molar volume of the CO₂! VSTP = P₁V₁T STP T1PSTP 1.080 * 0.240* 273 303*1 = 0.233L 1.200 * 0.240 = 0.2889 0.4899 98-206-98-005 +0.288 = 0.4 0.489/44.81 = 0.0111mol.com 0-233/0.0111 = 20.99 L/mol Mass of air = (density of air)(volume of flask) 1.200 * 0.240 = 0. 0.2889 Mass of CO₂ = (Mass of flask filled with CO₂) - (Mass of empty flask) + (Mass of air) 92-206-98·005 +0.288 = 0 0.4899
+ 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…
Battery A sample of methane gas at a pressure of 0.876 atm and a temperature of 20.9 °C, occupies a volume of 882 mL. If the gas is allowed to expand at constant temperature until its pressure is 0.606 atm, the volume of the gas sample will be 1 pts 2req mL. Visited Battery Lew 1 pts 2req Submit Answer Retry Entire Group 9 more group attempts remaining 12 AM Screen On Us 12 AM Apr 22 And u cnec +1 (404) 502- I don't have T refuse to sh I have been re +1 (770) 899-245 Felt that
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Using the conversion between atmospheres and mm Hg (1 atm = 760 mm Hg), calculate %3D the value for R with units of L-mm Hg-K-1-mol-1. (Show all work and round to three significant digits.)
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