5. Does the pressure-volume relationship follow the ideal gas law PV=nRT(is PV constant at constant n and T)Using the room temperature calculate the number of moles in thepressure/volume experiment when the pressure is 1.00atm in 3.1

To calculate the number of moles in the pressure/volume experiment, we can ideal gas law, which is…

Answered: 5. Does the pressure-volume…

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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A 9.00 L tank at 12.6 °C is filled with 7.50 g of carbon dioxide gas and 13.2 g of dinitrogen difluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. mole fraction: x10 carbon dioxide partial pressure: || atm ? mole fraction: dinitrogen difluoride partial pressure: atm Total pressure in tank: || atm
Sketch three isochores for the same gas at three different volumes V1, V2 and V3 where V1 = V3 and V2<V3. How the temperature scale (K vs oC) will change on your plot?
5. There are 1.07 X 103 moles of gas molecules contained in a CO2 cartridge under 5.0-atm of internal pressure. After several uses, the internal pressure is 3.4-atm. How many moles of gas remain in the cartridge? How much gas will remain in the cartridge when the internal pressure equilibrates to standard pressure? (Assume that the temperature and volume remain constant.)
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).
The number of moles of CO2 in that last equation was 0.119 moles.
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- |(V-nb) = nRT The van der Waals equation of state. R stands for the gas constant and n for moles of gas. 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. Ar What are the units of a? 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. Oat ||atm Use the van der Waals equation to calculate the pressure of a sample of water at 430.0 °C with a molar volume of 4.03 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. atm
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A 7.00 L tank at 15.8 °C is filled with 5.07 g of sulfur tetrafluoride gas and 11.5 g of sulfur hexafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. mole fraction: x10 sulfur tetrafluoride partial pressure: || atm mole fraction: sulfur hexafluoride partial pressure: atm Total pressure in tank: atm
For the following reaction: C3H8(g) + 3CO₂(g) + 4H₂O(1) 502(g) The change in gaseous moles, An = To maximize the product yield, the volume of the container should ◆ , so that the pressure will be (> →
The volume of a 0.5333-g sample of gas was measured at 298 K and pressures of 0.059, 0.143, 0.288, 0.341, and 0.489 bar with the results V = 14.8, 6.07, 2.99, 2.45, and 1.75 dm3. What is the molar mass of the gas? Identify which of the following gases is the correct gas sample – N2, H2O, O2 , or NH3? Note: Quantities with specific units must carry the correct units.
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 |(V-nb)=nRT The van der Waals equation of state. R stands for the gas constant and n for moles of gas. 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? What are the units of b? For ammonia the numerical value of a is 4.169 and the numerical value of b is 0.0371. | atm Use the van der Waals equation to calculate the pressure of a sample of ammonia at 170.0 °C with a molar volume of 5.01 L/mol. Round your answer to 3 significant digits. Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round this answer to 3 significant digits also. O atm APR 24 w A olo

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5. Does the pressure-volume relationship follow the ideal gas law PV=nRT (is PV constant at constant n and T) Using the room temperature calculate the number of moles in the pressure/volume experiment when the pressure is 1.00atm in 3.1