Part C Calculate the relative difference of the real (van-der- Waals) gas pressure to the ideal gas pressure under these conditions in %. Assume the ideal gas pressure to be 100%. By how many % does the predicted pressure increase (positive answer) or decrease (negative answer) upon the use of the van - der - Waals corrections compared to the ideal gas law? Express your answer as a percentage with 3 significant figures. For carbon dioxide gas (CO₂), the constants in the van der Waals equation 3 3 m are a = 0.364J*ol² and b = 4.27 x 10 -ol. -5m m m For carbon dioxide gas (CO₂), the constants in the van der Waals equation are a 0.364 J-m³/mol and b= 4.27 x 10 m³/mol.

Part C Calculate the relative difference of the real (van-der- Waals) gas pressure to the ideal gas pressure under these conditions in %. Assume the ideal gas pressure to be 100%. By how many % does the predicted pressure increase (positive answer) or decrease (negative answer) upon the use of the van - der - Waals corrections compared to the ideal gas law? Express your answer as a percentage with 3 significant figures. For carbon dioxide gas (CO₂), the constants in the van der Waals equation 3 3 m are a = 0.364J*ol² and b = 4.27 x 10 -ol. -5m m m For carbon dioxide gas (CO₂), the constants in the van der Waals equation are a 0.364 J-m³/mol and b= 4.27 x 10 m³/mol.

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

Water vapor is a polar gas molecule. Because of this it has fairly strong interactions with itself in the gas phase that can make it behave less like an ideal gas that other gases under similar conditions. What is the difference between the calculated pressures found using the ideal gas law and found using the van der Waals gas equation for 1 mole of water vapor at -100°C in a 1.00L container. (van der Waals constants for water are a = 5.464 L2 atm mol-2, b = 0.03049 L mol-1) i atm
Some N, gas is mixed with some O, gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured, and found to be 1250. torr. key carbon hydrogen nitrogen sulfur dlo oxygen chlorine Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 4 significant digits. You may assume each gas behaves as an ideal gas. gas mole fraction partial pressure torr torr
Some N2 gas is mixed with some O2 gas, and The picture shows a representative sample of the mixture. The total pressure of the mixture is measured, and found to be 1.55atm. Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to three significant digits. You may assume each gas behaves as an ideal gas.
Oo.151. Subject:- Chemistry
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: n 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. For water the numerical value of a is 5.464 and the numerical value of b is 0.0305. | atm Use the van der Waals equation to calculate the pressure of a sample of water at 445.0 °C with a molar volume of 2.47 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. ||atm APR 49 X W 24 : MacBook Air DD 80 DO0 O00 888 F9 F10 F7 F8 F5 F6 F2 F3 F4
A 6.00 L tank at 14.5 °C is filled with 10.2 g of sulfur tetrafluoride gas and 5.04 g of carbon dioxide gas. You can assume both gases behave as ideal gases under these conditions. Calculate the partial pressure of each gas in the tank. Be sure your answers have the correct number of significant digits. sulfur tetrafluoride carbon dioxide partial pressure: partial pressure: 0 atm atm 10 X
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 800. torr. gas N₂ 0₂ carbon nitrogen oxygen 0 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. mole fraction partial pressure torr key torr hydrogen x sulfur chlorine X S OL A
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: 2 p+a (V-nb)=nRT The van der Waals equation of state. R stands for the gas constant and n for moles of gas. v? 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 195.0 °C with a molar volume of 4.12 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. || atm O
A gas of unknown molecular mass was allowed to effuse through a small opening under constant pressure conditions. It required 72 s for 1.0 L of the gas to effuse. Under identical experimental conditions it required 27 s for 1.0 L of 02 gas to effuse. Calculate the molar mass of the unknown gas. (Remember that the faster the rate of effusion, the shorter the time required for effusion of 1.0 L; that is, rate and time are inversely proportional.) 367.1175859 X g/mol
A gas mixture contains 1.0 mol neon, 2.0 mol argon, and 3.0 mol krypton in a 10.0 L flask at 0°C. Determine the partial pressure of neon.
A 5.00 L tank at 7.96 °C is filled with 10.8 g of chlorine pentafluoride gas and 4.88 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. ol. mole fraction: x10 chlorine pentafluoride Ar ? partial pressure: atm mole fraction: dinitrogen difluoride partial pressure: atm Total pressure in tank: atm
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 I for gases better than the Ideal Gas Law does: 72 (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 argon the numerical value of a is 1.337 and the numerical value of b is 0.0320. Use the van der Waals equation to calculate the pressure of a sample of argon at -110.0 °C with a molar volume of 2.98 L/mol Round your answer to the correct number of significant digits. atm 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 x10 §