The ideal gas law describes the relationship between pressure (P), temperature (T), volume (V), and the number of moles of gas (n). PV = nRT The additional symbol, R, represents the ideal gas constant. The ideal gas law is a good approximation of the behavior of gases when the pressure is low and the temperature is high. (What constitutes low pressure and high temperature varies with different gases.) In 1873, Johannes Diderik van der Waals proposed a modified version of the ideal gas law that better models the behavior of real gases over a wider range of temperature and pressure. na P + ")(v – nb) = nRT In this equation the additional variables a and b represent values characteristic of individual gases.

The ideal gas law describes the relationship between pressure (P), temperature (T), volume (V), and the number of moles of gas (n). PV = nRT The additional symbol, R, represents the ideal gas constant. The ideal gas law is a good approximation of the behavior of gases when the pressure is low and the temperature is high. (What constitutes low pressure and high temperature varies with different gases.) In 1873, Johannes Diderik van der Waals proposed a modified version of the ideal gas law that better models the behavior of real gases over a wider range of temperature and pressure. na P + ")(v – nb) = nRT In this equation the additional variables a and b represent values characteristic of individual gases.

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

For many purposes we can treat ammonia (NH3) as an ideal gas at temperatures above its boiling point of −33. °C. Suppose the temperature of a sample of ammonia gas is raised from 15.0 °C to 16.0 °C, and at the same time the pressure is changed. If the initial pressure was 0.18 kPa and the volume increased by 40.0%, what is the final pressure? Round your answer to 2 significant digits. kPa x10 X
A 4.52 g sample of nitrogen gas, N2(g), is held in a 3.00 L gas flask at 298 K. Calculate the pressure of the nitrogen gas in the flask in kPa. Give your answer to three significant figures. Do not include units. Data: Molar mass N2: 28.02 g mol-1
A sample of an ideal gas at 1.00 atm and a volume of 1.59 L was placed in a weighted balloon and dropped into the ocean. As the sample descended, the water pressure compressed the balloon and reduced its volume. When the pressure had increased to 80.0 atm, what was the volume of the sample? Assume that the temperature was held constant.
For many purposes we can treat ammonia NH3 as an ideal gas at temperatures above its boiling point of −33.°C. Suppose the temperature of a sample of ammonia gas is raised from 46.0°C to 78.0°C, and at the same time the pressure is increased by 5.0%. Does the volume of the sample increase, decrease, or stay the same? If you said the volume increases or decreases, calculate the percentage change in the volume. Round your answer to the nearest percent.
For many purposes we can treat ammonia (NH, ) as an ideal gas at temperatures above its boiling point of - 33. °C. Suppose the temperature of a sample of ammonia gas is raised from 50.0 °C to 82.0 °C, and at the same time the pressure is increased by 5.0%. increase Does the volume of the sample increase, decrease, or stay the same? decrease ? stays the same If you said the volume increases or decreases, calculate the percentage change in the volume. Round your answer to the nearest percent. %
A flask contains 740 mmHg of nitrogen (N2) gas in a 4.00 L container at 25.0 °C. If 44.0 g of carbon dioxide (CO2) gas is added to this flask at constant volume and temperature without any loss of the nitrogen already inside, what is the final pressure (in atm) of the container? Assume both gases behave as ideal gases. Given: 1 atm =760 mmHg Enter the numerical value (no units), using 3 significant figures. Type your answer...
A student recovered0.398g of THF vapor in a 125 mL flask. Assuming the vapor is an ideal gas with a molar volume of 22.4 L/mol, calculate the molar mass of THF.
Dinitrogen difluoride gas is collected at 10.0 °C in an evacuated flask with a measured volume of 15.0 L. When all the gas has been collected, the pressure in the flask is measured to be 0.110 atm . Calculate the mass and number of moles of dinitrogen difluoride gas that were collected. Be sure your answer has the correct number of significant digits.O mass: |X10 mole: | mol dlo Ar
Zn reacts with hydrochloric acid to give zinc chloride and hydrogen gas. A sample of 5 g of a Zn mineral requires 10 mL of commercial HCl of 37% purity, by weight and density 1.19 g/mL, to react completely. Find: a) The mass of zinc contained in the sample. b) The purity of the zinc mineral. c) The pressure exerted by the hydrogen gas collected in a 2 L container and at a temperature of 20ºC.please use conversion factors and mark the solutions
Chlorine pentafluoride gas is collected at 26.0 °C in an evacuated flask with a measured volume of 5.0 L. When all the gas has been collected, the pressure in the flask is measured to be 0.160 atm. Calculate the mass and number of moles of chlorine pentafluoride gas that were collected. Round your answer to 2 significant digits. mass: g mole: mol x10 ×
8
A sample of an ideal gas at 1.00 atm and a volume of 1.89 L was placed in a weighted balloon and dropped into the ocean. As the sample descended, the water pressure compressed the balloon and reduced its volume. When the pressure had increased to 35.0 atm, what was the volume of the sample? Assume that the temperature was held constant.