A real gas most closely approaches the behaviour of an ideal gas under conditions of: O STP Low pressure and high temperature O High pressure and low temperature Low pressure and low temperature High pressure and high temperature Show Transcribed Text Consider a hypothetical gas which has the following Van der Waals constants: a = 0.0 L² bar mol-² b = 0.0344 L mol-1 Under conditions of very high pressures, what would you predict about the experimental volume of the gas?

A real gas most closely approaches the behaviour of an ideal gas under conditions of: O STP Low pressure and high temperature O High pressure and low temperature Low pressure and low temperature High pressure and high temperature Show Transcribed Text Consider a hypothetical gas which has the following Van der Waals constants: a = 0.0 L² bar mol-² b = 0.0344 L mol-1 Under conditions of very high pressures, what would you predict about the experimental volume of the gas?

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

Calculate the density of propane gas, C3H8, at 20.0oC and 1.15 atm?
A small carbon dioxide gas cylinder used to propel paint balls has a mass of 56.3g. When all the gas is expelled from the cylinder and the cartridge is empty, the cylinder has a mass of 50.4g. If the volume of the cylinder is 25cm3 and the temperature of the cylinder was initially 23 c, determine the initial pressure of the gas.
how many moles of gas are there in a 38.0L container at 25C 0.712 atm? (Given: universal gas constant R = 0.082057 L • atm / mol • K)
A sample of N2N2 gas has a volume of 19.0 L at a pressure of 1.50 atm and a temperature of 23 ∘C. What volume, in liters, will the gas occupy at 3.50 atm and 231 ∘C? Assume ideal behavior.
3..Calculate the volume of the ideal gas if 0.280 mol of it has a pressure of 3.03 atm, and a temperature of 55.0 Celsius. Use R = 0.0821 L-atm/ mol- K for the value of the gas constant.
A container with nitrogen N2 gas had an initial volume of 1.34 L and conditions of 25.9 ∘∘C and 1.2 atm. What will be the volume in liters of the gas if the conditions change to 36.8 ∘∘C and 2.1 atm?
A sample of an ideal gas has a volume of 3.40 L3.40 L at 12.80 ∘C12.80 ∘C and 1.40 atm.1.40 atm. What is the volume of the gas at 22.00 ∘C22.00 ∘C and 0.989 atm?
Hi, can someone please confirm if this would be the right answer, I'm not fully sure. Thank you!!
What is the molecular weight of a gas which has a density of 2.25 g / L at 20.0oC and 1.12atm?
What is the volume occupied by 0.398 moles of di-oxygen gas at a pressure of 2.48 atm and a temperature of 465 K (ideal gas)? What is the volume occupied by 0.398 moles of di-oxygen gas at a pressure of 2.48 atm and a temperature of 105 K (van der Waals gas):
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
Sometimes in lab we collect the gas formed by a chemical reaction over water (see sketch at right). This makes it easy to isolate and measure the amount of gas produced. Suppose the H₂ gas evolved by a certain chemical reaction taking place at 30.0 °C is collected over water, using an apparatus something like that in the sketch, and the final volume of gas in the collection tube is measured to be 116. mL. g G Sketch of a gas-collection apparatus X collected gas water Calculate the mass of H₂ that is in the collection tube. Round your answer to 2 significant digits. You can make any normal and reasonable assumption about the reaction conditions and the nature of the gases. chemical reaction