SubmitPart BWould the volume be different if the gas was argon (under the same conditions)?Match the words in the left column to the appropriate blanks in the sentences on the right.Reset Helpthe sameThe volume would beif the gas was argon because the ideal gas law is dependent onnumber of molestheof the gas and not themassdifferentSubmitRequest AnswerProvide FeedbackNext >MacBook AirDIIDD000000F12F11F9F10F8

ideal gas volume is independent of molar mass of the gas.

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Would the volume be different if the gas was argon (under the same conditions)? Match the words in the left column to the appropriate blanks in the sentences on the right.

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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Concept explainers

Kinetic-Theory of Gases

Kinetic theory of gases is the model or method which was developed in the 19th century by Maxwell and Boltzmann. This is possible as the interatomic force which is of short-range forces that are important for solids and liquids can be neglected for gases. This theory or gas law gives a molecular interpretation of the pressure and temperature of a gas and is consistent with gas laws and Avogadro’s hypothesis. This theory is very helpful to correctly explain the specific heat capacities of many gases, kinetic energy and it also explains the transport qualities such as viscosity, thermal conductivity, and diffusion with molecular parameters. As stated in the kinetic-molecular theory, the temperature of a substance or gas particle is related to the average kinetic energy of the particles of that substance. When a substance is heated, some of the absorbed energy is stored within the particles, while some of the energy increases the motion of the particles, called average kinetic energy.

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Would the volume be different if the gas was argon (under the same conditions)?
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1. A 270-mL flask contains pure helium at a pressure of 759 torr . A second flask with a volume of 455 mL contains pure argon at a pressure of 717 torr A. If we connect the two flasks through a stopcock and we open the stopcock, what is the partial pressure of helium? Express the partial pressure in torr to three significant figures. B. If we connect the two flasks through a stopcock and we open the stopcock, what is the partial pressure of argon? Express the partial pressure in torr to three significant figures. C. If we connect the two flasks through a stopcock and we open the stopcock, what is the total pressure? Express the total pressure in torr to three significant figures.
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