Pick a correct description of Charles's law::O A. The volume of a fixed amount of gas is directly proportional to its temperature in Kelvin at constant pressure.B. The volume of a fixed amount of gas is inversely proportional to its pressure at constant temperature.C. The total pressure of a mixture of gases is the simple sum of the partial pressure of all of the gaseous compounds.D. The rates of effusion of gases are inversely proportional to the square roots of their molar masses.E. Equal amounts of gases occupy the same volume at constant temperature and pressure.

Interpretation: The correct statement is to be determined.

Pick a correct description of Charles's law:: O A. The volume of a fixed amount of gas is directly proportional to its temperature in Kelvin at constant pressure. O B. The volume of a fixed amount of gas is inversely proportional to its pressure at constant temperature. O C. The total pressure of a mixture of gases is the simple sum of the partial pressure of all of the gaseous compounds. O D. The rates of effusion of gases are inversely proportional to the square roots of their molar masses. E. Equal amounts of gases occupy the same volume at constant temperature and pressure.

Pick a correct description of Charles's law:: O A. The volume of a fixed amount of gas is directly proportional to its temperature in Kelvin at constant pressure. O B. The volume of a fixed amount of gas is inversely proportional to its pressure at constant temperature. O C. The total pressure of a mixture of gases is the simple sum of the partial pressure of all of the gaseous compounds. O D. The rates of effusion of gases are inversely proportional to the square roots of their molar masses. E. Equal amounts of gases occupy the same volume at constant temperature and pressure.

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.

Question

Pick a correct description of Charles's law::
O A. The volume of a fixed amount of gas is directly proportional to its temperature in Kelvin at constant pressure.
B. The volume of a fixed amount of gas is inversely proportional to its pressure at constant temperature.
C. The total pressure of a mixture of gases is the simple sum of the partial pressure of all of the gaseous compounds.
D. The rates of effusion of gases are inversely proportional to the square roots of their molar masses.
E. Equal amounts of gases occupy the same volume at constant temperature and pressure.

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