The relationship between Dalton’s law and kinetic theory of gases has to be explained. Concept Introduction: Postulates of Kinetic theory: 1. In a gas, there are a huge number of tiny particles called as molecules of similar size and weight. 2. Unlike solids, the interaction between the molecules are said to be negligible. 3. In a gas, the state of molecules is in random motion with different velocities from zero to infinity in all possible direction. 4. On comparison with volume of gas, the size of the molecule is negligible. 5. A perfect elastic collision should take place when the molecules collide with each other. 6. A pressure is exerted as the molecules collide on the walls of the container. During the impact of collision, the pressure of gas is the average force per unit area of the molecules. Higher will be the pressure, larger the number of impacts. 7. Because of random motion of molecules in gas, molecules posses kinetic energy that varies as absolute temperature.

Question

Want to see the full answer?

Answer 1

Question

Chapter 8, Problem 15ALQ

Interpretation Introduction

Interpretation: The relationship between Dalton’s law and kinetic theory of gases has to be explained.

Concept Introduction:

Postulates of Kinetic theory:

1. In a gas, there are a huge number of tiny particles called as molecules of similar size and weight.

2. Unlike solids, the interaction between the molecules are said to be negligible.

3. In a gas, the state of molecules is in random motion with different velocities from zero to infinity in all possible direction.

4. On comparison with volume of gas, the size of the molecule is negligible.

5. A perfect elastic collision should take place when the molecules collide with each other.

6. A pressure is exerted as the molecules collide on the walls of the container. During the impact of collision, the pressure of gas is the average force per unit area of the molecules. Higher will be the pressure, larger the number of impacts.

7. Because of random motion of molecules in gas, molecules posses kinetic energy that varies as absolute temperature.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

Correct each molecule in the drawing area below so that it has the skeletal ("line") structure it would have if it were dissolved in a 0.1 M aqueous solution of HCI. If there are no changes to be made, check the No changes box under the drawing area. No changes. HO Explanation Check NH, 2 W O :□ G ©2025 M unter Accessibility

An expression for the root mean square velocity, vrms, of a gas was derived. Using Maxwell’s velocity distribution, one can also calculate the mean velocity and the most probable velocity (mp) of a collection of molecules. The equations used for these two quantities are vmean=(8RT/πM)1/2 and vmp=(2RT/M)1/2 These values have a fixed relationship to each other.(a) Arrange these three quantities in order of increasing magnitude.(b) Show that the relative magnitudes are independent of the molar mass of the gas.(c) Use the smallest velocity as a reference for establishing the order of magnitude and determine the relationship between the larger and smaller values.

The reaction of solid dimethylhydrazine, (CH3)2N2H2, and liquefied dinitrogen tetroxide, N2O4, has been investigated for use as rocket fuel. The reaction produces the gases carbon dioxide (CO2), nitrogen (N2), and water vapor (H2O), which are ejected in the exhaust gases. In a controlled experiment, solid dimethylhydrazine was reacted with excess dinitrogen tetroxide, and the gases were collected in a closed balloon until a pressure of 2.50 atm and a temperature of 400.0 K were reached.(a) What are the partial pressures of CO2, N2, and H2O?(b) When the CO2 is removed by chemical reaction, what are the partial pressures of the remaining gases?