Concept explainers
(a)
Interpretation:
The trend in diffusion constant under given conditions is to be predicted.
Concept introduction:
The diffusion of any gas particle among its own gas particles is known as self-diffusion. The diffusion constant is directly proportional to the product of mean free path and average velocity. The self-diffusion of a particle is given as,
Where,
•
•
•
•
•
•
(b)
Interpretation:
The trend in diffusion constant under given conditions is to be predicted.
Concept introduction:
The diffusion any gas particle among its own gas particles is known as self-diffusion. The diffusion constant is directly proportional to the product of mean free path and average velocity. The self-diffusion of a particle is given as,
Where,
•
•
•
•
•
•
(c)
Interpretation:
The trend in diffusion constant under given conditions is to be predicted.
Concept introduction:
The diffusion any gas particle among its own gas particles is known as self-diffusion. The diffusion constant is directly proportional to the product of mean free path and average velocity. The self-diffusion of a particle is given as,
Where,
•
•
•
•
•
•
(d)
Interpretation:
The trend in diffusion constant under given conditions is to be predicted.
Concept introduction:
The diffusion any gas particle among its own gas particles is known as self-diffusion. The diffusion constant is directly proportional to the product of mean free path and average velocity. The self-diffusion of a particle is given as,
Where,
•
•
•
•
•
•
Want to see the full answer?
Check out a sample textbook solutionChapter 19 Solutions
Physical Chemistry
- A flask at room temperature contains equal numbers of di-nitrogen molecules and krypton atoms. (a) Which of the two gases exerts the higher partial pressure? (b) Which gas has a higher kinetic energy per molecule/atom? (c) Which gas has molecules with a higher velocity? Explain your answers.arrow_forwardDescribe what happens to the average kinetic energy of ideal gas molecules when the conditions are changed as follows:(a) The pressure of the gas is increased by reducing the volume at constant temperature.(b) The pressure of the gas is increased by increasing the temperature at constant volume.(c) The average velocity of the molecules is increased by a factor of 2.arrow_forwardQ6. (a)The vander waals equation is used to describe the behaviour of real gases but still not so useful in many industrial applications. Explain why?(3) (b)In kinetic molecular theory of gases it is assumed that The molecules of the gases occupy negligible volume as compared to the total volume of the gas' which factor can be actually described by this postulate?(2)arrow_forward
- (5) Using the data in Table 1C.3 (from the textbook), calculate the pressure that 2.500 moles of carbon dioxide confined in a volume of 1.000 L at 450 K exerts. Compare the pressure with that calculated assuming ideal-gas behavior.arrow_forwardQ1.A glass vessel was filled with an unknown quantity of nitrogen gas and the pressure at 28°C was 4.2 x 10⁴Pa. Oxygen gas was introduced at the same temperature until the pressure was to 1.013 ×10⁵Pa. (I) calculate the partial pressures of nitrogen gas and oxygen gas (II) calculate the mass ratio of the two gases. ( N=14, O=16) Q2. When temperature is increased by 10K, what happens to the rate of reaction? Why is it so?arrow_forwardWhat is the effect of the following on the volume of 1 mol of an ideal gas?(a) The pressure is reduced by a factor of 4 (at constant T).(b) The pressure changes from 760 torr to 202 kPa, and the temperature changes from 37°C to 155 K.(c) The temperature changes from 305 K to 32°C, and the pressure changes from 2 atm to 101 kPa.arrow_forward
- (a) A rigid tank contains 1.60 moles of helium, which can be treated as an ideal gas, at a pressure of 28.0 atm. While the tank and gas maintain a constant volume and temperature, a number of moles are removed from the tank, reducing the pressure to 5.00 atm. How many moles are removed? mol (b) What If? In a separate experiment beginning from the same initial conditions, including a temperature T, of 25.0°C, half the number of moles found in part (a) are withdrawn while the temperature is allowed to vary and the pressure undergoes the same change from 28.0 atm to 5.00 atm. What is the final temperature (in °C) of the gas? °Carrow_forwardWhen a large evacuated flask is filled with argon gas, its massincreases by 3.224 g. When the same flask is again evacuatedand then filled with a gas of unknown molar mass, the massincrease is 8.102 g. (a) Based on the molar mass of argon,estimate the molar mass of the unknown gas. (b) What assumptionsdid you make in arriving at your answer?arrow_forwardSamples of F2 gas and Xe gas are mixed in a container of fixed volume. The initial partial pressure of the F2 gas is 8.0 atmospheres and that of the Xe gas is 1.7 atmospheres. When all of the Xe gas reacted, forming a solid compound, the pressure of the unreacted F2 gas was 4.6 atmospheres. The temperature remained constant. What is the formula of the compound? (A) XeF (B) XeF3 (C) XeF4 (D) XeF6 (E) XeF8arrow_forward
- 7. You are given two samples of gas at identical P, T, and V, all near room temperature. Gas A is monatomic and gas B is diatomic. Both gas A and gas B have the same molar mass. (a) In which gas do the particles have a greater speed? (b) In which gas do the particles have more kinetic energy? (c) The temperature of each gas is increased by 8. The particles in which gas now have a greater average speed? A greater change in internal energy?arrow_forwardSection 1.2 P1.1 Devise a temperature scale, abbreviated G, for which the magnitude of the ideal gas constant is 7.41J G¹ mol-¹.arrow_forwardAn alternate way to state Avogadro’s law is “All other things being equal, the number of molecules in a gas is directly proportional to the volume of the gas.” (a) What is the meaning of the term “directly proportional?” (b) What are the “other things” that must be equal?arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY