Concept explainers
(a)
Interpretation: The increasing order of effusion rate for the mixture of disulfur difluoride, dinitrogen tetrafluoride and sulfur tetrafluoride gases placed in an effusion apparatus needs to be determined.
Concept Introduction:
Graham's Law of effusion of gases states that at same conditions, the effusion rate of two gases vary inversely with the square roots of molar masses of the gases. The mathematical expression for the Graham’s law for two gases ‘a’ and ‘b’ can be written as:
(a)
Answer to Problem 5.63P
The rate of effusion of gases must be:
Explanation of Solution
As the molar mass increases, the rate of effusion decreases. The molar mass of gases are:
- Disulfur difluoride = 102.13 g/mol
- Dinitrogen tetrafluoride =104.00 g/mol
- Sulfur tetrafluoride = 108.07 g/mol
Hence, the rate of effusion of gases must be:
(b)
Interpretation: The ratio of effusion rate of gases disulfur difluoride and dinitrogen tetrafluoride is placed in an effusion apparatus needs to be determined.
Concept Introduction:
Graham's Law of effusion of gases states that at same conditions, the effusion rate of two gases vary inversely with the square roots of molar masses of the gases. The mathematical expression for the Graham’s law for two gases ‘a’ and ‘b’ can be written as:
(b)
Answer to Problem 5.63P
Explanation of Solution
Graham's Law of effusion of gases states that at the same conditions the rate of effusion of two different gases are inversely proportional to the square roots of their molar masses. The mathematical expression for the Graham’s law for two gases ‘a’ and ‘b’ can be written as:
As the molar mass increases, the rate of effusion decreases. The molar mass of gases are:
- Disulfur difluoride = 102.13 g/mol
- Dinitrogen tetrafluoride = 104.00 g/mol
Substitute the values of molar mass to calculate the rate of effusion:
(c)
Interpretation: The molar mass of X gas that is added to gas mixture and effuses at 0.935 times at the rate of
Concept Introduction:
Graham's Law of effusion of gases states that at same conditions, the effusion rate of two gases vary inversely with the square roots of molar masses of the gases. The mathematical expression for the Graham’s law for two gases ‘a’ and ‘b’ can be written as:
(c)
Answer to Problem 5.63P
Explanation of Solution
As the molar mass increases, the rate of effusion decreases. The molar mass of gas:
- Sulfur tetrafluoride = 108.07 g/mol
Substitute the values to calculate the molar mass:
Thus, molar mass of unknown gas is 123.6 g/mol.
Want to see more full solutions like this?
Chapter 5 Solutions
Principles of General Chemistry
- perform stoichiometric ca1cu1uions for reactions involving gases as reactants or products.arrow_forward5-114 Carbon dioxide gas, saturated with water vapor, can be produced by the addition of aqueous acid to calcium carbonate based on the following balanced net ionic equation: (a) How many moles of wet CO (g), collected at 60.°C and 774 torr total pressure, are produced by the complete reaction of 10.0 g of CaCO3 with excess acid? (b) What volume does this wet CO2 occupy? (c) What volume would the CO2 occupy at 774 torr if a desiccant (a chemical drying agent) were added to remove the water? The vapor pressure of water at 60.°C is 149.4 mm Hg.arrow_forward47 HCl(g) reacts with ammonia gas, NH3(g), to form solid ammonium chloride. If a sample of ammonia occupying 250 mL at 21 C and a pressure of 140 torr is allowed to react with excess HCl, what mass of NH4Cl will form?arrow_forward
- Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning