Concept explainers
Interpretation:
The number in metric tons (t) should be calculated for each gas emitted per year.
Concept Introduction:
Where,
P = Pressure
V = Volume
n = Number of moles
R = Universal gas constant
T = Temperature
Rearrange the above formula in terms of number of moles:
Number of moles is defined as the ratio of mass to the molar mass.
The mathematical expression is given as:
Mole fraction is defined as the ratio of number of moles of a gas to the total number of moles of gas.
The mathematical expression is given as:
Answer to Problem 5.92P
Mass of
Mass of
Mass of
Mass of
Mass of
Mass of
Mass of
Mass of
Explanation of Solution
Given information:
Hawaiian volcano Kilauea emits an average of
Temperature = 298 K
Pressure = 1.00 atm
Mole fractions: 0.4896
The number of moles is calculated as:
Volume in L =
Put the values,
=
Now, number of moles of carbon dioxide is calculated as:
=
Molar mass of
Molar mass of
Mass of
=
=
Since, 1 kg = 0.001 ton
Thus,
Mass of
=
Mass of
= 481.8 tons per year
Number of moles of
=
Molar mass of
Molar mass of
Mass of
=
=
Since, 1 kg = 0.001 ton
Thus,
Mass of
=
Mass of
= 9.136 tons per year
Number of moles of
=
Molar mass of
Molar mass of
Mass of
=
=
Since, 1 kg = 0.001 ton
Thus,
Mass of
=
Mass of
= 149.285 tons per year
Number of moles of
=
Molar mass of
Molar mass of
Mass of
=
=
Since, 1 kg = 0.001 ton
Thus,
Mass of
=
Mass of
= 169.85 tons per year
Number of moles of
=
Molar mass of
Molar mass of
Mass of
=
=
Since, 1 kg = 0.001 ton
Thus,
Mass of
=
Mass of
= 0.43 tons per year
Number of moles of
=
Molar mass of
Molar mass of
Mass of
=
=
Since, 1 kg = 0.001 ton
Thus,
Mass of
=
Mass of
= 0.212 tons per year
Number of moles of
=
Molar mass of
Molar mass of
Mass of
=
=
Since, 1 kg = 0.001 ton
Thus,
Mass of
=
Mass of
= 0.652 tons per year
Number of moles of
=
Molar mass of
Molar mass of
Mass of
=
=
Since, 1 kg = 0.001 ton
Thus,
Mass of
=
Mass of
= 0.229 tons per year
Want to see more full solutions like this?
Chapter 5 Solutions
Principles of General Chemistry
- Given that a sample of air is made up of nitrogen, oxygen, and argon in the mole fractions 0.78 N2, 0.21 O2, and 0.010 Ar, what is the density of air at standard temperature and pressure?arrow_forwardperform stoichiometric ca1cu1uions for reactions involving gases as reactants or products.arrow_forwardThe density of air 20 km above Earths surface is 92 g/m3. The pressure of the atmosphere is 42 mm Hg, and the temperature is 63 C. (a) What is the average molar mass of the atmosphere at this altitude? (b) If the atmosphere at this altitude consists of only O2 and N2, what is the mole fraction of each gas?arrow_forward
- A sample of a smoke stack emission was collected into a 1.25-L tank at 752 mm Hg and analyzed. The analysis showed 92% CO2, 3.6% NO, 1.2% SO2, and 4.1% H2O by mass. What is the partial pressure exerted by each gas?arrow_forwardIn the anaerobic oxidation of glucose by yeast, CO2 is produced: If 1.56 L of CO2 were produced at 22.0 C and 0.965 atm, what mass of C6H12O6 is consumed by the yeast? Assume the ideal gas law applied.arrow_forwardYou have an equimolar mixture of the gases SO2 and O2, along with some He, in a container fitted with a piston. The density of this mixture at STP is 1.924 g/L. Assume ideal behavior and constant temperature and pressure. a. What is the mole fraction of He in the original mixture? b. The SO2 and O2 react to completion to form SO3. What is the density of the gas mixture after the reaction is complete?arrow_forward
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning