Skip to main content
Ch.10 - Gases
Brown - Chemistry: The Central Science 15th Edition
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 15th EditionCh.10 - GasesProblema 98a
Capitolo 10, Problema 98a

Carbon dioxide, which is recognized as the major contributor to global warming as a “greenhouse gas,” is formed when fossil fuels are combusted, as in electrical power plants fueled by coal, oil, or natural gas. One potential way to reduce the amount of CO2 added to the atmosphere is to store it as a compressed gas in underground formations. Consider a 1000-megawatt coal-fired power plant that produces about 6×106 tons of CO2 per year. a. Assuming ideal-gas behavior, 1.00 atm, and 27°C, calculate the volume of CO2 produced by this power plant.

Guida verificata passo dopo passo
1
Convert the temperature from degrees Celsius to Kelvin by adding 273.15 to the Celsius temperature: \( T(K) = 27 + 273.15 \).
Use the ideal gas law equation \( PV = nRT \) to find the volume \( V \). Rearrange the equation to solve for \( V \): \( V = \frac{nRT}{P} \).
Calculate the number of moles \( n \) of CO2 using the given mass and the molar mass of CO2 (approximately 44.01 g/mol). First, convert the mass from tons to grams, then use \( n = \frac{\text{mass in grams}}{\text{molar mass}} \).
Substitute the values into the ideal gas law equation: \( P = 1.00 \text{ atm} \), \( R = 0.0821 \text{ L atm/mol K} \), \( T \) in Kelvin, and \( n \) calculated in the previous step.
Calculate the volume \( V \) in liters, which will give you the volume of CO2 produced by the power plant under the given conditions.

Risposta video verificata per un problema simile:

Questa soluzione video è stata consigliata dai nostri tutor come utile per risolvere questo problema.
Durata del video:
7m

Concetti chiave

Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.

Ideal Gas Law

The Ideal Gas Law is a fundamental equation in chemistry that relates the pressure, volume, temperature, and number of moles of a gas. It is expressed as PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature in Kelvin. This law allows us to predict the behavior of gases under various conditions, making it essential for calculating the volume of gases like CO2 produced in combustion processes.
Video consigliato:
Percorso guidato
01:15
Ideal Gas Law Formula

Molar Volume of a Gas

The molar volume of a gas is the volume occupied by one mole of an ideal gas at standard temperature and pressure (STP), which is 0°C and 1 atm. At these conditions, the molar volume is approximately 22.4 liters. However, in this question, we are dealing with different conditions (27°C and 1 atm), so we must adjust our calculations using the Ideal Gas Law to find the volume of CO2 produced by the power plant.
Video consigliato:
Percorso guidato
00:51
The Ideal Gas Law: Molar Mass

Combustion of Fossil Fuels

The combustion of fossil fuels involves a chemical reaction where hydrocarbons react with oxygen to produce carbon dioxide and water, releasing energy. This process is a significant source of CO2 emissions, contributing to global warming. Understanding the amount of CO2 produced by such processes is crucial for developing strategies to mitigate climate change, such as carbon capture and storage.
Video consigliato:
Percorso guidato
02:24
Combustion Apparatus
Pratica correlata
Domanda del libro di testo

Assume that a single cylinder of an automobile engine has a volume of 524 cm3. a. If the cylinder is full of air at 74°C and 0.980 atm, how many moles of O2 are present? (The mole fraction of O2 in dry air is 0.2095.)

1
views
Domanda del libro di testo

A gas bubble with a volume of 1.0 mm3 originates at the bottom of a lake where the pressure is 3.0 atm. Calculate its volume when the bubble reaches the surface of the lake where the pressure is 730 torr, assuming that the temperature does not change.

691
views
Domanda del libro di testo

Nickel carbonyl, Ni(CO)4, is one of the most toxic substances known. The present maximum allowable concentration in laboratory air during an 8-h workday is 1 ppb (parts per billion) by volume, which means that there is one mole of Ni(CO)4 for every 109 moles of gas. Assume 24°C and 1.00 atm pressure. What mass of Ni(CO)4 is allowable in a laboratory room that is 12ft×20ft×9ft?

Domanda del libro di testo

Table 10.3 shows that the van der Waals b parameter has units of L/mol. This means that we can calculate the sizes of atoms or molecules from the b parameter. Refer back to the discussion in Section 7.3. Is the van der Waals radius we calculate from the b parameter of Table 10.3 more closely associated with the bonding or nonbonding atomic radius discussed there? Explain.

1152
views
Domanda del libro di testo

Consider the arrangement of bulbs shown in the drawing. Each of the bulbs contains a gas at the pressure shown. What is the pressure of the system when all the stopcocks are opened, assuming that the temperature remains constant? (We can neglect the volume of the capillary tubing connecting the bulbs.)

1529
views