The ideal gas law describes the relationship among the volume of an ideal gas (V), its pressure (P), its absolute temperature (T), and number of moles ( n): PV = nRT Under standard conditions, the ideal gas law does a good job of approximating these properties for any gas. However, the ideal gas law does not account for all the properties of real gases such as intermolecular attraction and molecular volume, which become more pronounced at low temperatures and high pressures. The van der Waals equation corrects for these factors with the constants a and b, which are unique to each substance: (P+ ²) (V- nb) =nRT The gas constant R is equal to 0.08206 L-atm/(K-mol). A 3.00-1 flask is filled with gaseous ammonia, NH3. The gas pressure measured at 16.0 °C is 2.45 atm . Assuming ideal gas behavior, how many grams of ammonia are in the flask? Express your answer to three significant figures and include the appropriate units. ▸ View Available Hint(s) ▼ mass of NH3 = Submit Part B O HA Pideal-Preal = Value Ideal versus real behavior for gases In the following part you can see how the behavior of real gases deviates from the ideal behavior. You will calculate the pressure values for a gas using the ideal gas law and also the van der Waals equation. Take note of how they differ. 3 HA Units If 1.00 mol of argon is placed in a 0.500-L container at 19.0 °C, what is the difference between the ideal pressure (as predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation)? For argon, a = 1.345 (L² atm)/mol2 and b =0.03219 L/mol. Express your answer to two significant figures and include the appropriate units. View Available Hint(s) Value ? PE ? Units
The ideal gas law describes the relationship among the volume of an ideal gas (V), its pressure (P), its absolute temperature (T), and number of moles ( n): PV = nRT Under standard conditions, the ideal gas law does a good job of approximating these properties for any gas. However, the ideal gas law does not account for all the properties of real gases such as intermolecular attraction and molecular volume, which become more pronounced at low temperatures and high pressures. The van der Waals equation corrects for these factors with the constants a and b, which are unique to each substance: (P+ ²) (V- nb) =nRT The gas constant R is equal to 0.08206 L-atm/(K-mol). A 3.00-1 flask is filled with gaseous ammonia, NH3. The gas pressure measured at 16.0 °C is 2.45 atm . Assuming ideal gas behavior, how many grams of ammonia are in the flask? Express your answer to three significant figures and include the appropriate units. ▸ View Available Hint(s) ▼ mass of NH3 = Submit Part B O HA Pideal-Preal = Value Ideal versus real behavior for gases In the following part you can see how the behavior of real gases deviates from the ideal behavior. You will calculate the pressure values for a gas using the ideal gas law and also the van der Waals equation. Take note of how they differ. 3 HA Units If 1.00 mol of argon is placed in a 0.500-L container at 19.0 °C, what is the difference between the ideal pressure (as predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation)? For argon, a = 1.345 (L² atm)/mol2 and b =0.03219 L/mol. Express your answer to two significant figures and include the appropriate units. View Available Hint(s) Value ? PE ? Units
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Question
![The ideal gas law describes the relationship among
the volume of an ideal gas (V), its pressure (P), its
absolute temperature (T), and number of moles (
n):
PV = nRT
Under standard conditions, the ideal gas law does
a good job of approximating these properties for
any gas. However, the ideal gas law does not
account for all the properties of real gases such as
intermolecular attraction and molecular volume,
which become more pronounced at low
temperatures and high pressures. The van der
Waals equation corrects for these factors with the
constants a and b, which are unique to each
substance:
(P+ ²) (V-nb) = nRT
an²
The gas constant R is equal to 0.08206
L.atm/(K-mol).
Part A
A 3.00-L flask is filled with gaseous ammonia, NH3. The gas pressure measured at 16.0 °C is 2.45 atm . Assuming
ideal gas behavior, how many grams of ammonia are in the flask?
Express your answer to three significant figures and include the appropriate units.
View Available Hint(s)
mass of NH3 =
Submit
▾ Part B
HÅ
Value
Pideal-Preal =
3
Ideal versus real behavior for gases
In the following part you can see how the behavior of real gases deviates from the ideal behavior. You will calculate the
pressure values for a gas using the ideal gas law and also the van der Waals equation. Take note of how they differ.
Units
If 1.00 mol of argon is placed in a 0.500-L container at 19.0 °C, what is the difference between the ideal pressure (as
predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation)? For argon,
a = 1.345 (L² atm)/mol2 and b=0.03219 L/mol.
Express your answer to two significant figures and include the appropriate units.
View Available Hint(s)
L
i HA 1
Value
?
Units
?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4d09ffa2-b6c2-4e97-915d-74d176d987ab%2Fa6325a9c-8282-4a27-99ce-5fdc0f12e11d%2Fkito7cp_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The ideal gas law describes the relationship among
the volume of an ideal gas (V), its pressure (P), its
absolute temperature (T), and number of moles (
n):
PV = nRT
Under standard conditions, the ideal gas law does
a good job of approximating these properties for
any gas. However, the ideal gas law does not
account for all the properties of real gases such as
intermolecular attraction and molecular volume,
which become more pronounced at low
temperatures and high pressures. The van der
Waals equation corrects for these factors with the
constants a and b, which are unique to each
substance:
(P+ ²) (V-nb) = nRT
an²
The gas constant R is equal to 0.08206
L.atm/(K-mol).
Part A
A 3.00-L flask is filled with gaseous ammonia, NH3. The gas pressure measured at 16.0 °C is 2.45 atm . Assuming
ideal gas behavior, how many grams of ammonia are in the flask?
Express your answer to three significant figures and include the appropriate units.
View Available Hint(s)
mass of NH3 =
Submit
▾ Part B
HÅ
Value
Pideal-Preal =
3
Ideal versus real behavior for gases
In the following part you can see how the behavior of real gases deviates from the ideal behavior. You will calculate the
pressure values for a gas using the ideal gas law and also the van der Waals equation. Take note of how they differ.
Units
If 1.00 mol of argon is placed in a 0.500-L container at 19.0 °C, what is the difference between the ideal pressure (as
predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation)? For argon,
a = 1.345 (L² atm)/mol2 and b=0.03219 L/mol.
Express your answer to two significant figures and include the appropriate units.
View Available Hint(s)
L
i HA 1
Value
?
Units
?
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