Calculate the pressure exerted by 1.0 mol of hydrogen at 0°C in a vessel with volume of 5.0 dm3 using: a. The ideal gas law b. The Van der Waals equation (for constants see Table 1C.3, Resource section, p. 869) C. The Dieterici equation (for formula, refer to table of EOS in slide no. 63) d. The virial EOS up to 2nd virial coefficient (use constant from Table 1C.1, p. 868)
Calculate the pressure exerted by 1.0 mol of hydrogen at 0°C in a vessel with volume of 5.0 dm3 using: a. The ideal gas law b. The Van der Waals equation (for constants see Table 1C.3, Resource section, p. 869) C. The Dieterici equation (for formula, refer to table of EOS in slide no. 63) d. The virial EOS up to 2nd virial coefficient (use constant from Table 1C.1, p. 868)
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter6: The Gaseous State
Section: Chapter Questions
Problem 6.18QE
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Question
Answer only letter c and d.
Equation in letter c is provided in the picture.
Reference: Atkins' Physical Chemistry 11th ed.
Transcribed Image Text:Calculate the pressure exerted by 1.0 mol of hydrogen at 0°C in a vessel with volume of 5.0 dm³
using:
a. The ideal gas law
b. The Van der Waals equation (for constants see Table 1C.3, Resource section, p. 869)
C.
The Dieterici equation (for formula, refer to table of EOS in slide no. 63)
d. The virial EOS up to 2nd virial coefficient (use constant from Table 1C.1, p. 868)
Transcribed Image Text:1C Real gases 25
Table 1C.4 Selected equations of state
Critical constants
Equation
Reduced form
Pe
V.
T.
Perfect gas
nRT
p=v
nRT
p=
n'a
V-nb
8T
3
8a
van der Waals
P.= 3V, –1 V
36
27b?
27BR
nRT
n'a
P=V-nb
1( 2aR
8T,
P. =
3V, –1¯ T,V
3
2a
Berthelot
36
TV?
3b
3bR
nRTea RTV
V– nb
a
a
Dieterici
P. =
2V, – 1
4e'b²
2b
46R
nRT
1+
n'C(T)
Virial
+
* Reduced variables are defined as X, = X/X, with X= p, V and T. Equations of state are sometimes expressed in terms of the molar volume, V = V/n.
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