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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)

Physical Chemistry
Physical Chemistry
2nd Edition
ISBN:9781133958437
Author:Ball, David W. (david Warren), BAER, Tomas
Publisher:Ball, David W. (david Warren), BAER, Tomas
Chapter1: Gases And The Zeroth Law Of Thermodynamics
Section: Chapter Questions
Problem 1.55E: The Berthelot equation of state for one mole of gas is p=RTV-b-aTV2 Where a and b are constants...
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Answer only letter c and d. Equation in letter c is provided in the picture. Reference: Atkins' Physical Chemistry 11th ed.
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: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)
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.
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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