Thermodynamics, Statistical Thermodynamics, & Kinetics
3rd Edition
ISBN: 9780321766182
Author: Thomas Engel, Philip Reid
Publisher: Prentice Hall
expand_more
expand_more
format_list_bulleted
Question
Chapter 3, Problem 3.19NP
Interpretation Introduction
Interpretation:The expression for the internal pressure of a gas that obeys the Bethelot equation of state is to be derived.
Concept introduction:The van der Waals equation can be defined as the types of the equation that corrects the two properties of the real gas. The van der Waals equation is the modified version of the ideal gas equation while the Bethelot equation is the modified version of the van der Waals equation.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Estimate the internal pressure of sulfur dioxide at 1.00 bar and 298 K, treating it as a van der Waals gas, when πT = a/Vm2. You may simplify the problem by assuming that the molar volume can be predicted from the perfect gas equation.
One of the more commonly used compressed gases is nitrogen (N2), often in large metal cylinders.
If a cylinder holds 711 mol of N2 when pressurised to 5.3 x 104 kPa at T = 20oC, how many litres is its capacity?
The equation of state of a certain gas is given by p = RT/Vm + (a + bT)/Vm2, where a and b are constants. Find (∂Vm/∂T)p.
Chapter 3 Solutions
Thermodynamics, Statistical Thermodynamics, & Kinetics
Ch. 3 - Prob. 3.1CPCh. 3 - Prob. 3.2CPCh. 3 - Prob. 3.3CPCh. 3 - Prob. 3.4CPCh. 3 - Why can qv be equated with a state function if q...Ch. 3 - Prob. 3.6CPCh. 3 - Prob. 3.7CPCh. 3 - Prob. 3.8CPCh. 3 - Prob. 3.9CPCh. 3 - Why is qv=U only for a constant volume process? Is...
Ch. 3 - Prob. 3.11CPCh. 3 - Why are q and w not state functions?Ch. 3 - Prob. 3.13CPCh. 3 - What is the relationship between a state function...Ch. 3 - Prob. 3.15CPCh. 3 - Is the following statement always, never, or...Ch. 3 - Is the following statement always, never, or...Ch. 3 - Prob. 3.18CPCh. 3 - Prob. 3.19CPCh. 3 - Is the expression UV=T2T1CVdT=nT1T2CV,mdT only...Ch. 3 - Prob. 3.1NPCh. 3 - Prob. 3.2NPCh. 3 - Prob. 3.3NPCh. 3 - Prob. 3.4NPCh. 3 - Prob. 3.5NPCh. 3 - Prob. 3.6NPCh. 3 - Integrate the expression =1/VV/TP assuming that ...Ch. 3 - Prob. 3.8NPCh. 3 - Prob. 3.9NPCh. 3 - Prob. 3.10NPCh. 3 - Prob. 3.11NPCh. 3 - Calculate w, q, H, and U for the process in which...Ch. 3 - Prob. 3.13NPCh. 3 - Prob. 3.14NPCh. 3 - Prob. 3.15NPCh. 3 - Prob. 3.16NPCh. 3 - Prob. 3.17NPCh. 3 - Prob. 3.18NPCh. 3 - Prob. 3.19NPCh. 3 - Prob. 3.20NPCh. 3 - Prob. 3.21NPCh. 3 - Prob. 3.22NPCh. 3 - Derive the following relation, UVmT=3a2TVmVm+b for...Ch. 3 - Prob. 3.24NPCh. 3 - Prob. 3.25NPCh. 3 - Prob. 3.26NPCh. 3 - Prob. 3.27NPCh. 3 - Prob. 3.28NPCh. 3 - Prob. 3.29NPCh. 3 - Prob. 3.30NPCh. 3 - Prob. 3.31NPCh. 3 - Prob. 3.32NPCh. 3 - Prob. 3.33NPCh. 3 - Prob. 3.34NPCh. 3 - Derive the equation H/TV=CV+V/k from basic...Ch. 3 - Prob. 3.36NPCh. 3 - Prob. 3.37NPCh. 3 - Show that CVVT=T2PT2VCh. 3 - Prob. 3.39NP
Knowledge Booster
Similar questions
- Estimate the internal pressure of water vapour at 1.00 bar and 400 K, treating it as a van der Waals gas, when πT = a/Vm2. You may simplify the problem by assuming that the molar volume can be predicted from the perfect gas equation.arrow_forwardP2D.2 Starting from the expression Cp − CV = T(∂p/∂T)V(∂V/∂T)p, use theappropriate relations between partial derivatives (The chemist’s toolkit 9 inTopic 2A) to show thatC CT V TV p( / )( / ) p VpT2− = ∂ ∂∂ ∂ Use this expression to evaluate Cp − CV for a perfect gas.arrow_forward13. (a) ] Determine the reduced temperature, reduced pressure and reduced molar volume of a sample of argon with a molar volume of 4.518 L at 10.0°C and 3.00 bar pressure. For Ar, T=150.86 K, Vc = 74.57 x 10-³ L, P = 48.98 bar (b) [ Calculate the P and I values for which NH3 is in a corresponding state with Ar. For NH3, Tc=405.40 K, Pc = 113.53 bararrow_forward
- Rearrange the van der Waals equation of state, p = nRT/(V − nb) − n2a/V2(Topic 1C) to give an expression for T as a function of p and V (with n constant). Calculate (∂T/∂p)V and confirm that (∂T/∂p)V = 1/(∂p/∂T)V.arrow_forwardCp− ̄Cv=T ̄V β^2/κ reduces to ̄CP− ̄CV=R for an ideal gas.arrow_forwardCalculate the pressure exerted by 1.0 mol C2H6 behaving as a van der Waals gas when it is confined under the following conditions: (i) at 273.15 K in 22.414 dm3, (ii) at 1000 K in 100 cm3. Use the data in Table 1C.3 of the Resource section.arrow_forward
- where a and b are constants. Find V RT a+bT 2) The equation of state of a certain gas is given by p : aV Vm ),arrow_forwardA certain gas obey's the following equation of state: RT P = V – b V²T a Write the constants a andb in terms of the critical P V. and T?arrow_forwardDetermine the partial molar volume of a component of a gas mixture based on the provided equation of state. When PV (1 – bP) = n2RT, the constant b is taken into consideration.arrow_forward
- The Boyle temperature of a gas is defined to be the temperature at which the second virial coefficient in the inverse volume expansion vanishes. A certain gas obeys the equation of state RT a Р- Vm – b T³V - m where a and b are numerical constants. Expand the equation of state in virial form, and determine the Boyle temperature of the gas in terms of a, b and R.arrow_forward(a) For an ideal gas equation of state, prove that P P P dP = dn +=dT dv n (b) Suppose 1.000 mol of ideal gas at 300.0 K in a 30.00 L vessel increased in volume by 0.050 L. Use your answer from part (a) to compute the change in the pressure AP. (c) Compare to the exact change in pressure using the ideal gas equation of state to the estimate given by AP.arrow_forward1C.5 The virial equation of state may also be written as an expansion in terms of pressure: Z= 1 + B'p+ ... The critical constants for water, H,0, are 218.3 atm, 55.3 cm³ mol-1 and 647.4 K. Assuming that the expansion may be truncated after the second term, calculate the value of the second virial coef- ficient B'at the critical temperature. %3Darrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning