(a) Derive, given that dU = dq+ dw, andconsidering that dU is an exact differential, ageneral relation between Cy and Cp.(b) Consequently, assume ideal gas behaviourand simplify your result.

Given a system:dU=δQ+δW where:dU is the differential change in internal energy UδQ is the…

Answered: (a) Derive, given that dU = dq+ dw, and…

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter2: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 2.56E: What are the numerical values of the heat capacities c-v and c-p of a monatomic ideal gas,in units...

See similar textbooks

Similar questions

Determine an expression for V/T p, n in terms of and . Does the sign on the expression make sense in terms of what you know happens to volume as temperature changes?
Derive the fact that HpT is also zero for an ideal gas.
Show that = T/p for an ideal gas.
Use the ideal gas law to demonstrate the cyclic rule of partial derivatives.
(*), (*): P Use the Euler and reciprocal relations to show that it is equivalent to Cp - Cy = T Ср - Cv = −T. Сү = -Т. Әр ат av 2 T (1) (2) Use this expression to evaluate Cр - Cv for (1) an ideal gas, and (2) for a van der Waals gas.
Calculate the work done by a gas w hen it expandsthrough (a) 1.0 cm3, (b) 1.0 dm3 against an atmospheric pressure of 100 kPa . What work must be done to compress thegas back to original state in each case?
A sample of Ar of mass 8.30 g occupies 1.75dm3 at 330 K. (a) Calculate the work done when the gas expands isothermally against a constant external pressure of 1 bar until itsvolume has increased by 0.35 dm3 (b) Calculate the work that would be done if thesame expansion occurred reversibly
(7) Combustion of CH4 and H₂. For 100 g mol of a gas mixture of 75 mol % CH4 and 25 mol % H₂, calculate the total heat of combustion of the mixture at 298 K and 101.32 kPa, assuming that combustion is complete.
3. Assume that the van der Waal's "b" Parameter be ignored. Delive an (a) can equation for the work done in Isothermal, reversible expansion of this goed. (b) is the work done an the surroundings ideal gas More or less than an expansion ?
7:53 PM Mon Nov 21 8) A sample of 1 mol of perfect gas at 298 K and 1 bar with Cvm = 3/2 R and Cp.m= 5/2 R is put through the following cycle: (a) constant-volume heating to twice its initial pressure, (b) reversible, adiabatic expansion back to its initial temperature, (c) reversible, isothermal compression back to 1 bar. Calculate q, w, AU, and AH for each step, as well as any necessary variables (e.g. V₁, T, etc.) n=1 mol T= 298 K P= I bar Cum 3R - 2 Cp.m-2R T b) a) w=0 n=1 T= 298 K Cvm = 3R 2 AP= 1 bar 9,² AU= ΔΗ: PV = nRT V = nRT @87% 8
(a) How much work is required to compress 4.99 mol of air at 20.4°C and 1.00 atm to one-tenth of the original volume by an isothermal process? (b) How much work is required to produce the same compression in an adiabatic process? (c) What is the final pressure in part (a)? (d) What is the final pressure in part (b)?
4.44. Show that a (a), - = 1 where a is the expansion coefficient and K is the isothermal compressibility.

SEE MORE QUESTIONS

Recommended textbooks for you

Physical Chemistry

Chemistry

ISBN:

9781133958437

Author:

Ball, David W. (david Warren), BAER, Tomas

Publisher:

Wadsworth Cengage Learning,

Physical Chemistry

Chemistry

ISBN:

9781133958437

Author:

Ball, David W. (david Warren), BAER, Tomas

Publisher:

Wadsworth Cengage Learning,

SEE MORE TEXTBOOKS

(a) Derive, given that dU = dq+ dw, and considering that dU is an exact differential, a general relation between Cy and Cp. (b) Consequently, assume ideal gas behaviour and simplify your result.