2. (a) H2O (g) obeys the truncated viral equation of state given below at 400 K and up to 100 bar pressure.nRT n°RTB(T)P =VCalculate the amount of work done as 2.00 mol of H2O (g) expands reversibly and isothermally from 2.00to 50.0 dm³ at 400 K with B(T) = B(400 K) =-356 cm³ mol.(b) An ideal gas is expanded reversibly and isothermally. Decide which of q, w, AU, and AH are 0, positive,or negative.

The gas equation pertains to the ideal gas molecules is that relates pressure (P), volume (V),…

Answered: 2. (a) H2O (g) obeys the truncated…

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...

See similar textbooks

Similar questions

The enthalpy increase of N; when heated between 300 and 1500 does not exceed 100 kl/mol. The final temperature when a CO: gas at 298.15 K undergoes a reversible adiabatic expansion from 500 cm' to 2 dm' exceeds 210 K. The isothermal compressibility for the equation of state, P(V-b) = RT, differs from that of a perfect gas by b/PV. The quantity of work obtained in a reversible isothermal (400 K) vs. isobaric (10 atm) process upon compression of C,He from 1.2 to 0.1 L/mol differ by more than 4.5 ki/mol. The change in the internal energy of system if the surrounding gain 2501 of heat and if 470 J of work is performed by the surrounding exceeds 720 J
Ammonia (an ideal gas) is containted in a 1.5 cubic meter piston. Initially it is 200 kPa, 20C but it is compressed to 40C (at a constant pressure). During this process, 1500 kJ of heat is rejected to the 20C surrounding and 750 kJ of work is done Is this process possible?
(a) Calculate the final temperature of a sample of CO2 of mass 16.0 g that is expanded reversibly and adiabatically from 500 cm at 298.15 K to 2. 00 dm³ if Cp.m is equal to 37.11 J K' mol'. Tr=Ti (Vi/Vr)"C
Please provide detailed solution and give the explanation of the concept
Suppose a piece of solid lead weighing 41.3 g at a temperature of 312 °C is placed in 413 g of liquid lead at a temperature of 374 °C. Calculate the temperature after thermal equilibrium is reached, assuming no heat loss to the surroundings. The enthalpy of fusion of solid lead is AH fus = 4.77 kj mol¹ at its melting point of 328 °C, and the molar heat capacities cp of solid and liquid lead are 26.9 and 28.6 J K¹ mol-¹, respectively. (Enter your answer to three significant figures.) T₁= Jc Submit Answer Try Another Version 1 item attempt remaining
Q3) Thermodynamic Processes- 2.0 mol of a diatomic ideal gas undergoes a process in which it is compressed very slowly from state a (V. = 3.0 m³, P, = 1000 Pa) to state b (V, = 1.0 m³), in such a way that the system maintains thermal equilibrium with its surroundings at all times. P (Pa) 3000 2000 A. Find the change in internal energy during the process. 1000 B. Find the final pressure of the gas. 1 3 4 V(m³) C. Find the work done by the piston on the gas during this process. (Hint: Since Pis not constant during this process, it doesn't come out of the integral. Use the ideal gas law to find an expression for Pin terms of constants and the integration variable V) D. So what's the work done by the gas on the piston during this process? E. How much heat – if any - was transferred between the gas and surroundings during this process? Did heat flow from the gas to the surroundings or from the surroundings to the gas? Explain your reasoning. F. At the end of the process, is the average…
(a) Suppose that attractions are the dominant interaction between gas molecules, and the equation of state is p = nRT/V – n2a/V2. Determine the work (W(non-ideal gas)) of reversible, isothermal expansion of such a gas from initial volume V (initial) = 20.0 L to final volume V(final) = 40.0 L if n = 2.00 mol, T = 300 K, and a = 3.621 atm-L2/mol2. Watch your units. (b)Determine the work (W(ideal gas) of reversible, isothermal expansion of an ideal gas from initial volume V (initial) = 20.0 L to final volume V(final) = 40.0 L if n = 2.00 mol and T = 300 K. (c) Show the difference W(non-ideal) – W(ideal). If all your calculations are done correctly, this result shows you the effect of attractive interaction between gas particles on the work done by the system.
Compare DHm from (1) and (2) and comment.
(b) An ideal gas of 2.5 moles undergoes an adiabatic expansion at an initial pressure of 4.25 bar and at an initial temperature of 540 K to a final temperature of 400 K. Calculate the work done which is equal to internal energy change under such conditions. Assume Cp,m = 5/2 R %3D
2. A7.0 x 102 mol sample of Kr (g) expands reversibly and isothermally at 373 K from 5.25 mL to 6.29 mL and the internal energy of the sample is known to increase by 83.5 J. Use the virial equation of state up to the second coefficient (where Bx --28.7 mL/mol) to calculate w, q, and AH for this change. =
2. Calculate the work done by 2.00 mol of an ideal gas contained in a piston/cylinder assembly that expands isothermally at T=25°C) reversibly and irreversibly from 1.5 to 5 L. For the irreversible case, assume Pext = 9.9 bar.

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS