One mole of an ideal gas initially kept in a cylinder at pressure 1 MPa and temperature 27°C is made to expand until its volume is doubled. (a) How much work is done if the expansion is (i) adiabatic (ii) isobaric (iii) isothermal? (b) Identify the processes in which change in internal energy is least and is maximum. (c) Show each process on a PV diagram. (d) Name the processes in which the heat (Take y = 5/3 and R=8.3 J mol-1 K-1)

One mole of an ideal gas initially kept in a cylinder at pressure 1 MPa and temperature 27°C is made to expand until its volume is doubled. (a) How much work is done if the expansion is (i) adiabatic (ii) isobaric (iii) isothermal? (b) Identify the processes in which change in internal energy is least and is maximum. (c) Show each process on a PV diagram. (d) Name the processes in which the heat (Take y = 5/3 and R=8.3 J mol-1 K-1)

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

When 5.84 mols of 02 gas is heated at a constant pressure of 118. kPa, the temperature increases from 257. K to 292. K. Given the molar heat capacity of molecular oxygen at constant pressure is 29.4 J K1 mole -1, calculate the change of internal energy. AU = kJ Hint: Because H = U + PV, it follows that AH = AU + A(PV) or for and ideal gas AH = AU + A(nRT).
Half a mole of an ideal gas expands isothermally and reversibly at 273.15 K from a volume of 22 L to volume of 10 L. (i) What is the change in the entropy of the gas in J/K). (ii) How much work is done on the gas in (j) (iii) What is q surrounding in (j)
1. (a) In reaching equilibrium, how much heat transfer occurs from 1.2 kg of water at 40°C when it is placed in contact with 1.2 kg of 20°C water? Specific heat of water c=4186 J/(kg°C) Hint: If the masses of water are equal, what is the equilirium temperature of the water mixture? Q= ✓ J (b) What is the change in entropy due to this heat transfer? AS total ✔J/K (c) How much work is made unavailable, taking the lowest temperature to be 20°C? = W unavailable ✓ J
13. (a) How much heat wiH be evolved or absorbed in the solution of 2 moles of H,SO,(1) in a very large volume of water at 25°C? (b) What will be the dif- ferential heats of solution of the acid and the water under these conditions?
gas undergoes an adiabatic expansion from 10 − 3 m 3 to 8 × 10 − 3 m 3 . The adiabatic line for the gas is given by P 3 V 5 = C (C is a constant). (a) Calculate the reversible work performed along the adiabatic line if the initial pressure is 10 5 P a and the initial volume = 10 − 3 m 3 . (b) What is the value of the constant C ? What is the unit of C ? (c) The gas reaches the final state in a two step process. An expansion at a constant initial pressure to the final volume followed by a decrease in pressure to the final volume 8 × 10 − 3 m 3 . What is the reversible work and heat in this process?
4. Calculate the work done under isothermal conditions for 5.5 mols of an ideal gas expanding from 10.0 bar to 2.00 bar at –20.0°C both for a reversible (a) and irreversible (b) process. For the latter, Pext = 2.00 bar. The general expression for work is, w=-[P_dV
Thermodynamics
Determine the number of possible unique products from treating the following compound with NBS and light (hv). Count stereoisomers as a single product. of
Silver, Water and Aluminum
Half a mole of a perfect gas expands isothermally and at 298.15 K from a volume of 10 L to avolume of 20 L. (a) What is the change in the entropy of the gas? (b) How much work is doneon the gas? (c) What is the heat of Surroundings ? (d) What is the change in the entropy of the surroundings? (e)What is the change in the entropy of the system plus the surroundings?
The following reaction has these standard thermodynamie parameters: An-30.6 kmol and AS 55.3 J(mol K).