Consider two initially separate metal blocks of aluminium (M, = 26.98 g/mol) and lead (Mr = 207.19 g/mol) in a chamber with adiabatic walls. The lead block of mass 3 g is initially at 100°C and that of aluminium of mass 4 g is initially at 25°C. The blocks are then placed in contact and allowed to thermally equilibrate. The molar heat capacities of the metals are considered constant over the temperature of experiment. At 1 bar, Cpm (Al) = 24.35 JK¹¹mol-¹ and Cp,m(Pb) = 26.44 JK¹mol-¹ Calculate a. b. C. the final temperature. the change in the entropy of the blocks in contact. identify evidence that the process occurred spontaneously or not.

Consider two initially separate metal blocks of aluminium (M, = 26.98 g/mol) and lead (Mr = 207.19 g/mol) in a chamber with adiabatic walls. The lead block of mass 3 g is initially at 100°C and that of aluminium of mass 4 g is initially at 25°C. The blocks are then placed in contact and allowed to thermally equilibrate. The molar heat capacities of the metals are considered constant over the temperature of experiment. At 1 bar, Cpm (Al) = 24.35 JK¹¹mol-¹ and Cp,m(Pb) = 26.44 JK¹mol-¹ Calculate a. b. C. the final temperature. the change in the entropy of the blocks in contact. identify evidence that the process occurred spontaneously or not.

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

A mole of perfect monoatomic gas is expanded adiabatically and reversibly from 1 bar and 300K to 0.1 bar. Calculate the AU of the system in kJ
3. Derive the thermodynamic equation of state for an ideal gas starting from internal energy then express this equation in a form without differentials. = -P +T| T LƏT.
Benzoic acid, C;HsO:H, is typically used as a çalibrant for determining the specific heat of bomb calorimeters. It combusts via the following unbalanced chemical reaction: C,H5O2H (s) + 02(g) → CO2 (g) + H2O(1) 3. For this experimental setup and reaction, the constant volume heat flow is known to be gy = -26.979 kJ. Over the course of the reaction, the temperature rose from 19.863 °C to 22.540 °C. Calculate the heat capacity, Cou, for this calorimeter in kJ °C-!.
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
(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.
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. =
A horizontally-oriented cylinder contains an unknown noble gas at 42100 Pa and is sealed with a massless piston of radius 0.272 m. The piston is quasi-statically and isobarically moved inward 0.189 m, while 19500 J of heat is removed from the gas. Calculate the change in internal energy AU of the system. AU=
Qui Air in a closed piston-cylinder arrangement is expanded from the initial pressure of 8.3 bar and initial volume of O.029 m to the final state of p2 2.2 bar. A polytropic relation of pV13 = constant was followed between pressure and volume for the process. The specific internal energy at the initial and final states are 156.5 and 101.5 kJ/kg, respectively. The mass of the air is 0.28 kg. Neglecting the effect of kinetic and potential energy, determine the heat transfer, inkJ.
Physical chemistry - please refer to pics Now, consider 2.0 moles of methane (CH4 ), initially at 273 K, that is reversibly and adiabatically compressed from an initial volume of 10.00 L to a final volume of 2.00 L. 3a. Determine the final temperature, considering the gas to be described by the ideal gas equation of state. 3b. Determine the work required w, the associated heat flow q, and the internal energy change ∆U for the gas between the initial and final states.
0.1 kg of nitrogen gas at 200 kPa and 50°C is contained in a piston-cylinder arrangement. The piston is moved compressing nitrogen until the pressure becomes 1 MPa and temperature becomes 150°C. The work done during the process is 40 kJ. Calculate the heat transferred from the nitrogen to the surroundings. C y for nitrogen = 0.75 kJ/kg K.