P2.30 A 1.75 mol sample of an ideal gas for which Cv.m = 3R/2 undergoes the following two-step process: (1) From an initial state of the gas described by T = 15.0°C and P = 5.00 X 104 Pa, the gas undergoes an isothermal ex- pansion against a constant external pressure of 2.50 X 104 Pa until the volume has doubled. (2) Subsequently, the gas is cooled at constant volume. The temperature falls to -19.0°C. Calculate q, w, AU, and AH for each step and for the overall process.

P2.30 A 1.75 mol sample of an ideal gas for which Cv.m = 3R/2 undergoes the following two-step process: (1) From an initial state of the gas described by T = 15.0°C and P = 5.00 X 104 Pa, the gas undergoes an isothermal ex- pansion against a constant external pressure of 2.50 X 104 Pa until the volume has doubled. (2) Subsequently, the gas is cooled at constant volume. The temperature falls to -19.0°C. Calculate q, w, AU, and AH for each step and for the overall process.

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

Indicate the true option about calorimetry.(A). Internal energy is an intensive quantity.(B). The enthalpy does not depend on p, since this variable is the amount of heat put into play during an isobaric transformation.(C). The superscript ° added to the thermodynamic functions indicates that it is operated at p = 1 atm and T = 298.15 K.(D). The heat exchanged between a system and the medium is not a state function.
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.
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
Consider a gas obeying van der waals equation. Let one mole of the gas expands reversibly from volume ΔΗ, under isothermal condition. The expression of ORT 1 1 V ·b V -b m2 m1 bRT a V m2 1 Vm2-b V V ORT In- m1 V -b m2 V-b m1 1 m1 V b -b m for this process is: a m2 + 2a V m2 a V + m1 2a V. m1 V V m1 to m2
(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.
The reduction of iron(III) oxide (Fe₂O,) to pure iron during the first step of steelmaking, 4 - 4 Fe(s) + 30, (e) 4 2 Fe,0,(3) is driven by the high-temperature combustion of coke, a purified form of coal: C(s) + O₂(e) co₂(e) Suppose at the temperature of a blast furnace the Gibbs free energies of formation AG, of CO, and Fe₂O, are-413. kl/mol and -826. kJ/mel, respectively. Calculate the maximum mass of pure iron that can be produced by the combustion of 6200. kg of cake. Round your answer to 2 significant digits. A kg 0.P 00 1.60 9
For the reaction bellow: C„H(2n+2) + a(02 + 3.76 N2) → nC02 + (n+ 1)H,0 + 3.76a N2 If the heat of combustion writing as: Qc = 618.49 n+ 187. 83 And the mole fraction of CO, in products is Xco, 1. Type of fuel. 2. Heat of combustion (KJ/mole of fuel) 25 find: 227 3. If n=4, find the mole fractions of Co, H,0 and N2
1.50 mol of an ideal gas with a constant ratio of heat capacities at constant pressure and volume y = Cy = 1.40 is taken through the (reversible) cycle shown in the figure below. The process A → B is an expansion at constant temperature, whereas B → C and C → A are constant-pressure compression and constant-volume processes, respectively. a) What is the temperature TA of the gas at A? P (atm) For the cycle as a whole, 5- Isothermal b) calculate the (net) work done W (by the gas), process c) calculate the (total) heat transfer Q, d) find the change in the (internal) energy U of the gas, ●B e) verify that the 1st law of thermodynamics -V (liters) 50 is satisfied. 1 liter=1.00x10³ m³ ,1 atm=1.01x105 N/m² , kB = 10 1.38x10-23 J/K , NA=6.02x10²3 mol1.
Two ideal gases, one monoatomic and the other diatomic are mixed with one another and form an ideal gas again. The equation of the adiabatic process of the mixture is 11 PVY= = constant; where What is the ratio of the number of molecules of the monoatomic gas to that of the diatomic gas in the mixture?