Suppose that one of water at its boiling point is kept in a cylinder that hasfrictionless piston. For equilibrium to be established, a pressure ismaintained above the piston. If the piston sweeps out a volume of 2.0dm³. Calculate the work done by the system for the following paths:a- Free expansionb- Reversible expansion against constant pressure of 1.0 atmc- Isothermal reversible expansion with initial volume = 0.5 dm³.

Given: Water is at boiling point, so Temperature = 373 K Volume sweep by the piston = 2.0 dm3 To…

Answered: a- Free expansion b- Reversible…

a- Free expansion b- Reversible expansion against constant pressure of 1.0 atm c- Isothermal reversible expansion with initial volume = 0.5 dm

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 sample of methane, CH4, of mass 4.50g occupies 12.7 dm³ at 310K. a. Calculate the irreversible work done when it expands isothermally against an external pressure of 200 torr until its volume is increased by 3.3 dm³. b. Calculate the work done if the same expansion occurs reversibly.
The two processes that equivalent are for an ideal gas Isothermal reversible expansion and Adiabatic free expansion O Isothermal free expansion and Adiabatic free expansion O othermal reversible expansion and Adiabatic reversible expansion O Adiabatic free expansion and Adiabatic reversible expansion O
Consider 1.2 moles of a diatomic gas that expands adiabatically from an initial pressure of 5.0 x 10^5 Pa and a temperature of 400 K to a final pressure of 1.0 x 10^5 Pa. a) Find the final temperature. b) Find the final volume. c) Find the work done by the gas. d) Find the change in internal energy of the gas.
Use the data from this table of thermodynamic properties to calculate the maximum amount of work that can be obtained from the combustion of 1.00 mole of ethane, CH3CH3(g), at 25 °C and standard conditions. mo
Suppose that one of water at its boiling point is kept in a cylinder that has frictionless piston. For equilibrium to be established, a pressure is maintained above the piston. If the piston sweeps out a volume of 0 dm3. Calculate the work done by the system for the following paths: Free expansion Reversible expansion against constant pressure of 4.0 atm Isothermal reversible expansion with initial volume = 0.80 dm3. When 2.0 mol of CO2 is heated at a constant pressure of 1.25 atm, its temperature increases from 280.00 K to 307.00 K. The heat (q) absorbed during this process is determined to be 2.0 kJ. Calculate (a) ΔH for this process (b) The molar heat capacity of CO2 at constant pressure (CP,m) (Hint: you can assume that CP,m is constant over this temperature range and that the CO2behaves ideally). (c) ΔU. Heat capacity of a material is temperature dependent. The T-dependence of the molar heat capacities of water (H2O(l)), H2(g) and O2(g) can be…
2 moles of He gas (assume ideal) expands isothermally and reversibly at a constant external pressure of 1 atm and a temperature of 298 K from a volume of 10 L to a volume of 40 L. Calculate ΔA in kilojoules
In which of the following scenarios is no change in the internal energy of the system possible? O q 0 O q = 0, w > 0 O q 0, w > 0
Consider the free, isothermal (constant T) expansion of an ideal gas. "Free" means that the external force is zero, perhaps because a stopcock has been opened and the gas is allowed to expand into a vacuum. Calculate AU for this irreversible process. Show that q sion is also adiabatic (q = 0) for an ideal gas. This is analogous to a classic experiment first performed by Joule. 0, so that the expan-
Calculate w for the adiabatic reversible expansion of 65 moles of an ideal gas at 273.2 K and 20 atm to a final pressure of 2 atm. Given the following: Cp = 5R/2, mole–1deg–1 Cv = 3R/2, mole–1deg–1 R = 8.314J mole–1deg–1
13) Calculate the AGᵒrxn at 298 K using the following information. 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H₂O(g) - 33.4 -300.1 -228.6 AG°f (kJ/mol) A) -990.6 kJ B) +112.4 kJ C) +66.8 kJ 2A1 (s) + 312 (s) AG°r rxn ? D) -528.7 kJ 14) The standard cell potential for the cell using the overall cell reaction below is +2.20 V: 2A13+ (aq) + 61- (aq) The voltage generated by the cell when [A13+] = 4.5 × 10-3 M and [I-] = 0.15 Mis A) 2.32 B) 2.10 C) 2.39 D) 2.20 E) -495.3 kJ V. E) 2.23
2. A sample consisting of 2.00 moles Helium is expanded isothermally at 22⁰C from 22.8 L to 31.7 L,(a) reversibly (b) against a constant external pressure equal to the final pressure of the gas (c) freely (against zero external pressure). For the three processes calculate q, w, ∆U, and ∆H
Below are the three scenarios for isothermal expansion of 1 mole of ideal gas at 300K. Calculate work, heat, internal energy change and enthalpy change by the system for each case. a. pi=8 atm, V1=2L, p2=2 atm and V2=8L and pext=0 p= 0 p= 0 P2.V2 P1,V1 b. pi-8 atm, V1=2L, pz=2 atm and V,-8L P2 P2 P2. V2 P1,V1