Calculate the change in entropy of 1.0 kg of lead when it cools from 500 °C to 100 °C. Take Cp,m= 26.44 J K-1 mol -1. Change in entropy = J/K. 3 sig. figures. Note: There is no need to add the units. Just the numerical value is sufficient as long as it is calculated in J/K. Please also indicate sign if it is necessary without a space from the numerical answer.

Calculate the change in entropy of 1.0 kg of lead when it cools from 500 °C to 100 °C. Take Cp,m= 26.44 J K-1 mol -1. Change in entropy = J/K. 3 sig. figures. Note: There is no need to add the units. Just the numerical value is sufficient as long as it is calculated in J/K. Please also indicate sign if it is necessary without a space from the numerical answer.

Physics for Scientists and Engineers, Technology Update (No access codes included)

9th Edition

ISBN:9781305116399

Author:Raymond A. Serway, John W. Jewett

Publisher:Raymond A. Serway, John W. Jewett

Chapter22: Heat Engines, Entropy, And The Second Law Of Thermodynamics

Section: Chapter Questions

Problem 22.2OQ: Assume a sample of an ideal gas is at room temperature. What action will necessarily make the...

See similar textbooks

Similar questions

A copper rod of cross-sectional area 5.0 cm2 and length 5.0 m conducts heat from a heat reservoir at 373 K to one at 273 K. What is the time rate of change of the universe's entropy for this process?
Assume a sample of an ideal gas is at room temperature. What action will necessarily make the entropy of the sample increase? (a) Transfer energy into it by heat, (b) Transfer energy into it irreversibly by heat, (c) Do work on it. (d) Increase either its temperature or its volume, without letting the other variable decrease, (e) None of those choices is correct.
An ideal gas at temperature T is stored in the left half of an insulating container of volume V using a partition of negligible volume (see below). What is the entropy change per mole of the gas in each of the following cases? (a) The partition is suddenly removed and the gas quickly fills the entire container. (b) A tiny hole is punctured in the partition and after a long period, the gas reaches an equilibrium state such that there is no net flow through the hole. (c) The partition is moved very slowly and adiabatically all the way to the light wall so that the gas finally fills the entire container.
Experimental measurements of the heat capacity of aluminum at low temperatures (below about 50 K) can be fit to the formula Cv = aT+bT3 ,where Cv is the heat capacity of one mole of aluminum, and the constants a and b are approximately a = 0.00135 J/K2 and b = 2.48 X 10-5 J/K4. From this data, find a formula for the entropy of a mole of aluminum as a function of temperature. Evaluate your formula at T = 1 K and at T = 10 K, expressing your answers both in conventional units (J/K) and as unitless numbers (dividing by Boltzmann's constant).
By how much does the entropy of 1.0 kg of water change when heated from 263.15 K up to 283.15 K at a pressure of 1 bar? (The solution is 1.5 kJ/K)
The boiling point of compound X is 12° C and its enthalpy of vaporization is 24.6 KJ/mole. What is the entropy (in Joules/mole) of vaporization for this compound?(NOTE: express answer in the NEAREST WHOLE NUMBERS)
Can you help me show the process in these problem? 1. Thermodnamics Calculate the change ΔGm in the Gibbs energy of 1 mol of liquid mercury initially at 1 bar pressure if a pressure of 1000 bar is applied to it. The process occurs at the constant temperature of 25 °C, and the mercury may be assumed to be incompressible and to have a density of 13.5 g cm–3. Ans: 1.485 kJ/mole 2. The entropy of argon is given to a good approximation by the expression: Sm/J K–1 mol–1 = 36.36 + 20.79 ln(T/K). Calculate the change in Gibbs energy of 1 mol of argon if it is heated at constant pressure from 25°C to 50°C. Ans: -3.89 kJ/mol 3. The variation of the equilibrium vapor pressure with temperature for liquid and solid chlorine in the vicinity of the triple point is given by (image Below) Use P/pascal in the equations. Calculate the triple point pressure and temperature. Ans: 270.4 K 4. Calculate the heat of vaporization of water at 373.15 K and 101.325 kPa using the Clausius-Clapeyron equation. The…
In Debye Approximation the entropy at some temperature T (less than 10 K) is aT(Blank 1 ) /3 If the value of this entropy at T = 3.5 K is 1.55 J / K , then the value of the coefficient "a" is : ( Blank 2)
Hi, could I get some help with this macro-connection physics problem involving isothermal expansion? The set up is: For an isothermal reversible expansion of two moles of an ideal gas, what is the entropy change of the a) gas and b) the surroundings in J/K to 4 digits of precision if the gas volume quadruples, assuming NA = 6.022e23 and kB = 1.38e-23 J/K? Thank you.
A perfect gas at 727 oC and with a volume of 0.003 m3expands reversibly in a cylinder behind a piston until its temperature is 2 oC and volume is 0.6 m3according to a linear relationship on the T-s diagram such that its entropy increases as the temperature decreases. Sketch the process on the T-s diagram and calculate the work transfer per kilogram of gas. The specific heat capacity at constant volume, cv is 1.23 kJ/kg K and the specific gas constant, R is 0.3198 kJ/kg K
Starting with the Clausius Inequality, ∂S ≥ ∂q/T, can you prove that, under conditions of constant pressure and entropy, for the total entropy to increase, ∂H ≤ 0 J?
The initial temperature and pressure for one mole of an ideal gas is (Cv = 5 cal mol-1 deg-1) 27oC and 1 atm. Pressure is increased reversibly to 5.3 atm and the temperature is incremented to 90 oC. Calculate the entropy of the process. R = 2 cal mol-1deg-1 answer in cal deg-1