![Fundamentals of Physics, Volume 1, Chapter 1-20](https://www.bartleby.com/isbn_cover_images/9781118233764/9781118233764_largeCoverImage.gif)
Water standing in the open at 32.0°C evaporates because of the escape of some of the surface molecules. The heat of vaporization (539 cal/g) is approximately equal to en, where e is the average energy of the escaping molecules and n is the number of molecules per gram, (a) Find ε. (b) What is the ratio of ε to the average kinetic energy of H2O molecules, assuming the latter is related to temperature in the same way as it is for gases?
![Check Mark](/static/check-mark.png)
Want to see the full answer?
Check out a sample textbook solution![Blurred answer](/static/blurred-answer.jpg)
Chapter 19 Solutions
Fundamentals of Physics, Volume 1, Chapter 1-20
Additional Science Textbook Solutions
Essential University Physics: Volume 2 (3rd Edition)
Physics: Principles with Applications
College Physics: A Strategic Approach (4th Edition)
Tutorials in Introductory Physics
Lecture- Tutorials for Introductory Astronomy
Essential University Physics: Volume 1 (3rd Edition)
- On a hot summer day, the density of air at atmospheric pressure at 35.0C is 1.1455 kg/m3. a. What is the number of moles contained in 1.00 m3 of an ideal gas at this temperature and pressure? b. Avogadros number of air molecules has a mass of 2.85 102 kg. What is the mass of 1.00 m3 of air? c. Does the value calculated in part (b) agree with the stated density of air at this temperature?arrow_forwardOne of a dilute diatomic gas occupying a volume of 10.00 L expands against a constant pressure of 2.000 atm when it is slowly heated. If the temperature of the gas rises by 10.00 K and 400.0 J of heat are added in the process, what is its final volume?arrow_forwardAssuming the human body is primarily made of water, estimate the number of molecules in it. (Note that water has a molecular mass of 18 g/mol and there are roughly 1024 atoms in a mole)arrow_forward
- Using a numerical integration method such as Simpson's rule, find the fraction of molecules in a sample of oxygen gas at a temperature of 250 K that have speeds between 100 m/s and 150 m/s. The molar mass of oxygen (O2) is 32.0 g/mol. A precision to two significant digits is enough.arrow_forwardFor a temperature increase of 10 at constant volume, what is the heat absorbed by (a) 3.0 mol of a dilute monatomic gas; (b) 0.50 mol of a dilute diatomic gas; and (c) 15 mol of a dilute polyatomic gas?arrow_forwardTwo monatomic ideal gases A and B are at the same temperature. If 1.0 g of gas A has the same internal energy as 0.10 g of gas B, what are (a) the ratio of the number of moles of each gas and (b) the ration of the atomic masses of the two gases?arrow_forward
- An ideal gas initially at 300 K undergoes an isobaric expansion at 2.50 kPa. If the volume increases from 1.00 m3 to 3.00 m3 and 12.5 kJ is transferred to the gas by heat, what are (a) the change in its internal energy and (b) its final temperature?arrow_forwarda) Calculate the volume in ft of one Ib-mole of air (MW = 29 lbm/lb-mole) at a temperature of 492 R at a pressure of 1 atm (absolute). b) Repeat the calculation of a) but now considering 1 Ib-mole of CO2 (MW= 44 lbmlb-mole). c) Calculate the molar volume (V) of this mole of air in ft'/lb-mole. d) Calculate the density (P) of air in Ibm/ft under these conditions e) Calculate the density (p) of CO, in Ib.m/ft under these conditionsarrow_forwardThe ideal gas law relates the pressure P, volume V, and temperature T of an ideal gas: PV = nRT where n is the number of moles and R = 8.3145 J/(K mol). Plots of pressure versus volume at constant temperature are called isotherms. Plot the isotherms for one mole of an ideal gas for volume ranging from 1 to 10 m', at tempera- tures of T = 100, 200, 300, and 400 K (four curves in one plot). Label the axes and display a legend. The units for pressure are Pa. n=1arrow_forward
- The Ideal Gas Law is given by the equation: PV — пRT Where: P = pressure V = volume n = moles T = temperature in Kelvin In order to solve for the moles, n, you must multiply both sides of the equation by the same expression: PV × = nRT × The resulting equation is: n =arrow_forwardSuppose the amount of air in a person's lungs is 1.75 L. Calculate the number of moles of air molecules in the person’s lungs when the pressure there is atmospheric pressure. Note that the air is at 37.0°C (body temperature).arrow_forwardThe enthalpy of a system is given by the equation H=U+PV where U is the internal energy, P=pressure, and V=volume. In addition, the internal energy, U=Q+W where Q is the heat and W is the work. Suppose we want to find the rate of change in the enthalpy at constant pressure of 1.75 atm, what is the value when heat is absorbed by the system at a rate of 55 J/s and work is done by the system at a rate of 200 J/s when the change of volume is rated at 76 x 10^-5 m^3/s? 1. What is the change in heat with respect to time?2. What is the change in internal energy of the system with respect to time?3. What is the change in enthalpy of the system with respect to time?arrow_forward
- Physics for Scientists and Engineers: Foundations...PhysicsISBN:9781133939146Author:Katz, Debora M.Publisher:Cengage LearningUniversity Physics Volume 1PhysicsISBN:9781938168277Author:William Moebs, Samuel J. Ling, Jeff SannyPublisher:OpenStax - Rice University
- Principles of Physics: A Calculus-Based TextPhysicsISBN:9781133104261Author:Raymond A. Serway, John W. JewettPublisher:Cengage Learning
![Text book image](https://www.bartleby.com/isbn_cover_images/9781133939146/9781133939146_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781938168161/9781938168161_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781938168277/9781938168277_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781133104261/9781133104261_smallCoverImage.gif)