Answered: One mole of an ideal gas initially at a…

One mole of an ideal gas initially at a temperature of T; = 5.2°C undergoes an expansion at a constant pressure of 1.00 atm to eight times its original volume.

Principles of Physics: A Calculus-Based Text

5th Edition

ISBN:9781133104261

Author:Raymond A. Serway, John W. Jewett

Publisher:Raymond A. Serway, John W. Jewett

Chapter17: Energy In Thermal Processes: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 38P: One mole of an ideal gas does 3 000 J of work on its surroundings as it expands isothermally to a...

See similar textbooks

Related questions

Q: 1.00 moles of an ideal monatomic gas (such as He) initially at a temperature of 298 K and a pressure…

Q: An ideal monatomic gas contracts in an isobaric process from 1.05 m³ to 0.540 m3 at a constant…

Q: A3.00 mol sample of an ideal diatomic gas expands adiabatically from a volume of 0.1630 m to 0.735…

A: Given that:n=3.00 moleVi=0.1630 m3Vf=0.735 m3Pi=1.00 atmGas is diatomic and expansion is adiabatic

Q: A gas expands from 1.00 m3 to 4.00 m3. If the expansion is isobaric at a pressure of 2.00 x 105 Pa,…

Q: The temperature of 1.89 mol of a monatomic ideal gas is 376 K. The internal energy of this gas is…

Q: How much work is performed by a gas as it expands from 30L to 45L against a constant external…

Q: A room contains 2500 moles of air. If air is treated as an ideal gas with k = 1.4 compute the change…

Q: An ideal monatomic gas expands isothermally from 0.500 m3 to 1.25 m3 at a constant temperature of…

A: a) The work done on the gas in an isothermal process is given by,

Q: An ideal gas of volume 1.5 x 10 m3 and at pressure 1.0 x 105 Pa is supplied with 70 J of energy. The…

A: Given,Initial volume of the gas, Vi = 1.5×10-3 m3Pressure, Pi = 1.0×105 PadQ = 70 Jfinal volume, Vf…

Q: An ideal diatomic gas contracts in an isobaric process from 1.35 m3 to 0.600 m3 at a constant…

A: a. Write the expression for work done of an isobaric process So the work done on the gas is

Q: An ideal monatomic gas, consisting of 2.8 mol of volume 8.8x10-2 m , expands adiabatically. The…

A: initial volume, V = 8.8 x 10-2 m3 initial temperature, T = 20 degree C = 293 K final temperature, T'…

Q: A certain molecule has f degrees of freedom. Show that an ideal gas consisting of such molecules has…

A: Hello. Since your question has multiple sub-parts, we will solve first three sub-parts for you. If…

Q: A container with an initial volume of 0.0607 m3 holds 2.45 moles of a monatomic ideal gas at a…

A: The initial volume of a monatomic gas, Vi=0.0607 m3 The number of moles of a monatomic ideal gas,…

Q: One mole of an ideal gas initially at a temperature of T = 4.8°C undergoes an expansion at a…

A: (a) Calculate the final temperature by using the ideal gas equation.…

Q: During a compression at a constant pressure of 250 Pa, the volume of an ideal gas decreases from…

A: We know that the expression for the change in the internal energy of the gas is given as below

Q: A mole of a diatomic gas at 0.1 m^3 is expanded isothermally at 298 Kelvins to 1.0 m^3 bar against a…

A: We have a diatomic gas at initial volume V1=0.1 m3 expanded isothermally to volume V2=1 m3 at…

Q: how to answer part b

A: Write the expression for first law of thermodynamics.

Q: An ideal diatomic gas contracts in an isobaric process from 1.15 m to 0.540 m at a constant pressure…

Q: The mixture of a gas contains 10.7 mol nitrogen (N2) gas and 22.7 mol carbon dioxide (CO2) gas. The…

Q: One mole of an ideal gas initially at a temperature of Ti = 3.4°C undergoes an expansion at a…

Q: An ideal monatomic gas contracts in an isobaric process from 1.25 m3 to 0.500 m3 at a constant…

A: Since you have uploaded a question with multiple sub-parts, we will solve first three sub-parts (a),…

Q: One mole of an ideal gas initially at a temperature of Ti = 3.4°C undergoes an expansion at a…

Q: The pressure P and volume V of an expanding gas are related by the formula PV^b=C , where b and C…

Q: One mole of an ideal gas initially at a temperature of Ti = 7.4°C undergoes an expansion at a…

A: An ideal gas is at an initial temperature of 7.4 degree-Celcius goes a constant pressure or isobaric…

Q: A certain molecule has f degrees of freedom. Show that an ideal gas consisting of such molecules has…

A: Let us consider the molecule has f degrees of freedom, then according to the equipartition energy…

Q: For an ideal gas C'y and Cp are different because of the work W associated with the volume change…

Q: A monatomic ideal gas in a rigid container is heated from 223 K to 303 K by adding 9040 J of heat.…

A: Given: Ti=223 K Tf=303 K Q=9040J To find: To determine the moles of gas are there in the…

Q: The molar specific heats of an ideal gas at constant pressure and volume are denoted by Cp and Cv,…

Q: An ideal monatomic gas expands isothermally from 0.590 m3 to 1.25 m3 at a constant temperature of…

Q: An ideal monatomic gas cools from 455.0 K to 405.0 K at constant volume as 831 J of energy is…

A: The internal energy of a thermodynamic is the energy contained within it. It is the energy essential…

Q: An ideal monatomic gas expands isothermally from 0.500 m3 to 1.25 m3 at a constant temperature of…

A: Formula to calculate the work done on the gas is,

Q: As a 1.00 mol sample of a monoatomic ideal gas expands adiabatically, the work done by the gas is 50…

A: As per sign convention work done by gas is taken positive and work done on the gas is taken…

Q: An ideal monatomic gas expands isothermally from 0.500 m³ to 1.25 m³ at a constant tempera- ture of…

Q: V V2 ATWWW味N

Q: 16. Calculate the change internal energy of an ideal gas in J if the temperature is changed from…

Q: What is the total internal energy of 2.00 moles of an ideal gas at 100 K?

Q: During an isothermal process, the number of mols of a gas is doubled while the pressure is held…

Q: The temperature of 2.00 mol of an ideal monatomic gas is raised 15.0 K in an adiabatic process.What…

A: a) In a constant volume process the work done by the gas will be zero.

Q: The pressure P and volume V of an expanding gas are related by the formula PV = C, where b and C are…

A: Given Data: Pressure, P=14 kPa=14×103 Pa Volume, V=50 cm3 dVdt=70 cm3/min Constant b=1.7

Q: When a quantity of monatomic ideal gas expands at a constant pressure of 4.00×10^4 Pa, the volume of…

Q: A 3.65-mol sample of an ideal diatomic gas expands adiabatically from a volume of 0.1210 m3 to 0.750…

Q: 2 moles of diatomic gas has a constant volume of 2.0 L and a temperature of 2000 K. If the…

A: Number of moles of the gas, n = 2 Volume of the gas is constant = 2.0 litres Initial temperature,…

Q: 3 moles of an ideal gas undergoes an isothermal expansion at constant temperature T = 290 K, its…

Q: A sealed ideal gas system contains 2.0 moles of monatomic ideal gas, initially at temperature 300 K…

Concept explainers

Proper Length

The theory of special relativity explains the connection between space and time to objects that move in a straight line at a constant speed. The objects move at the speed of light. When an object approaches light speed, its mass is endless and cannot move faster than light. The most crucial postulate of Einstein's special relativity is that the laws of nature do not change in each frame of reference.

Question

i tried many times but my anwer for b always wrong.Please help me

One mole of an ideal gas initially at a temperature of T; = 5.2°C undergoes an expansion at a constant pressure of 1.00 atm to eight
times its original volume.
(a) Calculate the new temperature T; of the gas.
2227.07
K
(b) Calculate the work done on the gas during the expansion.
16.2
|× k]

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, physics and related others by exploring similar questions and additional content below.

Similar questions

A sample of a monatomic ideal gas occupies 5.00 L at atmospheric pressure and 300 K (point A in Fig. P17.68). It is warmed at constant volume to 3.00 atm (point B). Then it is allowed to expand isothermally to 1.00 atm (point C) and at last compressed isobarically to its original state. (a) Find the number of moles in the sample. Find (b) the temperature at point B, (c) the temperature at point C, and (d) the volume at point C. (e) Now consider the processes A B, B C, and C A. Describe how to carry out each process experimentally. (f) Find Q, W, and Eint for each of the processes. (g) For the whole cycle A B C A, find Q, W, and Eint. Figure P17.68
An ideal gas has a pressure of 0.50 atm and a volume of 10 L. It is compressed adiabatically and quasi-statically until its pressure is 3.0 atm and its volume is 2.8 L. Is the monatomic, diatomic, or polyatomic?
A car tile contains 0.0380 m3 of air at a pressure of 2.20105 Pa (about 32 psi). How much more internal energy does this gas have than the same volume has at zero gauge pressure (which is equivalent to normal atmospheric pressure)?
One mole of an ideal gas does 3 000 J of work on its surroundings as it expands isothermally to a final pressure of 1.00 atm and volume of 25.0 L. Determine (a) the initial volume and (b) the temperature of the gas.
For 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?
The excess internal energy of metabolism is exhausted through a variety of channels, such as through radiation and evaporation of perspiration. Consider another pathway for energy loss: moisture in exhaled breath. Suppose you breathe out 22.0 breaths per minute, each with a volume of 0.600 L. Suppose also that you inhale dry air and exhale air at 37C containing water vapor with a vapor pressure of 3.20 kPa. The vapor comes from the evaporation of liquid water in your body. Model the water vapor as an ideal gas. Assume its latent heat of evaporation at 37C is the same as its heat of vaporization at 100.C. Calculate the rate at which you lose energy by exhaling humid air.
One 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?
Expand 1.00 mol of an monatomic gas initially at 5.00 kPaand 600 K from initial volume Vi = 1.00 m3 to final volume Vf =2.00 m3. At any instant during the expansion, the pressure p and volumeV of the gas are related by p = 5.00 exp[(Vi - V)/a], with p inkilopascals, Vi and V in cubic meters, and a = 1.00 m3.What are thefinal (a) pressure and (b) temperature of the gas? (c) How muchwork is done by the gas during the expansion? (d) What is S for theexpansion? (Hint: Use two simple reversible processes to find S.)
A 2.00-mol sample of helium gas initially at 300 K and0.400 atm is compressed isothermally to 1.20 atm.Assuming the behavior of helium to be that of an idealgas, find (a) the final volume of the gas, (b) the workdone by the gas, and (c) the energy transferred by heat
Suppose 1.00 L of a gas with g = 1.30, initially at 273 K and 1.00 atm, is suddenly compressed adiabatically to half its initial volume. Find its final (a) pressure and (b) temperature. (c) If the gas is then cooled to 273 K at constant pressure, what is its final volume?
Six moles of an ideal gas is compressed to one-third its initial volume. If the gas is maintained at a constant pressure of 2.00 atm, and starts at initial temperature190 &δεγ;C, what is the work done on the gas during the compression? (Note: 0 oC = 273K, and 1 atm = 101,325 Pascals.)
In a quasi-static isobaric expansion, 500 J of work are done by the gas. If the gas pressure is 0.80 atm, what is the fractional increase in the volume of the gas, assuming it was originally at 20.0 L?