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Consider a balloon filled with helium at the following conditions. 313 g He 1.00 atm 1910. L Molar Heat Capacity = 20.8 J/°C mol The temperature of this balloon is decreased by 41.6°C as the volume decreases to 1643 L, with the pressure remaining constant. Determine q, w, and ∆ E( in KJ ) for the compression of the balloon.

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Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

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Chapter
Section
BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 7, Problem 114CWP
Textbook Problem
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Consider a balloon filled with helium at the following conditions.

313 g He
1.00 atm
1910. L
Molar Heat Capacity = 20.8 J/°C mol

The temperature of this balloon is decreased by 41.6°C as the volume decreases to 1643 L, with the pressure remaining constant. Determine q, w, andE(in KJ) for the compression of the balloon.

Interpretation Introduction

Interpretation: The heat, work and internal energy change of the given balloon should be calculated.

Concept Introduction:  Internal energy is a total energy of a system, consists of kinetic, potential energies. The internal energy change is associate with heat flow or as work done on or by a system.

                    Equation:

                                           ΔE=q±w......(1)

                                                   q is a heat

                                                   w is a work

  •  The work is considered as a pressure and volume for the gases expansion and compressions in thermodynamic process.

    Formula:

Explanation of Solution

Explanation

Record the given data:

                           MassofHeis313gPressureis1.0atmInitialvolumeis1910L.MolarheatcapacityofHeis20.8J/°C.molFinalvolumeis1643LDecreasedtemperatureis41.6°C

  • The given mass of He, pressure, volumes molar heat capacity and decreased temperature are recorded as shown above.

To calculate the mole of given He gas.

                                                 =Mass of He(g)×1molofHeMassHe(g)=3131MoleHe4.003gHe=78.2mol

  • The given values are plugging in above equation to give mole of 313g of He.
  • The mole of 313g of He is 78.2mol.

To calculate the absorbed heat of He balloon.

Absorbed heat (J) = Molar heat capacity(J) /Temperature change(c)×mass ofsubstance (g)

                 absorbed heat(q) =20.8J°Cmol×78.2mol×(-41

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Chapter 7 Solutions

Chemistry: An Atoms First Approach
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