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Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

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BuyFindarrow_forward

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

Nitrogen gas (2.75 L) is confined in a cylinder under constant atmospheric pressure (1.01 × 105 pascals). The volume of gas decreases to 2.10 L when 485 J of energy is transferred as heat to the surroundings. What is the change in internal energy of the gas?

Interpretation Introduction

Interpretation:

The change in internal energy under the compression of nitrogen gas has to be determined.

Concept Introduction:

Internal energy:

The internal energy, U is the sum of kinetic energy and the potential energy inside the system.

Change in internal energy, ΔU is the measures of energy that is transferred as heat and work from the system or to the system.

  ΔU=qp+Wp

Where

  q = heat energy absorbed or released,

  W =work done to the system or from the system.

  W=-P(ΔV) ,

  ΔV is the change in volume

  P is the pressure.

Explanation

Given,

Initial volume is 2.75L

Final volume is 2.10L

  qp= -485J (heat is transferred from the system)

  Pressure=1.01×105P

Work done at constant pressure, Wp=-PΔV

Substitute in above equation we get,

  Wp= -1.01×105kg/ms2(2.10L - 2.75L)

  Wp= -1.01×105kgms2(-65m3)= 65

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