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College Physics

11th Edition
Raymond A. Serway + 1 other
ISBN: 9781305952300

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BuyFindarrow_forward

College Physics

11th Edition
Raymond A. Serway + 1 other
ISBN: 9781305952300
Textbook Problem

An ideal gas undergoes an adiabatic process so that no energy enters or leaves the gas by heat. Which one of the following statements is true? (a) Because no energy is added by heat, the temperature cannot change. (b) The temperature increases if the gas volume increases. (c) The temperature increases if the gas pressure increases. (d) The temperature decreases if the gas pressure increases. (e) The temperature decreases if the gas volume decreases.

(a)

To determine

To say True or False: An ideal gas undergoes an adiabatic process so that no energy enters or leaves the gas by heat. Because no energy added by heat the temperature cannot change.

Explanation

In an adiabatic process, a system will be thermally isolated from it environment. Hence no energy enters or leaves the particular system in an adiabatic process.

In an adiabatic process the energy exchanged between system and the surrounding is zero

That is Q=0. So first law of thermodynamics is given by,

ΔU=W

(b)

To determine

To say True or False: An ideal gas undergoes an adiabatic process so that no energy enters or leaves the gas by heat. The temperature increases if the gas volume increases.

(c)

To determine

To say True or False: An ideal gas undergoes an adiabatic process so that no energy enters or leaves the gas by heat. The temperature increases if the gas pressure increases.

(d)

To determine

To say True or False: An ideal gas undergoes an adiabatic process so that no energy enters or leaves the gas by heat. The temperature decreases if the gas volume increases.

(e)

To determine

To say True or False: An ideal gas undergoes an adiabatic process so that no energy enters or leaves the gas by heat. The temperature decreases if the gas volume decreases.

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