Book edition 10th Edition

Author(s) David Halliday

Pages 1328 pages

ISBN 9781118230718

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Short Answer

An ideal gas initially at $300 K$ is compressed at a constant pressure of $25 N / m^{2}$ from a volume of $3.0 m^{3}$ to a volume of $1.8 m^{3}$ . In the process, $75 J$ is lost by the gas as heat. What are
(a) the change in internal energy of the gas and
(b) the final temperature of the gas?

The internal energy change in the gas is $Δ E_{int} = - 45 J$ .
The temperature of the gas changes to $180 K$ .

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Step by Step Solution

TABLE OF CONTENTS :

TABLE OF CONTENTS

Step 1: Concept

The process that takes place at constant pressure is called an isobaric process. Using the formulas for work done W in an isobaric process, and the first law of thermodynamics, we can find the change in the internal energy ${ΔE}_{int}$ of the gas. Also, by using the ideal gas law in the ratio form, we can find the final temperature $T_{2}$ of the gas.

1.The work done W in anisobaric process is

$W = pΔV$

2.The ideal gas law in ratio form is

$T_{2} = T_{1} (\frac{V_{2}}{V_{1}})$

3.The change in the internal energy is

${ΔE}_{int} = Q - W$

Step 2: Given Data

The pressure . $p = 25 {N/m}^{2}$
The final volume $V_{f} = 1.8 m^{3}$
The initial volume . $V_{i} = 3.0 m^{3}$
The initial temperature $T_{1} = 300 K$
In the process, the energy lost by the gas as heat is $Q = - 75 J$ .

Step 3: Calculations

a.The work done in anisobaricprocess is expressed as-

$W = p Δ V$

Where p is the pressure and $Δ V = (V_{f} - V_{i})$ is change in the volume

Therefore,

$\begin{matrix} W = p (V_{f} - V_{i}) \\ = 25 N / m^{2} \times (1.8 m^{3} - 3.0 m^{3}) \\ = - 30 J \end{matrix}$

From the first law of thermodynamics, we have-

$Δ E_{int} = Q - W$

Where Q is the heat transferred and $Δ E_{i n t}$ is the change in the internal energy o the gas. It is given that Q amount of energy leaves the system; therefore, we can consider Q as negative. $Q = - 75 J$

$\begin{matrix} Δ E_{int} = - 75 J - (- 30 J) \\ = - 75 J + (30 J) \\ = - 45 J \end{matrix}$

Internal energy is decreased by $- 45 J$

b.Since the pressure is constant and the number of moles presumed are constant, the ideal gas law can be written as-

$\begin{matrix} T_{2} = T_{1} (\frac{V_{2}}{V_{1}}) \\ = 300 K \times (\frac{1.8 m^{3}}{3.0 m^{3}}) \\ = 180 K \end{matrix}$

Step 4: Conclusion

The change in internal energy of the gas is $- 45 J$ and the final temperature of the gas is $180 K$ .

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Fundamentals Of Physics

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Short Answer

An ideal gas initially at $300 K$ is compressed at a constant pressure of $25 N / m^{2}$ from a volume of $3.0 m^{3}$ to a volume of $1.8 m^{3}$ . In the process, $75 J$ is lost by the gas as heat. What are
(a) the change in internal energy of the gas and
(b) the final temperature of the gas?

Step by Step Solution

Step 1: Concept

Step 2: Given Data

Step 3: Calculations

Step 4: Conclusion

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An ideal gas initially at 300 K is compressed at a constant pressure of 25 N/m2 from a volume of 3.0 m3to a volume of 1.8 m3 . In the process, 75 J is lost by the gas as heat. What are (a) the change in internal energy of the gas and (b) the final temperature of the gas?

Step by Step Solution

Step 1: Concept

Step 2: Given Data

Step 3: Calculations

Step 4: Conclusion

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An ideal gas initially at $300 K$ is compressed at a constant pressure of $25 N / m^{2}$ from a volume of $3.0 m^{3}$ to a volume of $1.8 m^{3}$ . In the process, $75 J$ is lost by the gas as heat. What are
(a) the change in internal energy of the gas and
(b) the final temperature of the gas?