During an experiment, an ideal gas is found to obey an additional law ...
vp
2 = constant
putting ,
we have T
2/V = constant
or T∝√V
so , if V is doubled , T becomes √2 = 1.4times.
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During an experiment, an ideal gas is found to obey an additional law ...
vp
2 = constant
putting ,
we have T
2/V = constant
or T∝√V
so , if V is doubled , T becomes √2 = 1.4times.
During an experiment, an ideal gas is found to obey an additional law ...
Understanding the Given Law
In this experiment, the ideal gas follows the law \( p^2 V = \text{constant} \). This implies a relationship between pressure (p), volume (V), and temperature (T) of the gas.
Initial Conditions
- The initial conditions are:
- Pressure: \( p_1 \)
- Volume: \( V \)
- Temperature: \( T \)
From the ideal gas law, we know:
\[ p_1 V = nRT \]
Where \( n \) is the number of moles and \( R \) is the gas constant.
Final Conditions After Expansion
After expanding to volume \( 2V \), let the final pressure be \( p_2 \) and the final temperature be \( T_f \):
- New volume: \( 2V \)
- Applying the given law at the final state:
\[ p_2^2 (2V) = p_1^2 V \]
From this, we can derive:
\[ p_2^2 = \frac{p_1^2 V}{2V} = \frac{p_1^2}{2} \]
Thus:
\[ p_2 = \frac{p_1}{\sqrt{2}} \]
Applying the Ideal Gas Law
Now, applying the ideal gas law to the final state:
\[ p_2 (2V) = nRT_f \]
Substituting for \( p_2 \):
\[ \frac{p_1}{\sqrt{2}} (2V) = nRT_f \]
Equating with the initial state:
\[ p_1 V = nRT \]
We can solve for \( T_f \):
\[ \frac{2p_1 V}{\sqrt{2}} = nRT_f \]
Substituting \( p_1 V \):
\[ \frac{2(nRT)}{\sqrt{2}} = nRT_f \]
Simplifying gives:
\[ T_f = \frac{2T}{\sqrt{2}} = T \sqrt{2} \]
To find the numerical temperature, if \( T \) is normalized to 1, then:
\[ T_f = 1 \cdot \sqrt{2} \approx 1.4 \]
Conclusion
Hence, when the gas expands to volume \( 2V \), the final temperature becomes approximately 1.4.