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An ideal gas initially occupying 20 {~L} at 27^{} {C} and 2 at

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An ideal gas initially occupying $20 L$ at $2 7^{\circ} C$ and 2 atm pressure is allowed to expand into an evacuated vessel such that the final volume is $50 L$ . If the pressure were to remain at the same value of 2 atm, to what temperature should the gas be heated?

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IIT-JEE Super Course in Chemistry - Physical Chemistry (Pearson)

Text solutionVerified

Applying Charles' Law,

\frac{V _{1}}{T _{1}} = \frac{V _{2}}{T _{2}} \Rightarrow \frac{20}{300} = \frac{50}{T _{2}}

\Rightarrow T_{2} = \frac{300 \times 50}{20} = 750 K (or) t (in^{\circ} C) = 750 - 273 = 47 7^{\circ} C

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An ideal gas initially occupying

20 L

2 7^{\circ} C

and 2 atm pressure is allowed to expand into an evacuated vessel such that the final volume is

50 L

. If the pressure were to remain at the same value of 2 atm, to what temperature should the gas be heated?

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Question Text	An ideal gas initially occupying $20 L$ at $2 7^{\circ} C$ and 2 atm pressure is allowed to expand into an evacuated vessel such that the final volume is $50 L$ . If the pressure were to remain at the same value of 2 atm, to what temperature should the gas be heated?
Topic	States of Matter
Subject	Chemistry
Class	Class 11
Answer Type	Text solution:1
Upvotes	83

An ideal gas initially occupying $20 L$ at $2 7^{\circ} C$ and 2 atm pressure is allowed to expand into an evacuated vessel such that the final volume is $50 L$ . If the pressure were to remain at the same value of 2 atm, to what temperature should the gas be heated?

Text solutionVerified

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An ideal gas initially occupying $20 L$ at $2 7^{\circ} C$ and 2 atm pressure is allowed to expand into an evacuated vessel such that the final volume is $50 L$ . If the pressure were to remain at the same value of 2 atm, to what temperature should the gas be heated?