1. | same as the pressure initially. |
2. | \(2\) times the pressure initially. |
3. | \(10\) times the pressure initially. |
4. | \(20\) times the pressure initially. |
As gas breaks, the number of moles becomes twice of initial, so .
Step 2: Apply the ideal gas equation.
Now, by the ideal gas equation, PV =nRT
Hence, the final pressure becomes 20 times the initial pressure.
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