A bulb of unknown volume V contains an ideal gas at 1 atm pressure. This bulb was connected to another evacuated bulb of volume 0.5 litre through a stopcock. When the stopcock was opened the pressure at each became 530 mm while the temperature remained constant. Find V in litres.

Explanation

To solve the problem, we will use the ideal gas law and the principle of conservation of moles. Here’s a step-by-step breakdown of the solution:

### Step 1: Understand the Initial Conditions
We have a bulb of unknown volume \( V \) containing an ideal gas at a pressure of 1 atm. This is our initial state.

### Step 2: Convert Initial Pressure to mmHg
Since the final pressure is given in mmHg, we need to convert the initial pressure from atm to mmHg.
1 atm = 760 mmHg, so:
...