A bulb of unknown volume contained an ideal gas at 650 mm pressure. A certain amount of gas was withdraw and found to occupy 1.52 cc at 1 atm pressure. The pressure of the gas remaining in the bulb was 600 mm. If all measurements were made at a constant temperature, find the volume of the bulb.

Explanation

To solve the problem step by step, we will use the Ideal Gas Law, which states that \( PV = nRT \). Here, \( P \) is the pressure, \( V \) is the volume, \( n \) is the number of moles, \( R \) is the gas constant, and \( T \) is the temperature. Since the temperature is constant, we can compare the states of the gas before and after some gas is withdrawn.

### Step 1: Understand the Initial Conditions
- The initial pressure in the bulb is \( P_1 = 650 \, \text{mm Hg} \).
- After withdrawing some gas, the remaining pressure in the bulb is \( P_2 = 600 \, \text{mm Hg} \).
- The volume of the gas withdrawn occupies \( V_w = 1.52 \, \text{cc} \) at a pressure of \( P_w = 1 \, \text{atm} \).

### Step 2: Convert Units
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