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A evacuated bulb of unknown volume is fi...

A evacuated bulb of unknown volume is filled with `H_(2)` gas at room temperature `(30^(@)C)`. The pressure of the gas in the bulb is 750 mm Hg. A portion of the gas is transferred to a different flask and found to occupy a volume of 50.0 mL at 1 atm pressure and at the same temperature. the pressure of the `H_(2)` gas remaining in the original bulb drops to 600 mm Hg. What is the volume of the bulb assuming `H_(2)` gas is an ideal gas ?

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To solve the problem step by step, we will use the ideal gas law, which is given by the equation: \[ PV = nRT \] Where: - \( P \) = pressure - \( V \) = volume - \( n \) = number of moles ...
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