Answer:
[tex]2.42liter[/tex]
Explanation:
The question is incomplete; you need some additional data.
I will assume the missing data from a similar question and keep the final pressure of 703 torr given in your question.
An ideal gas at a pressure of 1.20 atm is contained in a bulb of unknown volume. A stopcock is used to connect this bulb with a previously evacuated bulb that has a volume of 0.720 L as shown here. When the stopcock is opened the gas expands into the empty bulb
If the temperature is held constant during this process and the final pressure is 703 torr , what is the volume of the bulb that was originally filled with gas?
Since the amount of gas and the temperature remain constant, we may use Boyle's law:
[tex]PV=constant\\\\P_1V_1=P_2V_2[/tex]
Form the data:
[tex]P_1=1.20atm\\\\P_2=703torr\\\\V_1=unknown\\\\V_2=V_1+0.720liter[/tex]
1. Convert 703 torr to atm:
[tex]P_2=703torr\times 1atm/760torr=0.925atm[/tex]
2. Sustitute the data in the equation:
[tex]1.2atm\times V_1=0.925atm\times(V_1+0.720liter)[/tex]
3. Solve:
[tex]1.2V_1=0.925V_1+ 0.666liter\\\\0.275V_1=0.666liter\\\\V_1=2.4218liter\approx 2.42liter[/tex]
The answer is rounded to 3 significant figures, according to the data.
