Question

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

Answer 1

`2.42liter`

Step-by-step 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?

Solution

Since the amount of gas and the temperature remain constant, we may use Boyle's law:

`PV=constant\\\\P_1V_1=P_2V_2`

Form the data:

`P_1=1.20atm\\\\P_2=703torr\\\\V_1=unknown\\\\V_2=V_1+0.720liter`

1. Convert 703 torr to atm:

`P_2=703torr* 1atm/760torr=0.925atm`

2. Sustitute the data in the equation:

`1.2atm* V_1=0.925atm*(V_1+0.720liter)`

3. Solve:

`1.2V_1=0.925V_1+ 0.666liter\\\\0.275V_1=0.666liter\\\\V_1=2.4218liter\approx 2.42liter`

The answer is rounded to 3 significant figures, according to the data.