Question

1. A sample of argon at a pressure of 785 mm Hg is transferred from a 125 ml dask to a 15 ml
Assuming constant temperature, what is the pressure inside the 155 mL flask?

Answer 1

Answer:

The pressure of argon inside the 155 ml flask is approximately 633 mm Hg.

Explanation:

Given:

The temperature is constant. So, the process is isothermal.

Initial pressure of argon is, $P_1=785\ mm\ Hg$

Initial volume of argon is, $V_1=125\ ml$

Final volume of argon is, $V_2=155\ ml$

Final pressure of argon is, $P_2=?$

Now, as per Boyle's law, for an isothermal process, the product of pressure and volume is always a constant or $PV=constant$. Therefore, we can write it as:

$P_1V_1=constant\\P_2V_2=constant\\\therefore P_1V_1=P_2V_2$

Rewriting the above in terms of $P_2$, we have:

$P_2=\frac{P_1V_1}{V_2}$

Plug in 785 for $P_1$, 125 for $V_1$, 155 for $V_2$ and solve for $P_2$. This gives,

$P_2=\frac{785\times 125}{155}\\P_2=633.06\approx 633\ mm\ Hg$

Therefore, the pressure of argon inside the 155 ml flask is approximately 633 mm Hg.