A gas has a volume of 300 mL at 300 mm Hg. What will its volume be if the pressure is changed to 500 mm Hg?

Question

17786 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2016-05-30T19:32:12

$V_{2} = 180 m L$ $V_2=180mL$

For this question, we will issue that the change happens at constant temperature and that the gas behaves ideally.

Thus, we can use the ideal gas law: $P V = n R T$ $PV=nRT$

Since the change is occurring at constant temperature and number of mole, we can modify the ideal gas law as follows:

$P V = k$ $PV=k$ where, $k = n R T$ $k=nRT$ .

For position 1: we have $P_{1}$ $P_1$ and $V_{1}$ $V_1$ .

For position 2: we will have $P_{2}$ $P_2$ and $V_{2}$ $V_2$ .

Since $P V = k$ $PV=k$ we can write $P_{1} V_{1} = P_{2} V_{2}$ $P_1V_1=P_2V_2$ .

Therefore, $V_{2} = \frac{P_{1} V_{1}}{P_{2}}$ $V_2=(P_1V_1)/(P_2)$

$=>V_2=(300cancel(mmHg)xx300mL)/(500cancel(mmHg))=180mL$