Question

A vessel contains 1.6 g of dioxygen at STP (273.15K, 1 atm pressure). The gas is now transferred to another vessel at constant temperature, where pressure becomes half of the original pressure. Calculate volume of the new vessel.

Answer 1

Initial pressure of \[\ce{O2(P1)}\] = 1 atm

Initial temperature of \[\ce{O2(T1)}\] = 273. 15 K

32 g of oxygen occupies 22.4 L of volume at STP. So, 1.6 g of oxygen will occupy as follows,

initial volume of \[\ce{O2(V1)}\] = `(22.4  L)/(32  g) xx 1.6  g` = 1.12 L

Final pressure \[\ce{(P2)}\] is the half of the original pressure \[\ce{(P1)}\].

Thus, P₂ = `1/2` atm

To Bolye's law,

\[\ce{P1V1 = P2V2}\]

Now, substituting the known values in the above equation,

1 atm × 1.12 L = `1/2` atm × V₂

V₂ = 2.24 L

Thus, the volume of the new vessel is 2.24 L.