Question

A balloon is filled to a volume of 1.50 L with 3.00 moles of gas at 25 °C. With pressure and temperature held constant, what will be the volume (in L) of the balloon if 0.50 moles of gas are released?

Answer 1

Answer:

Volume : 1.25 L

Explanation:

We are given here that the volume ( V$_1$ ) = 1.50 Liters, the initial moles ( held at 25 °C ) = 3.00 mol, and the final moles ( n$_2$ ) = 3.00 - 0.5 = 2.5 mol. The final mol is calculated given that 0.50 mol of gas are released from the prior 3.00 moles of gas.

Volume ( V$_1$ ) = 1.50 L,

Initial moles ( n$_1$ ) = 3.00 mol,

Final Volume ( n$_2$ ) = 3.00 - 0.5 = 2.5 mol

Applying the combined gas law, we can calculate the final volume ( V$_2$ ).

P$_1$V$_1$ / n$_1$T$_1$ = P$_2$V$_2$ / n$_2$T$_2$ - we know that the pressure and temperature are constant, and therefore we can apply the following formula,

V$_1$ / n$_1$ = V$_2$ / n$_2$ - isolate V$_2$,

V$_2$ = V$_1$ n$_2$ / n$_1$ = 1.50 L $*$ 2.5 mol / 3.00 mol = ( 1.5 $*$ 2.5 / 3 ) L = 1.25 L

The volume of the balloon will be 1.25 L.