Question

if a gas at 25.0 °C occupies 3.60 liters at a pressure of 104.3kPa what will be its volume at a pressure of 2.50atm

Answer 1

From the question, we will need to assume the temperature don't change.

In this case, assuming the gas behaves as an ideal gas, we can use the Boyle's Law to answer.

The Boyle's Law says that the product of the pressure and volume of an ideal gas, at constant temperature, is a constant:

`pV=k`

But the volume and pressure have to be on the same unit.

First, lets convert the final pressure of 2.50 atm to kPa. We can do that by multiplying the atm value by 101.325:

`p_2=2.50atm=2.50\cdot101.325kPa=253.3125kPa`

Now, we can apply the Boyle's Law:

`\begin{gathered} p_1V_1=k \\ p_2V_2=k \\ p_2V_2=p_1V_1_{} \\ V_2=\frac{p_1V_1}{p_2_{}}=(104.3kPa\cdot3.60L)/(253.3125kPa)=1.4822\ldots L\approx1.48L_{} \end{gathered}`

So, its volume will be approximately 1.48 L.