# A sample of oxygen gas has a volume of 150.0 mL at a pressure of 0.947 atm. What will the volume of the gas be at a pressure of 1.000 atm if the temperature remains constant?

Mar 6, 2016

$142.05 m L$

#### Explanation:

From the information given for this question, we can see that this kind of situation is involving Boyle's Law.

Boyle's Law states that the pressure of a fixed mass of gas at a constant temperature is inversely proportional to its volume .

In which from the definition, the equation is derived as;

$P \quad \propto \quad \frac{1}{V}$ or $P = \frac{k}{V}$ or $P V = k$

$P =$ Pressure of gas
$V =$ Volume of gas
$k =$ Constant

When there are two situations , given initial and final value of both pressure and volume, the equation is derived as;

${P}_{i} {V}_{i} = {P}_{f} {V}_{f}$

From the information given in this question;

${P}_{i} =$ Initial pressure of gas $= 0.947 a t m$
${P}_{f} =$ Final pressure of gas $= 1.000 a t m$
${V}_{i} =$ Initial volume of gas $= 150 m L$
${V}_{f} =$ Final volume of gas =?mL

Calculating ${V}_{f}$;

$\left(0.947 a t m\right) \left(150 m L\right) = \left(1.000 a t m\right) {V}_{f}$

${V}_{f} = \frac{142.05 \cancel{a t m} m L}{1.000 \cancel{a t m}}$

${V}_{f} = 142.05 m L$