Question

If a nitrogen gas occupies a volume of 500 ml at a pressure of .971atm. What volume will the gas occupy at a pressure of 1.50 atm, assuming the temperature remains constant?

Answer 1

Knowing the two variables in this problem are volume (liter) and pressure (atm), we can determine that the law ought to be used would be Boyle's Law.

Boyle's Law: P₁v₁=P₂V₂

Using the question, we can find:

P₁ (initial pressure)=0.971 atm

V₁ (initial volume)=500ml

P₂ (standard pressure)= 1.50atm

V₂=?

We can rearrange the equation to solve for V₂: V₂=P₁V₁/P₂

Next, we can plug in the values: V₂=$\frac{0.971atm*500mL}{1.50atm}$

We would receive an answer of 323.67 L. However, it appears that the significant digits would be 3 as both 0.971 and 1.50 have 3 digits. As such, the answer would be 324 Liters of gas at 1.50atm.