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?

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=

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.

3

explanation:

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