A certain mass of nitrogen gas occupies a volume of 1.19 L 1.19 L at a pressure of 5.08 atm. 5.08 atm. At what pressure will the volume of this sample be 3.57 L? 3.57 L? Assume constant temperature and ideal behavior.

1.69atm

Explanation:

Data obtained from the question include:

V1 (initial volume) = 1.19 L

P1 (initial pressure) = 5.08 atm

V2 (final volume) = 3.57 L

P2 (final pressure) =.?

Since the temperature is constant, it means that the gas is obeying Boyle's law

Using the Boyle's law equation P1V1 = P2V2, the final pressure of the gas can be obtained as follow:

P1V1 = P2V2

5.08 x 1.19 = P2 x 3.57

Divide both side by 3.57

P2 = (5.08 x 1.19) / 3.57

P2 = 1.69atm

Therefore, the pressure will 1.69atm

1.693 atm

Explanation:

According to Boyle's Law, an inverse relationship exists between pressure and volume ... The relationship for Boyle's Law can be expressed as follows: P1V1 = P2V2, where P1 and V1 are the initial pressure and volume values, and P2 and V2 are the values of the pressure and volume of the gas after change under a constant temperature and ideal behaviour

P1V1 = P2V2

P1 = 5.08

V1 = 1.19L

P2=?

V2 = 3.57L

P1V1 = P2V2

5.08x 1.19 = P2 (3.57L)

6.0452/3.57 = P2 = 1.693 atm