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A gas has a sample initial pressure of 1.24 atm and an initial volume of 0.671 L. What is the pressure (in torr) if the final volume of the gas is changed to 583. mL? Assume constant temperature and amount of gas.

Respuesta :

Answer:

1086.8 torr

Explanation:

Using Boyle's law  

[tex]{P_1}\times {V_1}={P_2}\times {V_2}[/tex]

Given ,  

V₁ = 0.671 L  

V₂ = 583 mL = 0.583 L ( 1 mL = 0.001 L )

P₁ = 1.24 atm

P₂ = ?

Using above equation as:

[tex]{P_1}\times {V_1}={P_2}\times {V_2}[/tex]

[tex]{1.24\ atm}\times {0.671\ L}={P_2}\times {0.583\ L}[/tex]

[tex]{P_2}=1.43\ atm[/tex]

The conversion of P(atm) to P(torr) is shown below:

[tex]P(atm)={760}\times P(torr)[/tex]

So,  

Pressure = 1.43*760 torr = 1086.8 torr

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