At what temperature will 5.00 g of F2, exert a pressure of 119.96 kPa at a volume of 750.0 mL?

-183.15 °C

Explanation:

Given data:

Mass of F₂ = 5.00 g

Pressure = 119.96 KPa (119.96/101 = 1.2 atm)

Volume = 750.0 mL ( 750.0/1000 = 0.75L)

Temperature = ?

Solution:

First of all we will calculate the number of moles.

Number of moles = mass/molar mass

Number of moles = 5.00 g/ 38g/mol

Number of moles = 0.13 mol

Now we will calculate the temperature:

PV = nRT

P= Pressure

V = volume

n = number of moles

R = general gas constant = 0.0821 atm.L/ mol.K  

T = temperature in kelvin

1.2 atm × 0.75 L = 0.13 mol ×0.0821 atm.L/ mol.K  × T

0.9 atm.L = 0.01 atm.L/ K  × T

T = 0.9 atm.L /0.01 atm.L/ K

T = 90 K

Kelvin to degree celsius:

90K -273.15 = -183.15 °C