The density of a sample of f2(g) is 1.559 g/l. if the gas is held at 755 torr, calculate the temperature.

how would i calculate the volume to use

The temperature is 590,10 K

Explanation:

As stated, we understand that there is one mole of F2, which is equivalent to 37.9968x2 grams = 75.936 grams. The unit of Torr is converted to atm, 1 Torr = 0.0013 atm, and with the data of grams it is converted into volume through density:

density = m / v ---> v = m / density = 75,936 g / 1,559 g / l = 48, 708 l

Exactly the formula PV = nRT

n = number of moles (according to what is interpreted in the sentence is 1 mole)

P = pressure 755 Torr (converted to atm 755Torr / 0.0013 atm / Torr = 0.99344 atm)

R = value constant 0.082 l x atm / K x mol

T = is our mystery (in degrees Kelvin)

0.99344 x 48, 708 l = 1 mol x 0.082 l x atm / K x mol x X

X = 0.99344 x 48, 708 l / 1 mol x 0.082 l x atm / K x mol

X = 590, 10 K

The temperature is 590.10 K

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