Sulfur hexafluoride gas is collected at 26.0 °C in an evacuated flask with a measured volume of 35.0 L. When all the gas has been collected, the pressure in the flask is measured to be 0.300 atm . Calculate the mass and number of moles of sulfur hexafluoride gas that were collected. Be sure your answer has the correct number of significant digits. mass: s mole

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Mergus Mergus · Answer 1 · 2019-12-07T09:11:59+01:00

Answer:

Moles of sulfur hexafluoride gas = 0.428 moles

Mass of sulfur hexafluoride gas = 62.5 g

Explanation:

Given that:

Pressure = 0.300 atm

Temperature = 26 °C

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15

So,

T = (26 + 273.15) K = 299.15 K

Volume = 35.0 L

Using ideal gas equation as:

[tex]PV=nRT[/tex]

where,

P is the pressure

V is the volume

n is the number of moles

T is the temperature

R is Gas constant having value = 0.0821 L.atm/K.mol

Applying the equation as:

0.300 atm × 35.0 L = n × 0.0821 L.atm/K.mol × 299.15 K

⇒n = 0.4275 moles

Moles of sulfur hexafluoride gas = 0.428 moles

Molar mass of sulfur hexafluoride gas = 146.06 g/mol

The formula for the calculation of moles is shown below:

[tex]moles = \frac{Mass\ taken}{Molar\ mass}[/tex]

Thus,

[tex]0.428= \frac{Mass}{146.06\ g/mol}[/tex]

Mass of sulfur hexafluoride gas = 62.5 g