Question

Assuming ideal behavior, one mole krypton gas is released into flexible container at STP. What is the density of Krypton gas in this container at STP? At STP one mole of any gas occupies 22.4 L. (R = 0.08206 L • atm/K • mol) Atomic mass of krypton is 83.8 AMU. Select one: A. 0.0561 g/L B. 0.0176 g/L C. 3.74 g/L D. 181 g/L E. 1.78 g/L

Answer 1

C. 3.74 g/L

Step-by-step explanation:

Using ideal gas equation as:

`PV=nRT`

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

Also,

Moles = mass (m) / Molar mass (M)

Density (d) = Mass (m) / Volume (V)

So, the ideal gas equation can be written as:

`PM=dRt`

At STP,

Pressure = 1 atm

Temperature = 273.15 K

Molar mass of krypton gas = 83.8 g/mol

Applying the equation as:

1 atm × 83.8 g/mol = d × 0.0821 L.atm/K.mol × 273.15 K

⇒d = 3.74 g/L