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

C. 3.74 g/L

Explanation:

Using ideal gas equation as:

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:

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

the molecules move in straight line until they collide with each other or with the walls of the container. collisions are perfectly elastic; when two molecules collide, they change their directions and kinetic energies, but the total kinetic energy is conserved.

explanation: