What is the velocity of 1.4 moles of bromine in a 3.5 l container at 4.35 atm?

Explanation:

Let the temperature at which gas is moving be T

Pressure exerted by the gas , P = 4.35 atm

Volume occupied by the gas ,V = 3.5 l

Moles of  bromine gas,n = 1.4 moles

Consider the bromine gas is behaving ideal .

Mass of bromine gas,M = Moles × Molar mass = 1.4 mole × 160 g/mol = 224 g = 0.224 kg

Value of R = 8.314 J/mol K

Root mean square velocity of the bromine gas:

Average velocity of the bromine gas:

Most probable velocity:

108

explanation:

ergfywefywefdwuduweefuy

a: 45.9 meters

b: 4.29 seconds

step-by-step explanation:

a: h(t)=1/2(-9.8)(3)^2+0(3)+90

h(t)=-4.9(3)^2+90

h(t)=-44.1+90

h(t)=45.9 meters

b: 0=1/2(-9.8)(t^2)+0t+90

0=-4.9t^2+90

-90=-4.9t^2

18.37=t^2

t=4.29 seconds

in the second question, the numbers aren't exact, but they're a close approximation.