Answer:
True...I think I'm not sure
Hey There!:
Molar mass O2 => 32.0 g/mol
Molar mass Cl2 => 71.0 g/mol
effusion rate α 1 / (√ molar mass )
E Cl2 / E O2 = √ molar mass O2 / √ molar mass Cl2
E Cl2 / E O2 = ( √ 32.0 ) / ( √ 71.0 )
=> 0.671
Hope that helps!
the elasticity of gas particle collisions, there is no energy loss when the particles pass one another. Gases are composed of a very large number of small particles, which spread out and avoid contact with one another.
<h3>Which of the following gas postulates from the kinetic molecular theory best explains why pressure exists in gases?</h3>
As the quantity of gas particles in the container rises, so does the frequency of wall interactions and subsequently the pressure of the gas. The average kinetic energy of a gas particle is exclusively dependent on the temperature of the gas, says the theory's final postulate. As the volume of gas particles inside the container grows, more of them will collide with the walls, increasing the pressure and the frequency of collisions.
Learn more about kinetic energy here:
brainly.com/question/26472013
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My solution
39.0983+126.90447=166.00277
x/166.002277=.06
x=9.96g
Explanation:
A and C are the only two places that would represent the oldest rocks