Question

# A flask at room temperature contains exactly equal amounts (in moles) of nitrogen and xenon. (MM...

A flask at room temperature contains exactly equal amounts (in moles) of nitrogen and xenon. (MM N2 = 28.01 g/mol, MM Xe = 131.3 g/mol) a. Which of the two gases exerts the greater partial pressure? BRIEFLY explain your answer. b. The molecules or atoms of which gas have a greater average speed? BRIEFLY explain your answer. c. If a small hole were opened in the flask, which gas would effuse more quickly? BRIEFLY explain your answer. d. The molecules or atoms of which gas have a greater kinetic energy? BRIEFLY explain your answer.

1) Solution-

Because the flask contains exactly equal amounts of both (in moles) of nitrogen and xenon, hence the partial pressure of the two gases will be the same.

b) Average velocity is inversely proportional to the molar mass the gas. .Therefore N2 will have the greater average speed.

c) Nitrogen because the molar mass is smaller than xenon

d) As we know that kinetic energy is directly proportional to the temperature. because the T is the same for both the gases, the average kinetic energy will be the same for both.

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