A sealed container contains 0.10 moles of nitrogen gas and 0.20 moles of oxygen gas. If Temperature of the mixture is constant, which of the followimg is true

a Molecular Masses of 2 gases are the same.

b Partial pressures of the two gases are same

c Average Kinetic energies of the two gases are same.

Question

Tripp Simpson

Chemistry

5 March, 21:03

A sealed container contains 0.10 moles of nitrogen gas and 0.20 moles of oxygen gas. If Temperature of the mixture is constant, which of the followimg is true

a Molecular Masses of 2 gases are the same.

b Partial pressures of the two gases are same

c Average Kinetic energies of the two gases are same.

+5

Answers (2)

Know the Answer?

Jaida · Answer 1

The answer to your question is C.

Sydney Simon · Answer 2

c. The average kinetic energies of the two gases are the same.

Step-by-step explanation:

A major postulate of the Kinetic Molecular Theory is that the average kinetic energies of all gases are the same at the same temperature.

a. is wrong. N₂ and O₂ are different elements with different molar masses.

b. is wrong. According to Avogadro's Law, the partial pressure varies directly as the number of moles. There are twice as many molecules of O₂ as of N₂, so p (O₂) = 2p (N₂).

A sealed container contains 0.10 moles of nitrogen gas and 0.20 moles of oxygen gas. If Temperature of the mixture is constant, which of the followimg is truea Molecular Masses of 2 gases are the same.b Partial pressures of the two gases are samec Average Kinetic energies of the two gases are same.