Which of the following statements is true for ideal gases, but is not always tru

Question

Which of the following statements is true for ideal gases, but is not always true for real gases?
Choose all that apply?

The size of the molecules is unimportant compared to the distances between them.

Collisions between molecules are elastic.

There are no attractive forces between molecules.

Average molecular kinetic energy increases with temperature.

Which of the following statements is true for real gases?
Choose all that apply?

As molecules increase in size, deviations from ideal behavior become more apparent at relatively low pressures.

As molecules increase in size, deviations from ideal behavior become more apparent at relatively high pressures.

Attractive forces between molecules cause an increase in pressure compared to the ideal gas.

The volume occupied by the molecules can cause an increase in pressure compared to the ideal gas.

The average molecular speed in a sample of N2 gas is 485 m/s at 311 K. The average molecular speed in a sample of O2gas is ?m/s at the same temperature.

The rate of effusion of NH3 gas through a porous barrier is observed to be 6.90E-4 mol / h. Under the same conditions, the rate of effusion of CH4 gas would be ?mol / h.

Explanation / Answer

Which of the following statements is true for ideal gases, but is not always true for real gases?
Choose all that apply?

The size of the molecules is unimportant compared to the distances between them. (TRUE for R.G)

Collisions between molecules are elastic. (FALSE for R.G)

There are no attractive forces between molecules. (FALSE for R.G)

Average molecular kinetic energy increases with temperature. (TRUE for R.G and I.G)

Which of the following statements is true for real gases?
Choose all that apply?

As molecules increase in size, deviations from ideal behavior become more apparent at relatively low pressures. (FALSE for R.G.)

As molecules increase in size, deviations from ideal behavior become more apparent at relatively high pressures. (TRUE for R.G.)

Attractive forces between molecules cause an increase in pressure compared to the ideal gas. (FALSE for R.G.)

The volume occupied by the molecules can cause an increase in pressure compared to the ideal gas. (TRUE for R.G.)

The average molecular speed in a sample of N2 gas is 485 m/s at 311 K. The average molecular speed in a sample of O2gas is ?m/s at the same temperature.

V = sqrt(3*R*T/MW)

R = 8314

T = 311

MW = molecular weigth = 32

V = sqrt(3*8314*311/32) = 492 m/s

V O2 = 492 m/s

The rate of effusion of NH3 gas through a porous barrier is observed to be 6.90E-4 mol / h. Under the same conditions, the rate of effusion of CH4 gas would be ?mol / h.

Apply Graham Law

Rate1 / Rate2 = sqrt(MW2/MW1)

6.9*10^-4 / (Rate2) = sqrt(16/17)

Rate 2 = (6.9*10^-4 )/(0.97) = 0.007113 or 7.11*10^-4

Rate of CH4 = 7.11*10^-4

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