The particles of two samples of different gases, nitrogen and hydrogen, have the

Question

The particles of two samples of different gases, nitrogen and hydrogen, have the same average speeds. Which of the two samples has the greater temperature? Explain. Two tanks containing an equal number of moles of an ideal gas are at equal temperatures. The volume of tank F is greater than the volume of tank E. Is the average speed of the particles in tank F greater than, less than, or equal to the average speed of the particles in tank E? Is the average change in momentum of one gas particle in a single collision with a wall in tank F greater than, less than, or equal to the average change in momentum of one particle in a single collision with a wall in tank E? Explain. On average, will a single particle collide with a wall more, less, or equally often in tank F than in tank E? Explain. Is the number of particles colliding with a wall per unit time and unit area in tank F greater than, less than, or equal to the number of particles colliding with a wall per unit time and unit area in tank E? Explain. Use your answers to parts b and c above to predict whether the pressure in tank B is greater than, less than, or equal to the pressure in tank A. Is your answer consistent with the ideal gas law?

Explanation / Answer

1) as the average speed of the gases is given as

average speed = sqrt(8 * R* T/(pi * M))

as the mass M of Hydrogen and Nitrogen ,

for the average speed to be same

sqrt(T/M) must be same

hence , the temperature of the gas Nitrogen must be higher than Hydrogen

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