Two one liter containers, one containing 6.0 times 10^5 atoms of Helium (M = 4 g

Question

Two one liter containers, one containing 6.0 times 10^5 atoms of Helium (M = 4 grams/mole), and the other 6.0 times 10^5 molecules of diatomic nitrogen (N_2) (M = 28 grams/mole). If both are at the same temperature, which of the following is true? Both containers contain the same mass of gas. the mean free path for the Helium is the same as for the Nitrogen. V_rms is the same for both gases V_most probable is the same for both gases. the pressure is the same for both containers Which explains how water can evaporate from a glass at room temperature (-22 degree C)? V_rms of the water is greater than the speed for 100 degree C water as a gas V_most probable of the water is greater than the speed for 100 degree C water as a gas the tail of the Maxwellian velocity distribution ensures some of the water molecules have the speed necessary to escape the liquid. According to the phase diagram, there is a natural tendency for water to vaporize at room temperature.

Explanation / Answer

(14) volume of both gases is same. number of atoms is also same.temperature is also same

According to Avagadro's law, "equal volumes of gases at the same temperature and pressure contain equal numbers of molecules"

since n, T and V is same, the pressure is same for both containers.so option e is correct..

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