Passage I

The molar volume of a gas is the volume occupied by 1 mole (mol; 6 × 1023 atoms or molecules) of that gas at a given pressure and temperature.

Table 1 shows how the molar volume, in L, of each of 6 gases—helium (He), neon (Ne), argon (Ar), hydrogen (H2), nitrogen (N2), and oxygen (O2)一varies with pressure, in atmospheres (atm), at a temperature of 273 Kelvins (K).

Table 2 shows how the molar volume of each of the 6 gases varies with temperature at a pressure of 1.00 atm.

6. Consider 2 separate 1 mol samples of O2, each at a pressure of 1 atm. One sample has a volume of about 18 L, and the other has a volume of about 63 L. Based on Table 2, the average kinetic energy of the O2 mole­cules is more likely greater in which sample?

Answer and Explanation

Your Answer is

Correct Answer is J

Explanation

Here we need to use a common sense of chemistry, that is, the average kinetic energy of a gas is only related to the temperature. The formula is KE=3/2RT. Looking at Table 2 longitudinally, it is found that the higher the temperature, the larger the volume of the same gas, so vice versa , so the higher the temperature of 63L, the higher the average kinetic energy