Question

equimolar samples of n2 and o2 are both at standard conditions (1 atm, 273k). a) which sample has more kinetic energy? why?

Answer 1

The gas that has more kinetic energy is nitrogen.

Which sample has a greater kinetic energy?

We know that from the ideal gas equation, the molecules that compose a gas are in constant random motion. The implication of this is that, the kinetic energy of the molecules of the gas would depend on the velocity of the molecules of the gas.

Since we can not measure the individual velocities of the molecules of a gas but we can be able to measure the root mean square speed of the molecules of the gas as we can see.

This root mean square velocity is going to depend on the molar mass of the gas as well as the temperature of the system. Where the system is at the same temperature, the greater the molar mass, the lesser the kinetic energy of the gas.

Nitrogen ($N_{2}$) has a molar mass of 28 g/mol while oxygen ($O_{2}$) has a molar mass of 32 g/mol.

Learn more about kinetic energy of a gas:https://brainly.com/question/4320273

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