Question

The molar mass of hydrogen molecules is 2g/mol and the molar mass of oxygen molecules is 32g/mol. What is the ratio of the average kinetic energy of the molecules of 1 mole of hydrogen gas at 300K to 1 mole of oxygen gas at a temperature of 300K, assuming they both behave as ideal gases?

Answer 1

The ratio of the average kinetic energy of 1 mole of hydrogen gas to 1 mole of oxygen gas at 300K is 1:1, assuming they both behave as ideal gases.

Step-by-step explanation:

The average kinetic energy (average KE) of a gas molecule at a particular temperature is given by the equation: average KE = (3/2)kT, where k is the Boltzmann constant and T is the temperature in Kelvin. Since the temperature (T) for both hydrogen (H2) and oxygen (O2) gases is the same at 300K, and since the average kinetic energy of a gas molecule depends only on the temperature for an ideal gas, the ratio of the average kinetic energy of 1 mole of hydrogen gas to 1 mole of oxygen gas at 300K is 1:1.

Answer 2

1

Step-by-step explanation:

For an ideal gas, the average kinetic energy is given by:

Ek = (3/2)*n*R*T

Where n is the number of moles, R is the gas constant (8.31 J/mol*K), and T the temperature. The gases have the same number of moles, and the same temperature, so they will have the same average kinetic energy:

Ek = (3/2)*1*8.31*300

Ek =3739.5 J

So, the ratio between then is 1.