A jar contains a mixture of nitrogen and oxygen gases. The average kinetic energies of the molecules of nitrogen and oxygen are E1 and E2 respectively. Then, (E1/E2)=

Question

A jar contains a mixture of nitrogen and oxygen gases. The average kinetic energies of the molecules of nitrogen and oxygen are E1 and E2 respectively. Then, (E1/E2)= (A) 6 (B) 28 (C) 32 (D) 1

Tardigrade Admin · Accepted Answer

E=(3/2) k ⋅ T E is independent of molecular mass and depends on temperature only. Thus, (E1/E2)=1 as nitrogen and oxygen when mixed will be at same temperature.

Q. A jar contains a mixture of nitrogen and oxygen gases. The average kinetic energies of the molecules of nitrogen and oxygen are $E_{1}$ and $E_{2}$ respectively. Then, $\frac{E _{1}}{E _{2}} =$

6

28

32

1

$E = \frac{3}{2} k \cdot T$
$E$ is independent of molecular mass and depends on
temperature only. Thus, $\frac{E _{1}}{E _{2}} = 1$ as nitrogen and oxygen when mixed will be at same temperature.

Q. A jar contains a mixture of nitrogen and oxygen gases. The average kinetic energies of the molecules of nitrogen and oxygen are E1​ and E2​ respectively. Then, E2​E1​​=

6

28

32

1

E=23​k⋅T E is independent of molecular mass and depends on temperature only. Thus, E2​E1​​=1 as nitrogen and oxygen when mixed will be at same temperature.

Q. A jar contains a mixture of nitrogen and oxygen gases. The average kinetic energies of the molecules of nitrogen and oxygen are $E_{1}$ and $E_{2}$ respectively. Then, $\frac{E _{1}}{E _{2}} =$

$E = \frac{3}{2} k \cdot T$
$E$ is independent of molecular mass and depends on
temperature only. Thus, $\frac{E _{1}}{E _{2}} = 1$ as nitrogen and oxygen when mixed will be at same temperature.