A container of fixed volume has a mixture of three moles of hydrogen and two moles of helium in equilibrium at temperature T. Assuming the gases are ideal, the correct statement is

Total energy of three moles of hydrogen is $\frac{5}{2}3RT$

Total energy of two moles of helium is $\frac{3}{2}2RT$

Total energy of mixture is $\frac{15+6}{2}RT=\frac{21}{2}RT$

Average energy per mole of the mixture is $\frac{\frac{21}{2}RT}{2+3}=\frac{21}{10}RT$

Average kinetic energy per molecule of the mixture is $\frac{15+6}{2N}RT=\frac{21}{10}{k}_{B}T$

$v_{rms}=\sqrt{\frac{3RT}{M_W},}\frac{v_{He}}{v_H}=\sqrt{\frac{2}{4}}=\frac{1}{\sqrt{2}}$