At what temperature will hydrogen molecules have the same kinetic energy as nitrogen molecules have at ${35}^{\circ }C$ ?

Since we are aware, the root denotes square velocity $\left({\mathrm{V}}_{\mathrm{rms}}\right)$ of a gas is given by-

$V_{\mathrm{rms}}=\sqrt{\frac{3\mathrm{RT}}{\mathrm{M}}}$

Consequently, nitrogen's root means square velocity at ${35}^{\circ }C$

Molar mass of nitrogen $\left(M\right)=28 \mathrm{g}$

Temperature $\left(\mathrm{T}\right)={35}^{\circ }\mathrm{C}=(35+273)\mathrm{K}=308\mathrm{K}$

$\therefore {\mathrm{V}}_{{\mathrm{N}}_2}=\sqrt{\frac{3\mathrm{R}\times 308}{28}}$

Root-mean-square hydrogen velocity at temperature  will have the same as of nitrogen at ${35}^{\circ }C$.