What is the effect of temperature change on the Boyle's law isotherm graph?

At $25 \, ^\circ C$,a $3.7 \, g$ gas occupies the same volume as $0.184 \, g$ of $H_2$ gas at $17 \, ^\circ C$ under the same pressure. What is the molar mass of the gas?

At $STP$,$2 \ mol$ of $N_2$ gas in a $50 \ L$ container exhibits:

At $25 \, ^\circ C$ temperature and $760 \, mm \, Hg$ pressure,the volume of a gas is $600 \, mL$. Calculate the pressure when the volume of this gas becomes $640 \, mL$ at $10 \, ^\circ C$ temperature. Use the ideal gas equation: $\frac{p_1 V_1}{T_1} = \frac{p_2 V_2}{T_2}$

At a constant pressure $p$,the plot of volume $(V)$ as a function of temperature $(T)$ for $2 \, mol$ of an ideal gas gives a straight line with a slope $0.328 \, L \, K^{-1}$. The value of $p$ (in $atm$) is closest to
[Gas constant,$R=0.0821 \, L \, atm \, mol^{-1} \, K^{-1}$ ]

At a temperature of $27\,^oC$,a $2.461 \, L$ vessel contains $0.3 \, mol$ of $N_2$,$0.5 \, mol$ of $He$,and $6.2 \, mol$ of $O_2$ gases. What is the partial pressure of $N_2$ in $atm$?