What is happening with the temperature of a sample of methane gas, if 1 litre at $735$ torr and $25.0^oC$ is compressed with a pressure of $1.8$ bar to a volume of 0.9 litres?
760 torr = 1 atm 1 atm = 1.013 bar
$P_1$ $=$ $\frac{735}{760}atm$ $P_2$ $=$ $\frac{1,8}{1,013}atm$ $\frac{P_1V_1}{T_1}$ $=$ $\frac{P_2V_2}{T_2}$ $T_2$ $=$ $\frac{P_2V_2T_1}{P_1V_1}$ $=$ $\frac{1.8\cdot 0.9\cdot 298\cdot 760}{1.013\cdot 735\cdot 1}$ $=$ $492.77K$ $t$ $=$ $219.62^oC$
