The ideal gas law

Tutorial 2

                

To how many atmospheres must be compressed $ 1.00\;L $ of a gas at $-10\;^oC $ and $1.00\;atm $ to bring it to $ 0.20 \; L $ at $ 0\;^oC $? Solution (Click): Conversion to Kelvin: ..........$T_1=$ $\color{red}273.15\; K$
$T_2=$ $\color{red}263.15\; K$ The ideal gas law: ..........$\frac{P_1\cdot V_1 }{T_1}=\frac{P_2\cdot V_2 }{T_2}$ Calculation: ..........$P_1=\frac{T_1\cdot V_2\cdot P_2}{T_2\cdot V_1}$ = $\frac{273.15 \cdot 1.00 \cdot 1.00}{263.15 \cdot 0.20} = 5.19\;atm$