Question

The total pressure inside a 1.43 L cylinder at 28C is 1.03 atm. If the temperatures drops to -35C, and the volume remains the same, what is the new pressure inside the cylinder?

Answer 1

Answer:

0.81452 atm

Explanation:

$P_1$ = Initial pressure = 1.43 L

$V_1=V_2$ = Volume

$T_1$ = Initial temperature = (28+273.15)  K

$T_2$ = Final temperature = (-35+273.15) K

$P_2$ = Final pressure

From the ideal gas law we have

$\dfrac{P_1V_1}{T_1}=\dfrac{P_2V_2}{T_2}\\\Rightarrow P_2=\dfrac{P_1V_1T_2}{T_2V_2}\\\Rightarrow P_2=\dfrac{1.03\times 1.43\times (273.15-35)}{(273.15+28)1.43}\\\Rightarrow P_2=0.81452\ atm$

The pressure in the cylinder is 0.81452 atm