Answer:
91.33 L
Explanation:
For an ideal gas, the product between the gas pressure and the gas volume is proportional to the absolute temperature of the gas. Mathematically:
[tex]pV\propto T[/tex]
where:
p is the pressure of the gas
V is the volume of the gas
T is the absolute temperature of the gas
For a transformation of the gas, we can write:
[tex]\frac{p_1 V_1}{T_1}=\frac{p_2 V_2}{T_2}[/tex]
For the sample of krypton in this problem, we have:
[tex]p_1 = 5.54 atm[/tex] (initial pressure)
[tex]V_1 = 18.6 L[/tex] (initial volume)
[tex]T_1=35.0^{\circ}+273=308 K[/tex] (initial temperature)
[tex]p_2=1 atm[/tex] (final pressure, at stp)
[tex]T_2=0^{\circ}+273=273 K[/tex] (temperature at stp)
Therefore, the volume at stp is:
[tex]V_2=\frac{p_1 V_1 T_2}{T_1 p_2}=\frac{(5.54)(18.6)(273)}{(308)(1)}=91.33 L[/tex]
