9. Change 500.0 mL of a gas at 60.0° C and 800.0 torr to standard conditions. 10
ID: 565129 • Letter: 9
Question
9. Change 500.0 mL of a gas at 60.0° C and 800.0 torr to standard conditions. 10. Change 800.0 mL at 40.0° C and 700.0 mm to standard conditions. I1. Change 60.0 mL at standard conditions to 55° C and 745 torr. 12. Change 35 mL at standard conditions to 25° C and 725 torr. 13. Change 50.0 mL at standard conditions to 43° C and 750 mm 14. Change 75.0 mL at 100.0° C and 450 torr to standard conditions. 15. Change 10.0 mL at 27° C and 1.25 atm to standard conditions. 16. Change 250 mL at 32° C and 750 torr to 47° C and 780 torr.Explanation / Answer
9.
According to ideal gas equation, PV = nRT and for two cases for same gas,
P1V1/n1T1 = P2V2/n2T2
P1 = initial pressure = 800 torr
V1 = initial volume = 500 mL
n1 = initial number of moles = n
T1 = initial temperature = 60 0C = 60+273 = 333 K
P2 = Final Pressure = 760 torr
V2 = Final volume = ?
n2 = Final number of moles = n
T2 = Final Temperature = 0+273 = 273K
from the formula,
800 * 500/n*333 = 760*V2/n*273
V2 = 431.484 mL
10.
According to ideal gas equation, PV = nRT and for two cases for same gas,
P1V1/n1T1 = P2V2/n2T2
P1 = initial pressure = 700 torr
V1 = initial volume = 800 mL
n1 = initial number of moles = n
T1 = initial temperature = 40 0C = 40+273 = 313 K
P2 = Final Pressure = 760 torr
V2 = Final volume = ?
n2 = Final number of moles = n
T2 = Final Temperature = 0+273 = 273K
11.
According to ideal gas equation, PV = nRT and for two cases for same gas,
P1V1/n1T1 = P2V2/n2T2
P1 = initial pressure = 760 torr
V1 = initial volume = 60 mL
n1 = initial number of moles = n
T1 = initial temperature = 0 0C = 0+273 = 273 K
P2 = Final Pressure = 745 torr
V2 = Final volume = ?
n2 = Final number of moles = n
T2 = Final Temperature = 55+273 = 328K
from the formula,
760 * 60/(n*273) = 745*V2/(n*328)
V2 = 73.5393 mL
12.
According to ideal gas equation, PV = nRT and for two cases for same gas,
P1V1/n1T1 = P2V2/n2T2
P1 = initial pressure = 760 torr
V1 = initial volume = 35 mL
n1 = initial number of moles = n
T1 = initial temperature = 0 0C = 0+273 = 273 K
P2 = Final Pressure = 725 torr
V2 = Final volume = ?
n2 = Final number of moles = n
T2 = Final Temperature = 25+273 = 298K
from the formula,
760 * 35/(n*273) = 725*V2/(n*298)
V2 = 40.0495 mL
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