Question

A sample of helium gas at a pressure of 772 torr and a temperature of 22.7 °C, occupies a volume of 814 mL. If the gas is allowed to expand at constant temperature until its pressure is 549 torr, the volume of the gas sample will be mL.

A sample of argon gas at a pressure of 697 torr and a temperature of 26.4 °C, occupies a volume of 448 mL. If the gas is compressed at constant temperature until its pressure is 858 torr, the volume of the gas sample will be  mL.

A sample of hydrogen gas at a pressure of 0.521 atm and a temperature of 25.3°C, occupies a volume of 12.9liters. If the gas is allowed to expand at constant temperature to a volume of 22.1 liters, the pressure of the gas sample will be  atm.

Answer 1

a. Initial                                         Final

     P1 = 772torr                           P2 = 549torr

     V1 = 814ml                             V2 =

     T1   = 22.7+273 = 295.7K       T2 = 22.7+273 = 295.7K

           P1V1/T1     =   P2V2/T2

                 V2         =     P1V1T2/P2T1

                               = 772*814*295.7/549*295.7    = 1144.64ml

b.

Initial                                         Final

     P1 = 697torr                           P2 = 858torr

     V1 =448ml                             V2 =

     T1   = 26.4+273 = 299.4K       T2 = 26.4+273 = 299.4K

           P1V1/T1     =   P2V2/T2

                 V2         =     P1V1T2/P2T1

                                = 697*448*299.4/858*299.4   = 363.93ml >>>>answer

c.

Initial                                                  Final

P1   = 0.521atm                                P2 =

V1 = 12.9L                                        V2 = 22.1L

T1   = 25.3+273 = 298.3K                 T2 = 25.3+273 = 298.3K

                 P1V1/T1    =    P2V2/T2

                      P2         =    P1V1T2/T1V2

                                    =   0.521*12.9*298.3/298.3*22.1    = 0.304atm >>>>answer