What is the mass of a 202.6 mL sample of hydrogen chloride gas at -12.4oC and 184.26 kPa.
A sample of hydrogen has a volume of 1143 mL when the temperature is 225.3 degC and the pressure is 1.061 atm. What will be the volume of the gas at STP?
Find The volume at STP
202.6 x 184.26/ 260.75 = V x 101.325/273.15
V= 202.6 x 184.26/ 101.325 x 273.15/ 260.75
= 385.95 ml
Now 1 mole of HCL (22.4 l) at STP weighs 36.44g
so 385.95 ml of HCL at STP weighs 36.44 x 0.386/22.4 = 0.628 g
Again use P1V1/T1 = P2V2/T2
1.061 x 1143/ 498.45 = 1 x V2/ 273.15
2.433 x 273.15 = V2
V2 =664.57 ml
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