What is the mass of a 202.6 mL sample of hydrogen chloride gas at -12.4^{o}C 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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