Question

At 27 degrees C and 750 mmhg a sample of hydrogen occupies 5.0 L how much space will occupy at STP​

Answer 1

Step-by-step explanation:

The number of mole of the hydrogen sample at 27 C and 750 mmHg pressure is:

`n=(PV)/(RT)=((0.9898* 10^(5))(5* 10^(-3)))/((8.314)(27+273))\approx 0.0198` mol

This number of mole will be the same although we change the pressure and temperature. For STP (Temperature = 0 C = 273 K, and Pressure = 760 mmHg = 76 cmHg = 1 Bar = 1.01 x
`10^(5)` Pa):

`P'V'=nRT' \rightarrow V'=(nRT')/(P')=(0.0198(8.314)(273))/(1.01* 10^(5))\approx 44.49 * 10^(-5)` in
`m^(3)`. But in L, we find that V' = 0.4449 L