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

Answer:

Explanation:

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

$n=\frac{PV}{RT}=\frac{(0.9898\times 10^{5})(5\times 10^{-3})}{(8.314)(27+273)}\approx 0.0198$ 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):

$P'V'=nRT' \rightarrow V'=\frac{nRT'}{P'}=\frac{0.0198(8.314)(273)}{1.01\times 10^{5}}\approx 44.49 \times 10^{-5}$ in $m^{3}$. But in L, we find that V' = 0.4449 L