Question

A chemist prepares a sample of hydrogen bromide and finds that it occupies 216 ml at 64 c and 535 torr. what volume would it occupy at0 c at the same pressure? answer in units of ml

Answer 1

PV=nRT

P₁=P₂=535 torr=71327.5 Pa

V₁=216ml=0.000216 m³

T₁=64 °C=337 K

T₂=0°C=273 K

R=8.31 J/(mole K)

$n=\frac{P_1V_1}{RT_1}=\frac{71327.5x0.000216}{8.31x337}=0.0055 mole$

$V_2=\frac{nRT_2}{P_2}=\frac{0.0055x8.31x273}{71327.5}=0.000175 m^3=175 ml$