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
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"
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