If o2 is bubbled through water at 393 k how many
If o2 is bubbled through water at 393 k how many
If ${N_2}$ gas is bubbled through water at $293K$ , how many millimoles of ${N_2}$ gas would dissolve in $1Litre$ water Assuming that ${N_2}$ exerts a
The correct answer is p=KH×=×103 bar×mol of O2mol of =×no2 x 18no2 =×10−3m mol of O2=1
if i won the lottery i wouldn''t tell anyone pKHx 09204682103 barmolofO2molofH2O 09204682103molofO2100018 0920468218nO2 0920468218nO2 109103n02 mmolofO21millimole
ifte and os licence Without the specific Henry's law constant for 303 K and the partial pressure, we cannot provide the number of millimoles of O2 that would
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