a)
for O2:
[O2] = 1/H*P-O2 = 1/(43*10^3) * 0.2 = 0.000004651 M
for N2
[N2] = 1/H*P-N2 = 1/(85*10^3) * 0.75= 0.00000882352 M
for N2
[CO2] = 1/H*P-CO2 = 1/(1.61*10^3) * 0.05 = 0.00003105 M
b)
find vpaor pressure:
Ptotal =x1*P1 + x2*P2 + x3*P4
Vapor pressure of water = 23.756 torr then
Pvapor = 23.756 torr
Problem 3 [10 points] (a) Using the following table of Henry's law constants (kB(atm)-PB/XB) calculate the...
㎜ Review Constants Periodic Table Part A gas has a Henry's law constant of 0.183 M/atm How much water would be needed to completely dissolve 1.56 L of the gas at a pressure of 740 torr and a temperature ot 40 C Submit Request Answer
need #7-10 answered
6. The solubility of nitrogen gas at 25°C and a nitrogen pressure of 522 mmHg is 4.7 x 10 mol/L. What is the value of the Henry's Law constant in mol/L-atm? A) 6.8 × 10-4 mol/L-atm B) 4.7 x 10 mol/L-atm C) 3.2 × 104 moVL-atm D) 9.0 x 10 mol/L atm E) 1.5 x 10mol/L atm 7. According to Raoult's law, which statement is false? A) The vapor pressure of a solvent over a solution decreases...
(1). Which of the following molecules is most soluble in hexane, C6H14? NH3 CH3NH2 CH3OH CH3CH3 H2O (2). Which of the following molecules is most soluble in methanol CH3OH? N(CH3)3 CH3NH2 CH3COCH3 CH3CH2CH2CH2CH2CH3 HOCH2CH2OH (3). Calculate the concentration of CO2 in a soft drink that is bottled with a partial pressure of CO2 of 5 atm over the liquid at 25 °C. The Henry’s Law constant for CO2 in water at this temperature is 3.12 ´ 10–2 mol L–1 atm–1....