L Octane (C3H₁8) has a vapor pressure of 14.3 torr and a density of 0.703 g/ mL. Benzene (C6H6) has a vapor pressure of 105.0 torr and a density of 0.876 g/mL. Calculate the vapor pressure (in torr) of a solution containing 655 mL of octane and 315 mL of benzene. Assume this solution behaves

The vapor pressure of benzene, C6H6 is 100.0 torr at 26.1 °C. How many moles of a nonvolatile solute must be added to 100.0 mL of benzene to decrease its vapor pressure by 10.0% at that temperature? The density of benzene is 0.8765 g/mL.

Pentane (C5H12) and hexane (C6H14) form an ideal solution. At 25°C the vapor pressures of pentane and hexane are 511 and 150 torr, respectively. A solution is prepared by mixing 25 mL pentane (density, 0.63 g/mL) with 43 mL hexane (density, 0.66 g/mL).   What is the vapor pressure of the resulting solution? Ptotal=         torr   What is the composition by the mole fraction of pentane in the vapor that is in equilibrium with this solution?

A solution is made using 16.7 percent by mass CH2Cl2 in CHCl3. At 30 °C, the vapor. pressure of pure CH2Cl2 is 490 mm Hg, and the vapor pressure of pure CHCl3 is 260 mm Hg. The normal boiling point of CHCl3 is 61.7 °C. What is the molality of CH2Cl2 in the solution?

A solution is prepared by adding 5.0 moles of LINO3 to 50.0 mole of water at 25 °C. Pure water has a vapor pressure of 24.0 torr at this temperature. What is the vapor pressure of the solution (torr)?

Ethanol (C₂H₂OH) has a vapor pressure of 93.0 torr and a density of 0.785 g/mL. Pentane (C₂H₁₂) has a vapor pressure of 435.0 torr and a density of 0.626 g/mL. Calculate the vapor pressure (in torr) of a solution containing 495 mL of ethanol and 165 mL of pentane. Assume this solution behaves ideally.

a sodium hydroxide solution that contains 41.5 grams of NaOH per L of solution has density of 1.08 g/mL. Calculate the molality of the NaOH in this solution

At a certain temperature the vapor pressure of water is 25.0 torr. A glucose solution is prepared by mixing 5.00 g of glucose and 2.00 moles of water. What is the expected vapor pressure of the solution? Molar mass of water = 18.02 g/mol and molar mass of glucose = 180.2 g/mol a) 0.342 torr b) 3.05 torr c) 22.0 torr d) 24.7 torr

Determine the vapor pressure of a solution at 35°C that contains 134.0 g of glucose (C6H1206) in 400.0 g of water. The vapor pressure of pure water at 35°C is 42.2 torr.

Order the following four aqueous solutions by their freezing point temperature. The concentrations are in molality. Assume complete dissociation of electrolytes. highest freezing point (highest temperature) 0.035 m sucrose, C6H12O6 1 2 3 0.010 m potassium bromide, KBr 4 0.010 m sodium carbonate, Na2CO3 0.015 m calcium chloride, CaCl2 lowest freezing point (lowest temperature)