Does adding 1 mol of nacl to 1 kg of water lower the vapor pressure of water to the same extent, a lesser extent, or a greater extent than adding 1 mol of c6h12o6 to 1 kg of water? and why?

Adding 1 mol of NaCl to 1 kg of water lower the vapor pressure of water to the same extent  by adding 1 mol of to 1 kg of water.

Explanation:

1) Moles of NaCl ,

Mass of water = m= 1 kg = 1000 g

Moles of water =

Vapor pressure of the solution =

Vapor pressure of the pure solvent that is water =

Mole fraction of solute(NaCl)=

The vapor pressure for the NaCl solution at 17.19 Torr.

2) Moles of sucrose ,

Mass of water = m  = 1 kg = 1000 g

Moles of water =

Vapor pressure of the solution =

Vapor pressure of the pure solvent that is water =

Mole fraction of solute ( glucose)=

The vapor pressure for the glucose solution at 17.19 Torr.

p = p' = 17.19 Torr

Adding 1 mol of NaCl to 1 kg of water lower the vapor pressure of water to the same extent  by adding 1 mol of to 1 kg of water.

the temperature of the gas, in k, not celsius.

the answer would be b i believe