The volume of a gas mixed with water vapor at 32.0c at 742torr is 1350ml. what would be the volume of the gas at 0.0c and 760torr if all the water vapor were removed? the pressure of water vapor at 32c is 36torr.
show me how to do this?

1122.5 mL

Explanation:

In the first scenario, by Dalton's law, the total pressure is the sum of the partial pressures of the components. So, the partial pressure of the gas is:

P1 = Ptotal - Pwater = 742 - 36 = 706 torr

By the ideal gas law, the change in a state of a gas can be calculated by:

P1*V1/T1 = P2*V2/T2

Where P is the pressure, V is the volume, T is the temperature in K, 1 is the state 1, and 2 the state 2.

P1 = 706 torr, V1 = 1350 mL, T1 = 32ºC + 273 = 305K

P2 = 760 torr, T2 = 0ºC + 273 = 273 K

706*1350/305 = 760*V2/273

760V2/273 = 3124.92

760V2 = 853102.62

V2 = 1122.5 mL

the best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.

lol for the pointsss