# chemistry

The freezing point of a solution is

A. higher than the freezing point of the solvent alone because higher temperature is required to accelerate solvent molecular motion enough to overcome obstruction by solute particles.

B. lower than the freezing point of the solvent alone because lower temperature is required to accelerate solvent molecular motion enough to overcome obstruction by solute particles.

C. lower than the freezing point of the solvent alone because higher temperature is required to accelerate solvent molecular motion enough to overcome obstructon by solute particles..

D. lower than the freezing point of the solvent alone because lower temperature is required to slow solvent molecular motion enough to overcome obstruction by solute particles.

E. None of these are true.

I think the answer is D..is that right?

1. 👍 0
2. 👎 0
3. 👁 35
1. I would go with D also but it is a TERRIBLY confusing set of answers.

1. 👍 0
2. 👎 0
posted by DrBob222
2. i thought it was C, it makes more sense how does a lower temperature make solvent molecules move ffaster when obstructions are in the way? that's like saying i move faster in low temperatures when walls are in the way

1. 👍 0
2. 👎 0
3. d is the correct answer

1. 👍 0
2. 👎 0
posted by david

## Similar Questions

1. ### Chemistry

The equation for lowering the freezing point of a solvent is given in your manual. Given that the freezing point for the pure solvent is 79.4 °C , the molality is 0.1 m , and the freezing point depression constant is 6.9 °C/m ,

asked by Asia on September 13, 2015
2. ### chemistry

if the freezing point of the solution had been incorrectly determined to be lower than the true freezing point, how would that affect the calculated molar mass? Explain. The molecular weight would be higher if the true freezing

asked by Anonymous on February 1, 2009
3. ### chemistry

1. Find the molality of the solution prepared by dissolving 0.238g toluene, C7H8, in 15.8g cyclohexane 2. A pure sample of the solvent phenol has a freezing point of 40.85 degrees C. A 0.414 molal solution of isopropyl alcohol was

asked by kales on February 9, 2015
4. ### Chemistry

Benzene (C6H6) has a normal freezing point of 5.50oC and a density of 0.88 g/mL. When 1.28 g of naphthalene (C10H8) is dissolved in 125 mL of benzene, the freezing point of the solution is 5.03oC. Determine the molal freezing

asked by Sarah on February 8, 2017
5. ### chemistry

you are conducting a freezing-point determination in the laboratory by using an aqueous solution of KNO3. The observed freezing point of the solution is -1.15 C. Using a pure water sample, you recorded the freezing point of the

asked by Anonymous on February 17, 2011

sorry i forgot add the question The freezing point of a solution is A. lower than the freezing point of the solvent alone because higher temperature is required to accelerate solvent molecular motion enough to overcome obstructon

asked by phys on April 2, 2010
7. ### Chemistry

Two moles of a nonelectrolyte solute are dissolved in 1 kg of an unknown solvent. The solution freezes at 7.8 degrees Celsius below its normal freezing point. What is the molal freezing point constant of the unknown solvent? What

asked by Alyssa on May 17, 2010
8. ### Chemisty

A solution contains 20g of C^6H^12O^6 in 250g of water. What is the freezing-point depression of the solvent? What is the Freezing point of the solvent?

asked by Veronica on March 7, 2010
9. ### Chemistry

I am stuck in this problem I need to calculate the molality first so I could find T but I don't know which one is the solvent and which one is the solution the problem is to calculate the freezing point of a solution containing

asked by Maria on October 27, 2008
10. ### chemistry(check my work)

The freezing point of a solution is A. lower than the freezing point of the solvent alone because higher temperature is required to accelerate solvent molecular motion enough to overcome obstructon by solute particles.. B. higher

asked by eng on April 6, 2010

More Similar Questions