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Vera_Pavlovna [14]
3 years ago
13

Which of the following is a correct statement about collision theory?

Chemistry
2 answers:
Evgen [1.6K]3 years ago
7 0

<u>Answer: </u>The correct answer is option D.

<u>Explanation:</u>

The number of collisions that take place per second per unit volume of the reaction is called as collision frequency.

Particles undergoing only effective collision will lead to chemical reactions.

For a collision to be effective, the colliding molecules must have energy more than a particular value known as threshold frequency.

The factors which are responsible for the number of effective collisions are:

  • Energy factor which means that the colliding molecules must have energy greater than the threshold energy.
  • Orientation factor which means that the colliding molecules must have proper orientations at the time of collisions.

Hence, the correct answer is option D.

rjkz [21]3 years ago
3 0
The answer is D. Effective collisions lead to chemical reactions!
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The colligative molality of an unknown aqueous solution is 1.56 m.
yawa3891 [41]

Answer:

Vapor pressure of solution = 17.02 Torr

T° of boiling point for the solution is 100.79°C

T° of freezing point for the solution is -2.9°C

Explanation:

Let's state the colligative properties with their formulas

- <u>Vapor pressure lowering</u>

ΔP = P° . Xm . i

- <u>Boiling point elevation</u>

ΔT = Kb . m . i

-<u> Freezing point depressión</u>

ΔT = Kf . m . i

ΔP = Vapor pressure pure solvent (P°) - Vapor pressure solution

ΔT = T° boling solution - T° boiling pure solvent

ΔT = T° freezing pure solvent - T° freezing solution

i represents the Van't Hoff factor (ions dissolved in the solution). If we assume that the solute is non-volatile and the solution is ideal i = 1

Kf and Kb are cryoscopic and ebulloscopic constant, they are  specific to each solvent.

Vapor pressure works with mole fraction (Xm) and the only data we have is molality, so we consider 1.56 moles of solute and 1000 g of solvent mass.

Moles of solvent → solvent mass / molar mass of solvent

Moles of solvent → 1000 g / 18 g/mol = 55.5 moles

Mole fraction is moles of solute / Total moles (mol st + mol sv)

Mole fraction: 1.56 / (1.56 + 55.5) = 0.027

- Vapor pressure lowering

ΔP = P° . Xm . i

17.5 Torr - Vapor pressure of solution = 17.5 Torr . 0.027 . 1

Vapor pressure of solution = - (17.5 Torr . 0.027 . 1 - 17.5 Torr)

Vapor pressure of solution = 17.02 Torr

- Boiling point elevation

ΔT = Kb . m . i

T° boiling solution - 100° = 0.512 °C/ m . 1.56 m . 1

T°boiling solution = 0.512 °C/ m . 1.56 m . 1 + 100°C

T°boiling solution = 100.79°C

- Freezing point depression

ΔT = Kf . m . i

0°C - T° freezing solution = 1.86 °C/m . 1.56 m . 1

T° freezing solution = - (1.86 °C/m . 1.56 m)

T° freezing solution = -2.9°C

3 0
3 years ago
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