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ACHEM - Testing 2 > Chemistry Unit #4: Gases and Solutions...... Test on Thursday, January 12, 2017 > Flashcards

Chemistry Unit #4: Gases and Solutions...... Test on Thursday, January 12, 2017 Flashcards

1
Q

State the three assumptions used for the kinetic theory of matter.

A

I.) All matter are made of small particles

II.) All matter is moving

    III.) All particle collisions are elastic
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2
Q

A.) What is solute? 2

A

Smallest component in a solution

Particle separate from each other

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3
Q

Consider two closed glass containers of the same volume. One is filled with hydrogen gas and the other Is filled with carbon dioxide gas both at room temperature and pressure. How do the two gases compare in mass

A

CO2 higher

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4
Q

In C = n/V, what do the letters represent?

A

(C) CONCENTRATION = MOLE/VOLUME

(n) MOLE = number of moles of solute (what you are dissolving into the solvent).

(V) VOLUME = total volume of the solvent.

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5
Q

State two unique ways in which, according to the kinetic theory, it is possible to cause water to boil.

A

I.) Increase temperature to increase average kinetic energy of particles

II.) Decrease pressure until it matches the vapour pressure of the liquid

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6
Q

What is unsaturated? 2

A

A qualitative measure

More solute may dissolve for given temperature

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7
Q

What 101.3 kPa equal to in terms of atm?

A

1 atm

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8
Q

What is miscible? 2

A

Substance pair that can both completely dissolve in each other

Unlimited solubility

Example: alcohol and water

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9
Q

What is an ideal gas? Do they exist? Explain. 2

A

An Ideal Gas is a gas that exhibits no IMF (or does not condense into a liquid).

   Most gases at LOW PRESSURE and/or HIGH TEMPERATURE act as ideal gas until IMF become significant
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10
Q

B.)What is solvent? 2

A

Biggest component in a solution that surrounds the solute particles

Called Solvation (hydration in water)

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11
Q

Consider two closed glass containers of the same volume. One is filled with hydrogen gas and the other Is filled with carbon dioxide gas both at room temperature and pressure. How do the two gases compare in number of molecules

A

Same

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12
Q

What 101.3 kPa equal to in terms of torr?

A

760

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13
Q

What is supersaturated? 5

A

A qualitative measure

Excess solute has been dissolved for a given temperature

Extra dissolved at a higher temperature and carefully cooled

Very unstable Seeding or shaking results in precipitate forming
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14
Q

Using the kinetic theory of matter, explain why diffusion occurs when someone farts. 3

A

Flatulence contains gases (some are odourless, others not…) that have a velocity.

The particles will diffuse out of an area of higher concentration to an area or low concentration, away from the issuer. 

     They will be detected first by others near then those farther away until their concentration is below the threshold of most noses.
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15
Q

What is immiscible? 2

A

Substance pair that will separate into layers and not dissolve

Completely insoluble

Ex: oil and water

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16
Q

Consider two closed glass containers of the same volume. One is filled with hydrogen gas and the other Is filled with carbon dioxide gas both at room temperature and pressure. How do the two gases compare in velocity

A

H2 higher

17
Q

What is solution?

A

Solute and Solvent combined

18
Q

Convert the following temperatures into the other unit for temperature. (Kelvin to/vice versa Celsius) -

(25°C)

A

273 + 25 = 298 K

19
Q

Consider two closed glass containers of the same volume. One is filled with hydrogen gas and the other Is filled with carbon dioxide gas both at room temperature and pressure. If the temperature of the hydrogen gas container is now increased, how do the two gases now compare in mass

A

CO2 higher

20
Q

What 760 torr equal to in terms of kPa?

A

101.3 kPa

100 kPa for STP

21
Q

What is concentration?

A

Is a measure of how much solute is dissolved in a solvent. Maybe be qualitative, (Unsaturated, Saturated and Supersaturated.)

22
Q

Convert the following temperatures into the other unit for temperature. (Kelvin to/vice versa Celsius) -

(-67°C)

A

273 - 67 = 206 K

23
Q

What 760 torr equal to in terms of atmosphere (atm)?

A

1 atm

24
Q

Convert the following temperatures into the other unit for temperature. (Kelvin ÜÞ Celsius) —

(325 K)

A

273 - 325 = -52

25
Q

What is saturated? 4

A

A qualitative measure

No more solute may dissolve for given temperature

Excess undissolved solute rests on bottom of container

Lower the temperature, the lower the solubility

26
Q

Consider two closed glass containers of the same volume. One is filled with hydrogen gas and the other Is filled with carbon dioxide gas both at room temperature and pressure. If the temperature of the hydrogen gas container is now increased, how do the two gases now compare in average kinetic energy

A

H2 higher

27
Q

What is 1 atmosphere pressure equal to in terms of torr?

A

760 torr

28
Q

Convert the following temperatures into the other unit for temperature. (Kelvin to/vice versa Celsius) —

(100 K)

A

273 - 100 = 173°C

29
Q

Consider two closed glass containers of the same volume. One is filled with hydrogen gas and the other Is filled with carbon dioxide gas both at room temperature and pressure. How do the two gases compare in average kinetic energy

A

Same

30
Q

What is 1 atmosphere pressure equal to in terms of Pascal or kiloPascal (SI unit)?

A

101.3 kPa

100 kPa for STP

31
Q

Consider two closed glass containers of the same volume. One is filled with hydrogen gas and the other Is filled with carbon dioxide gas both at room temperature and pressure. If the temperature of the hydrogen gas container is now increased, how do the two gases now compare in number of molecules

A

Same

32
Q

Convert the following temperatures into the other unit for temperature. (Kelvin ÜÞ Celsius) —

(458°C)

A

273 + 458 = 731 K

33
Q

Convert the following temperatures into the other unit for temperature. (Kelvin ÜÞ Celsius) —

(273 K)

A

273 - 273 = 0

34
Q

Consider two closed glass containers of the same volume. One is filled with hydrogen gas and the other Is filled with carbon dioxide gas both at room temperature and pressure. If the temperature of the hydrogen gas container is now increased, how do the two gases now compare in pressure

A

H2 higher

ACHEM - Testing 2 (6 decks)

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