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Chemistry 1 Honors > Unit 11 > Flashcards

Unit 11 Flashcards

1
Q

What’s specific heat?

A

The quantity of heat needed to change the temperature of 1 g of a substance by 1ma003-1.jpgC

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2
Q

Specific heat notation?

A

Joules/ grams x C*

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3
Q

What makes some things have lower/ higher specific heats?

A

Lower specific heats, like metals, are easier to heat up

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4
Q

What’s a joule?

A
  1. SI unit of energy
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5
Q

I Cal vs. 1 cal? (2)

A 
1 cal = 4.184 J
1 Cal (kilocalorie) = 1,000 cal
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6
Q

What happens if you increase hydrogen bonds?

A

Increasing # of hydrogen/polar bonds increases amount of energy required to break bonds

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7
Q

What does increasing hydrogen bonds affect?

A

Boiling, melting, etc

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8
Q

Water: 3 forms, which has the most volume?

A

Ice, bc specific bond length is wider, and expands

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9
Q

What’s enthalpy? (2)

A
  1. The heat content of a system @ constant pressure

2. How much heat does it have?

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10
Q

Enthalpy variable?

A

Q or H

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11
Q

Temp. Vs Heat

A

Temp: measure of average kinetic energy of particles
Heat: energy that flows from warmer ➡️ cooler objects

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12
Q

Endothermic vs. Exothermic reactions equations?

A

Endothermic: heat goes in, so ➕
Exothermic: heat goes out, so ➖

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13
Q

What’s the difference between potential and kinetic energy?

A

Kinetic: temp change (moving particles)
Potential: energy type in bond

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14
Q

Endothermic/ exothermic phase change diagram?

A

Endothermic: increases ↗️
Exothermic: decreases ↙️

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15
Q

Label
/
/ ______
———-
/. ___________
/. ___________
————/
/ ____________
/. ___________
/

A 
/
                                              / Gas
                            ----------
                          /.  Boiling point/ heat of vaporiz.
                         /.  Liquid 
   ------------/
  /  melting point/ heat of fusion 
 /.   Solid
/
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16
Q

What’s the heat of fusion? (2)

A
  1. Heat of fusion: change in enthalpy from heating a substance to change from solid ➡️ liquid.
  2. melting point
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17
Q

What’s the heat of vaporization? (2)

A
  1. Heat of vaporization: Change in enthalpy from heating so that liquid ➡️ gas
  2. boiling point
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18
Q

What’s the heat of condensation? (2)

A
  1. Heat of condensation: Change in enthalpy from heating so that gas ➡️ liquid
  2. Condensation point
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19
Q

What’s the heat of fission? (2)

A
  1. Heat of fission: Change in enthalpy from heating so that liquid ➡️ solid
  2. Freezing point
20
Q

Energy change w/ heat capacity formula?

A
  • Q = mc 🔼T
  • Q: heat added/ absorbed
  • m: mass
  • c: specific heat
  • 🔼T: change in temp. final- initial
21
Q

Energy changes with molar hfus + hvap formula?

A
  1. Melting/ fusion: q=m x 🔼Hf

2. Boiling/ vaporization: q=m x 🔼Hv

22
Q

Practice: If the temp of 34.4g of ethanol increases from 25C to 78.8C, how much heat has been absorbed by the ethanol?

A
  1. Q= MC🔼T

2. Q= 4553J

23
Q

Nutritional value calories (for food) are measured with…

A

Big C calories, so kilocalories

24
Q

The ___ law of thermodynamics states that energy is neither created nor destroyed.

25
The amount of energy required to raise the temperature of one gram of pure water by one degree Celsius is defined as
Calorie
26
Which of the following is NOT a form of energy? a. light b. pressure c. heat d. electricity
B. PRESSURE
27
When energy is changed from one form to another, ____. a. some of the energy is lost entirely b. all of the energy can be accounted for c. a physical change occurs d. all of the energy is changed to a useful form
B. All of the energy is accounted for.
28
What's transferred due to a energy difference?
Heat
29
The quantity of heat required to change the temperature of 1 g of a substance by 1*gC is defined as ____. a. a joule b. specific heat c. a calorie d. density
B. Specific heat
30
The heat capacity of an object depends in part on its ____. a. mass b. enthalpy c. shape d. potential energy
A. Mass
31
A piece of candy has 5 Calories (or 5000 calories). If it could be burned, leaving nothing but carbon dioxide and water, how much heat would it give off?
5 kilocalories
32
What would likely happen if you were to touch the flask in which an endothermic reaction were occurring? a. The flask would probably feel cooler than before the reaction started. b. The flask would probably feel warmer than before the reaction started. c. The flask would feel the same as before the reaction started. d. none of the above
A.
33
Which of the following substances has the highest specific heat? a. steel b. water c. alcohol d. chloroform
Water
34
A process that absorbs heat is a(n) ____.
endothermic process
35
During a phase change, the temperature of a substance ____. a. increases b. decreases c. remains constant d. may increase or decrease
C. Remains constant (think of a graph)
36
When 10 g of diethyl ether is converted to vapor at its boiling point, about how much heat is absorbed?
2 kJ
37
If the heat of fusion of water is 15 cal/ gram, the amount of energy required to change 80.0 grams of ice at 0º C to 80.0 grams of water at 0ºC is –
1200 cal
38
How much heat is required to vaporize 343 g of liquid ethanol at its boiling point? delta Hvap = 38.6 kJ/mol
287 kJ mol
39
As heat is added to a substance undergoing a phase change, the temperature remains constant because the energy is being used to — a. lower the specific heat capacity b. overcome intermolecular forces c. oppose electron cloud repulsions d. break covalent bonds
B.
40
Heat capacity
Quantity of heat needed to change the temperature of an object by 1*C
41
Rusting is not a spontaneous process.
False, rusting IS spontaneous
42
Energy
The ability to do work and produce heat
43
Calculate delta G, given delta H is -11kJ/mol, delta S is 195 J/ mol K, and temperature is 25*c. Give answer in kJ/mol.
-69.11 kJ/mol
44
On what principle does calorimetry depend? a. Hess's law b. law of conservation of energy c. law of enthalpy d. law of multiple proportions
B. Conservation of Energy is the best answer. Calorimetry depends on the fact that heat given off by a reaction equals the heat taken up by the surroundings, usually water in a calorimeter. Thus the energy is conserved.
45
Calculate the amount of heat in kJ evolved when 10. g of water is boiled. The !HVap is 2260 J/mol. (Answer in #.# format no units needed.)
Convert grams to moles, solve for q, convert J to kJ.
46
What's Hess's law?
The total enthalpy change for the reaction is the sum of all changes, and depends only on the initial and final results, not the ones in the middle.
47
What do Hess's law prove?
That enthalpy is a state function

Chemistry 1 Honors (15 decks)

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