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chemistry > Energy > Flashcards

Energy Flashcards

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AP® Chemistry flashcards Periodic Table flashcards
1
Q

Energy at rest, energy that is stored between bonds in atoms. Potential or kinetic?

A

Potential Energy(PE)

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2
Q

Energy of motion, energy of molecules moving, faster molecules = higher temperature. Potential or kinetic?

A

Kinetic Energy(KE)

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3
Q

Potential or kinetic?
car is off, gas is sitting in tank

A

Potential Energy(PE)

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4
Q

Potential or kinetic?
car is on, gas is burning

A

Kinetic Energy(KE)

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5
Q

Stored in bonds of potential energy, released in chemical reactions such as heat(kinetic energy)
Chemical or thermal?

A

Chemical Energy

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6
Q

Comes from heat, responsible for temperature
Chemical or thermal?

A

Thermal Energy

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7
Q

Digestion, batteries, and photosynthesis are examples of chemical or thermal?

A

Chemical Energy

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8
Q

Boiling water, electricity passing through a metal, and sun radiation are examples of chemical or thermal?

A

Thermal Energy

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9
Q

The energy in the universe is divided into two parts:

A
  1. The system
  2. The surroundings
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10
Q

What is the law of conservation of energy?
(aka the 1st law of thermodynamics)

A

Energy cannot be created nor destroyed. It can only change forms

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11
Q

The average of the kinetic motion of molecules

A

Temperature

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12
Q

Temperature ↑ and kinetic energy ↑ makes molecules move?

A

Faster

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13
Q

Temperature ↓ and potential energy ↑ makes molecules move?

A

Slower

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14
Q

The energy(heat) content of a system

A

Enthalpy

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15
Q

What does ΔH represent?

A

Measure of enthalpy change

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16
Q

What does ΔH depend on?

A

The initial enthalpy of reactants AND final enthalpy of products

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17
Q

Equation to find enthalpy change

A

ΔH = H products- H reactants

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18
Q

Energy exits to the environment, feels hot, energy is a product
Exothermic or endothermic?

A

Exothermic reaction

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19
Q

Energy of reactants is greater than energy of products
Exothermic or endothermic?

A

Exothermic reaction

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20
Q

When bonds form, energy is released, making the molecule more stable
Exothermic or endothermic?

A

Exothermic reaction

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21
Q

A+B → C +heat
Exothermic or endothermic?

A

Exothermic reaction

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22
Q

Energy is absorbed from the environment, feels cold, energy is a reactant
Exothermic or endothermic?

A

Endothermic reaction

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23
Q

To break bonds, energy is required
Exothermic or endothermic?

A

Endothermic reaction

24
Q

Energy of the reactants is less than the energy of products
Exothermic or endothermic?

A

Endothermic reaction

25
Q

A+B+heat → C
Exothermic or endothermic?

A

Endothermic reaction

26
Q

System gives away heat, in the form of E made from stable bonds, exothermic reaction
Positive or negative ΔH(enthalpy)?

A

Negative ΔH

27
Q

System is gaining heat, in the form of E to break bonds, endothermic reaction
Positive or negativeΔH(enthalpy)?

A

Positive ΔH

28
Q

In a graph, products end lower than reactants
Exothermic or endothermic?

A

Exothermic reaction

29
Q

In a graph, products end higher than reactants
Exothermic or endothermic?

A

Endothermic reaction

30
Q

CaCO3 + heat → CaO + CO2
Exothermic or endothermic?

A

Endothermic reaction

31
Q

C3H8 + 5 O2 → 3 CO2 + 4 H2O + 2,200 KJ
Exothermic or endothermic?

A

Exothermic reaction

32
Q

3 H2 + N2 → 2 NH3 + Energy
Exothermic or endothermic?

A

Exothermic reaction

33
Q

The standard unit of energy in metric system (SI unit)

A

Joule (J)

34
Q

The American system of counting energy

A

Energy

35
Q

4.18 J = 1.0 cal

A

Formula for energy

36
Q

The amount of heat required to raise the temperature of 1 gram of a substance by 1℃. Units are J/goC

A

Specific heat

37
Q

True or false?
Substances will heat up faster if they have a lower specific heat.

A

TRUE
(ex. on the common heat capacity chart on formula chart, Bismuth heats up faster because it has a lower specific heat0

38
Q

Formula for calculating energy

A

Q = m ༝ c ༝ ΔT

39
Q

How much energy is absorbed by 34.4 g of water to heat it from 25.0oC to 78.8oC? The specific heat of water is 4.18 J/goC.

A

Q = 7,736.0096 J = 7,740 J

40
Q

If 4.50 g of water absorbs 276 J of energy, calculate temperature change of the water. The specific heat of water is 4.18 J/goC.

A

Q = 14.6730463oC = 14.7oC

41
Q

Law of conservation of energy

A

Energy cannot be created nor destroyed. It can only change forms. E released = E absorbed

42
Q

1 cal = ____ joules

A

4.18 J

43
Q

Equipment used to measure the amount of energy stored in a chemical reaction. It prevents heat from escaping or entering the system and enables accurate temperature measurements.

A

Calorimeter

44
Q

Is melting endothermic or exothermic?

A

Endothermic

45
Q

Is freezing endothermic or exothermic?

A

Exothermic

46
Q

Is condensing endothermic or exothermic?

A

Exothermic

47
Q

Is vaporization endothermic or exothermic?

A

Endothermic

48
Q

Is sublimation(going from solid to gas w/o going to liquid) endothermic or exothermic?

A

Endothermic

49
Q

Is deposition endothermic or exothermic?

A

Exothermic

50
Q

At what temperature does water freeze?

A

0°C or 32°F

51
Q

At what temperature does ice melt?

A

0°C or 32°F

52
Q

On a heating curve, where is kinetic energy changing?

A

Energy in motion

53
Q

On a heating curve, where is potential energy changing?

A

Energy absorbed

54
Q

Quantity of heat necessary to change 1 g of a solid to a liquid with no temperature change.
Heat of fusion or heat of vaporization?

A

Heat of fusion

55
Q

Quantity of heat necessary to change 1 g of a liquid into a vapor with no temperature change.
Heat of fusion or heat of vaporization?

A

Heat of vaporization

56
Q

Rewrite the following so it’s in order
1. The liquid boils
2. The temperature of solid increases
3. The temperature of the liquid increases
4. The solid melts
5. The temperature of gas increases

A

2, 4, 3, 1, 5

chemistry (5 decks)

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