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Chemistry I > Chapter 11 Test > Flashcards

Chapter 11 Test Flashcards

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1
Q

What is energy?

A

The capacity or ability for doing work

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2
Q

What do all physical and chemical changes involve?

A

the absorption or emission of energy (energy changes)

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3
Q

What is heat?

A

The energy transferred as a result as result of a temperature difference.

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4
Q

What is the symbol for heat?

A

q

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5
Q

How is heat energy transferred?

A

Heat (energy) is transferred from the system of higher energy/temp to the system with lower energy/temp.

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6
Q

What is a Joule?

A

unit of energy and heat

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7
Q

What is a calorie?

A

the amount of heat required to raise the temperature of 1 gram of pure water 1 oC.

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8
Q

What is the ratio of Joules to calories?

A

1 cal=4.184 J

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9
Q

What are symbols for calories and Joules?

A

J and cal

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10
Q

What is a Calorie?

A

1000 calories = 1kcal, used in our foods

the amount of energy the human body can obtain by chemically breaking down food.

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11
Q

What is the symbol for a Calorie?

A

C

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12
Q

What are exothermic reactions with respect to heat and energy?

A

Energy is given off by a reaction, usually in the form of heat. These reactions are usually spontaneous and the products have less energy than the reactants because energy is given off by the system.

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13
Q

What are endothermic reactions with respect to heat and energy?

A

Energy is absorbed in a reaction. The products of this reaction are of higher energy than the reactants.

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14
Q

What is a catalyst?

A

speeds up a chemical reaction by lowering the Activation energy.

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15
Q

What is an inhibitor?

A

slows down a chemical reaction by lowering the Activation energy.

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16
Q

What are the two sides of a chemical reaction equation?

A

Reactants —– Products

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17
Q

What is a Calorimeter?

A

instrument used to measure energy given off or absorbed during a physical or chemical change.

18
Q

What is the Law of Conservation of Energy?

A

All chemical and physical changes obey this. A law of science that states that energy cannot be created or destroyed, but only changed from one form into another or transferred from one object to another.

19
Q

What is specific heat?

A

The amount of heat energy needed to raise the temperature of 1 gram of substance, 1 oC.

20
Q

What is the symbol for specific heat?

A

Cp

21
Q

What kind of specific heat to metals have?

A

Low

22
Q

What is heat capacity?

A

the amount of heat/energy needed to raise the temperature of an object 1.0oC

23
Q

What is the Cp of ice?

A

2.11 J/g degrees C

24
Q

What is the Cp of liquid water?

A

4.184 J/g degrees C

25
Q

What is the Cp of water vapor?

A

2.08 J/g degrees C

26
Q

What is the specific heat equation?

A

Specific Heat (Cp) = Heat (J)/ Mass (g) x ΔT (oC)

27
Q

How to you rearrange the specific heat equation to solve for the heat needed?

A

q=(m)(Cp)(ΔT)

28
Q

What is enthalpy of fusion?

A

the energy required to melt a substance at its melting point

29
Q

What is enthalpy of solidification?

A

the energy released when a substance freezes at its freezing point

30
Q

What is enthalpy of vaporization?

A

the energy required to vaporize a substance at its boiling point

31
Q

What is enthalpy of condensation?

A

the energy released when a substance condenses

32
Q

What is the symbol for enthalpy of a change of matter state?

A

∆H

33
Q

What is boiling point?

A

the temperature at which the vapor pressure of the liquid is equal to the atmospheric pressure

34
Q

What is melting point?

A

the temperature at which the vapor pressure of the solid and liquid phases of a substance is equal

35
Q

What is freezing point?

A

the temperature when the vapor pressure of liquid equals the vapor pressure of the solid.

36
Q

In the water specific heat diagram, describe the change types they are based on heat and energy.

A

All of these changes are endothermic when they go up (melting, vaporization), but when they go opposite, it is exothermic (condensation, freezing)

37
Q

What is ∆Hfus for pure water?

A

334 J/g

38
Q

What is ∆Hvap for pure water?

A

2260 J/g

39
Q

What is ∆Hsolid for pure water?

A

-334 J/g

40
Q

What is ∆cont for pure water?

A

-2260 J/g

Chemistry I (15 decks)

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