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Chemistry 1210 > Chapter 5 > Flashcards

Chapter 5 Flashcards

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1
Q

Energy

A

Capacity to do work (w) or transfer heat (q)

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2
Q

Kinetic energy (Ek)

A

Energy due to particle motion and temperature of sample

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3
Q

Potential energy (Ep or Eel)

A

Energy due to particles’ position

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4
Q

Kinetic energy equation

A

KE = (1/2)mv^2

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5
Q

Potential energy equation

A

Eel = (kQ1Q2)/d

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6
Q

Thermodynamics

A

The study of energy and its transformations

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7
Q

Thermochemistry

A

The study of chemical reactions and the energy changes that involve heat

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8
Q

Heat (q)

A

Energy transfer that results from temperature difference

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9
Q

Work (w) (Physics)

A

A force applied across a distance

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10
Q

Work (w) (physics) equation

A

W = F • d

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11
Q

Work (w) (chemistry)

A

A force done by an expanding gas at a constant pressure

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12
Q

Work (w) (chemistry) equation

A

W = -P(delta V)

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13
Q

Change in volume equation

A

Delta V = Vf - Vi

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14
Q

Internal energy (E)

A

Kinetic + potential energy in a sample

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15
Q

Change in energy equation

A

Delta E = Ef - Ei
Delta E = q + w

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16
Q

Unit of energy

A

Joule (J)

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17
Q

System

A

Portion of the universe we study. To chemists, it is typically the chemical reaction.

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18
Q

Surroundings

A

The rest of the universe except the system under study

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19
Q

1st law of thermodynamics

A

Change in universe = 0, so -system = surroundings

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20
Q

Closed system

A

Energy, but not matter, can be transferred between system and surroundings

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21
Q

Open system

A

Energy and matter can be transferred between system and surroundings

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22
Q

Isolated system

A

Energy and matter cannot be transferred between system and surroundings

23
Q

Potential energy is lowest when…

A

The particles of matter are attracted and close together, where a negative PE is positive and the most stable

24
Q

When PE = 0

A

Particles are neither repelled nor attracted. There is no interaction.

25
Q

Breaking a chemical bond…

A

Always requires energy

26
Q

Forming a chemical bond always…

A

Releases energy

27
Q

If delta E is positive (Ef > Ei)…

A

Esys has gained energy from Esurr

28
Q

If delta E is negative (Ef < Ei)…

A

Esys has given energy to Esurr

29
Q

Endothermic reaction

A

System gains heat (q is positive)

30
Q

Exothermic reaction

A

System loses heat (q is negative)

31
Q

Work of the system is positive when…

A

Surroundings work on system (volume decreases)

32
Q

Work of system is negative when…

A

System works on surroundings (volume increases)

33
Q

q (subscript p)

A

The heat gained or lost under these conditions of constant pressure

34
Q

q (subscript p) in relation to enthalpy equation

A

Delta H = q (subscript p)

35
Q

Enthalpy is a _________ property

A

Extensive; if you double the amount of matter, the delta H is doubled

36
Q

Reversing a reaction…

A

Changes the sign (+ or -) of delta H

37
Q

The state (s, l, g) of reactants & products are _________

A

Important; will change overall change in enthalpy of a reaction

38
Q

Because delta H is a state function, the total enthalpy change for a chemical reaction depends only on…

A

The initial state of the reactants and the final state of the products

39
Q

Calorimetry

A

Experiment to measure heat transferred between system and surroundings (closed system)

40
Q

Heat capacity (C)

A

The amount of heat required to raise an object’s temperature by 1K

41
Q

Heat capacity equation

A

C = q/delta T
C = Cs • m

42
Q

Specific heat (Cs)

A

The amount of heat required to raise 1 gram of object’s temperature by 1K

43
Q

Specific heat equation

A

Cs = q/(m•delta T)

44
Q

A large value for specific heat means…

A

More heat required to raise temperature and temperature of substance is not easily changed

45
Q

3 equations for the signs of q

A

-q lost = q gained
-q sys = q surr
-q rxn = q solution

46
Q

If the thermometer records a temperature increase…

A

Heat went into the surroundings, heat left the system (reaction), process is exothermic, and q rxn = delta H rxn = negative

47
Q

If the thermometer records a temperature decrease…

A

Heat left the surroundings, heat went into the system, process is endothermic, and the q rxn = delta H rxn = positive

48
Q

Delta T equation

A

Delta T = Tf - Ti

49
Q

Change in enthalpy of a reaction equation

A

Delta H rxn = q rxn/moles

50
Q

Two types of calorimeters

A

Coffee cup: reactions at constant pressure and bomb: reactions involving gases

51
Q

Equation for calculating q for a bomb calorimetry

A

q rxn = -q cal = -C cal • delta T

52
Q

Standard enthalpy of formation (delta H°f)

A

Enthalpy change for formation of 1 mol of a substance from its elements in their most stable form with all reactants and products at 1 atm pressure and 298 K

53
Q

Bond enthalpy

A

The energy it takes to break a typical bond (+ energy)

Chemistry 1210 (6 decks)

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