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Chemistry > Chapter 5 > Flashcards

Chapter 5 Flashcards

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1
Q

What is the equation to find Electrostatic Potential energy?

A

Eel= kQ1Q2/d

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2
Q

What is zero electrostatic potential energy?

A

as the potential energy at infinite speration of the charged particles.

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3
Q

When Q1 and Q2 have the same sign what happens to the particles?

A

they repel each other and a repulsive forces pushes them apart

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4
Q

How do you bring two postiviely charged objects closer?

A

you have to do work to overcome the repulsive force that exists between the two

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5
Q

What does the potential energy do as Electrostatic energy is postive?

A

deceares

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6
Q

What does distance do as potential energy decreases?

A

increase

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7
Q

What happens when Q1 and Q2 have opposite signs?

A

the particles attract each other and an attractive force pulls them toward each other

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8
Q

When is Electrostatic potential energy negative?

A

when the charges have opposite signs

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9
Q

What does the potential energy do as Electrostatic enrgy is negative

A

increases

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10
Q

What does distance do as potential energy increases?

A

decrease

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11
Q

How is energy released?

A

chemical bonds are formed

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12
Q

How is energy consumed?

A

chemical bonds are broken

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13
Q

What is the first law of thermodynamics?

A

energy can be converted from one from to another, but it is neither created nor destroyed

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14
Q

What is the equation to find internal energy?∆E

A

∆E= q+w

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15
Q

What is the system?

A

the portion of the unvierse that we single out for study

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16
Q

What is the surroundings?

A

everything that lies outside teh system that we study

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17
Q

What is an open system?

A

one in which matter and energy can be exchanged with the surroundings

Ex:an uncovered pot of boiling water on a stove

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18
Q

What is a closed system?

A

exchange energy but not matter with its surroundings

Ex:a mixture of hydrogen gas, and oxygen gas in a cylinder fitted with a piston

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19
Q

What is an isolated system?

A

neither energy nor matter can be exchanged with the surroundings

Ex: an insulated thermos containing hot coffee

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20
Q

What is internal energy?

A

the sum of all the kinetic and potnetial energies of the componetns of the system

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21
Q

What does a -∆E mean?

A

lost energy to its surroundings

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22
Q

What does a +∆E mean?

A

gained energy from its surroundings

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23
Q

What causes ther maginuted of internal energy(∆E) to change?

A

the adding and removing of heat or as work is done on or by the system

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24
Q

When heat is added to a system do the ∆E increase or decrease?

A

increases

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25
Q

When work is done on a system does ∆E increase or decrease?

A

increases

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26
Q

When does q or heat have a postive value?

A

when heat is transferred to the system from the surroundings

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27
Q

When does w(work) have a postive value?

A

when work is done on the system by the surroundings

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28
Q

When heat is lost by the system does ∆E increase or decrease?

A

decrease

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29
Q

When work is done by the system on the surroundings does ∆E increase or decrease?

A

decrease

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30
Q

When does w(work) have a negative value?

A

when work is done by the system on the surroundings

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31
Q

When does q(heat) have a negative value?

A

heat lost by the system to the surroiundings

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32
Q

When is a process endothermic?

A

system absorbs heat from its surroundings

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33
Q

When is a process exothermic?

A

system loses heat

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34
Q

What influences internal energy of a system?

A

temperature and pressure

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35
Q

What is a state function?

A

a property of a system that is determined by its state or condition and not by how it got to that state

36
Q

What are examples of state functions?

A

Tempature, pressure, composition

37
Q

What kind of a function is ∆E?

A

state function

38
Q

What kind of a function is q?

A

path function

39
Q

What kind of function is w?

A

path function

40
Q

What is ∆H?(change in enthalpy)

A

a reaction that occurs at constant pressure is the heat evolved or absorbed in the reaction

41
Q

How do you find enthalpy?(H)

A

E+PV

42
Q

What is pressure-volume work?

A

work perfomed by exapnsion of a gas against a resisting pressure

43
Q

What is the equation for volume-pressure work?

A

w=-P∆V

44
Q

When is pressure volume work positive?

A

when ∆V is negative, work done on the system by surroundings

45
Q

when is the pressure volume work negative?

A

∆V is positive, system does work on teh surroundings

46
Q

How many J is in 1L-atm?

A

101.3J

47
Q

What is the equation for ∆H(change in enthalpy)?

A

∆H= ∆E+P∆V

48
Q

What is ∆H= to?

A

q(heat of system at constant pressure)

49
Q

when ∆H(change in enthalpy) is positive what is q?

A

the system has gained heat from the surroundings so also postivie

50
Q

When ∆H( change in enthalpy) is negative what is q(heat)?

A

the system released heat to the surroundings(-)

51
Q

When ∆H is positive and q is postive is endothermic or exothermic?

A

endothermic

52
Q

When ∆H is negative and q is negative is it endothermic or exothermic?

A

exothermic

53
Q

Is ∆H a state or path function?

A

state function

54
Q

What is the ∆H for a chemical reaction?

A

∆H=Hproducts- Hreactants

55
Q

What is enthalpy of reaction?

A

the enthalpy change associated with a chemical reaction

56
Q

How is enthalpy of reaction written?

A

∆Hrxn

57
Q

Is enthalpy a extensive or intensive proerpty?

A

extensive property

58
Q

What is ∆H proportional to?

A

the amount of reactant consumed in the process

59
Q

What happens to the ∆H when you reverse the reaction?

A

the signs flip

60
Q

What does the ∆Hrxn depend on?

A

states of the reactants and products

61
Q

How to find heat(q) when given g of a reactant and the chemcial formula and the ∆H

A

Convert g to moles use the moles in chemical equation times the ∆H

62
Q

What is calorimetry?

A

the experimental measurement of heat produced in chemical and physical processes

63
Q

What is caloriemter?

A

an apparatus that measrues the heat released or absorbed in a chemical or physical process

64
Q

What is heat capacity?

A

the quantity of heat required to raise the temperature of a sample of matter

65
Q

What is molar heat capactiy?

A

the heat required to raise the temperature of one mole of a substance

66
Q

What is specifc heat?

A

the heat capacity of 1g of a substance the heat required to raise the temperature of 1g of a substance by 1 degree celsisus

67
Q

How can you find specifc heat(Cs)?

A

q(heat)/m x ∆T

68
Q

What is the units of Cs(specific heat)?

A

J/g-K

69
Q

How do you find q(heat)?

A

q=Cs(specific heat) x m x ∆ T

70
Q
A
71
Q

What is constant-pressure calorimetry?

A

monitoring the temp of the solution, we are seeing the flow of heat between teh system and the surroundings

72
Q

When does the tempature rise in constant pressure calorimetry?

A

heat is lost by the reaction and gained by the water in the solution(exothermic reaction)

73
Q

When is tempature decreased?

A

heat is gained by the reaction and lost by the water in teh solution

74
Q

What is the heat of the solution=?(qsoln)

A

-heat of reaction(-qrxn)

75
Q

When ∆T is positive what is qrxn?

A

negative

76
Q

What is a bomb calorimeter?

A

a device for measuring the heat evolved in the combustion of a substance under constant volume conditions

77
Q
A
78
Q

What is the qrxn for a bomb calorimeter?

A

qrxn=-Ccal x ∆T

79
Q

What is Hess’s law?

A

if a reaction is carried out in a seried of stpes, ∆H for the overall reaction equals the sum of the enthalpy changes for the steps

80
Q

What is enthalpy of formation?

A

the enthalpy change that accompanies the formation of a substance from the most stable forms of its component elements

81
Q

How do you find enthalpy of formation? (∆H˚f)

A

wanting to find the a compound of something by getting one mole of it

82
Q

How to find enthalpy formation of a reaction?(∆H˚rxn )

A

∑n∆H˚f(products)-∑m∆H˚f(reactants)

83
Q

What is the ∆H˚rxn for decomposition?

A

the reverse of the formation reaction

84
Q

What is bond enthalpy?

A

the enthalpy change, ∆H required to break a particular bond when the substance is in the gas phase

85
Q

How to find ∆Hrxn(for bonds)?

A

∑(bond enthalpies of bonds broken)-∑Bond enthalpies of bonds formed)

Chemistry (13 decks)

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