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Chemisrty > Thermochemisrty > Flashcards

Thermochemisrty Flashcards

0
Q

Specific heat capacity

A

Amount of heat needed to raise temp of 1 gram of a substance by 1 degree

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1
Q

Heat capacity

A

Amount of heat needed to raise the temp of an object by 1 degree

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2
Q

Specific heat capacity for water

A

4.186J/g degree Celsius

heats up slow

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3
Q

Specific heat capacity for lead

A

0.128J/g degree Celsius

Heats up fast

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4
Q

Heat absorbed by water

A

Q=mc

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5
Q

Heat of combustion

A

Energy released as heat when compound undergoes complete combustion with O under standard conditions

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6
Q

Endothermic

A

Reactant+reactant+ENERGY

=product+product

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7
Q

Exothermic

A

Reactant+reactant=product+product+ ENERGY

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8
Q

Isolated environment

A

Used to accurately determine how much thermal energy is produced in a combustion reaction

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9
Q

Open system

A

Can exchange both energy and matter with its strong surroundings

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10
Q

Closed system

A

No matter can enter or leave

Energy may be exchanged

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11
Q

Isolated system

A

No energy or matter can enter or leave

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12
Q

Bomb calorimeter

A

Isolated system

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13
Q

Molar enthalpy

A

Amount of energy released/ mole

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14
Q

Molar enthalpy equation

A
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15
Q

Chemical systems contain both _____ And _______ energy

A

Kinetic and potential

16
Q

Enthalpy change

A

Energy absorbed from or released to the surroundings when a system changes from reaction to products

17
Q

Enthalpy change equation

A

+or- lQsurroundingsl

18
Q

Molar enthalpy

A

Enthalpy change per mile of a substance undergoing a change

19
Q

Types of reactions

A 
Solution 
Combustion 
Vaporization 
Freezing 
Neutralization 
Formation
20
Q

Way to illustrate enthalpy change

A

Thermochemical equations

21
Q

Thermochemical equations with energy terms

A

Exothermic (-) value goes on PRODUCT side

Endothermic (+) value goes on REACTANT side

22
Q

Thermochemical equations with

A

Write balanced equation with

23
Q

Molar enthalpies of reaction

A

Write down energy associates with the reaction of one mile of a substance

24
Q

Enthalpy diagrams

A

LOOK AT NOTES

25
Q

Hess’ law

i)

A

Amount of energy change depends only on STATES of the reactants and state of products
NOT intermediate steps

26
Q

Hess’ law

ii)

A

Energy changes in chemical reactions are the SAME regardless whether the reactions occur in one or several steps

27
Q

Hess’ law

iii)

A

Total energy change in a chemical reaction is sum of energy changes in its many steps leading to overall reactions

28
Q

Hess’ law

A

Reactions may occur in any order or sequence

29
Q

A + B -> C + D

A

A -> 2D + E

30
Q

A -> B

A

B -> A

Chemisrty (1 decks)

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