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Chem 130 > Ch 9 > Flashcards

Ch 9 Flashcards

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1
Q

Energy

A

capacity to do work or produce hear

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2
Q

how is energy transfered

A

by work (force*displacement)

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3
Q

two main forms of energy

A

potential and kinetic

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4
Q

kinetic energy

A

energy due to motion

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5
Q

potential energy

A

energy due to position or composition

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6
Q

what is a system in a chemical equation

A

the molecules

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7
Q

first law of thermodynamics

A

total energy in universe is constanr

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8
Q

internal energy

A

sum of kinetic and potential energy in system

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9
Q

what is state function

A

property independent or pathway

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10
Q

state functions examples

A

temerature, pressure, concentrations, phase of matter, and internal energy

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11
Q

how do you find Change in energy of system

A

it is the negative change in surrounding energy

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12
Q

symbol for heat

A

q

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13
Q

symbol for work

A

w

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14
Q

how to find change in system energy

A

heat+ work

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15
Q

what does the sign of a mean

A

when positive it means system is endothermic, if it is negative it means system is exothermic

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16
Q

exothermic

A

energy released, hot to touch

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17
Q

endothermic

A

heat absorbed, cold to touch

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18
Q

what does sign of w mean

A

negative means work is done by system, when positive it means work is done to it

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19
Q

i what unit is measurement for thermal energy

A

temp

20
Q

how to find q equations

A

mass x heat capacity x change in temp

21
Q

specific heat capacity

A

amount of energy required to increase temp of 1g of substance

22
Q

expansion

A

work done by a gas +

23
Q

compression

A

work done to a gas -

24
Q

what does it mean if change in vol is 0

A

w is 0

25
Q

calorimetry

A

measure or heat transfer

26
Q

t or f using a calorimeter causes equations to change

A

false

27
Q

enthalpy

A

the amount of heat transferred under constant pressure

28
Q

enthalpy symbol

A

H

29
Q

equations for enthalpy

A

H = E+PV

30
Q

what is change in enthalpy equal to

A

heat of products

31
Q

Work equation

A

w = p x change in volune

32
Q

when manipulating a reaction with delta H what happens to delta H

A

same thing that happens to equation

33
Q

Hess’s law

A

if steps describe a reaction the sum of their delta h is equivalent

34
Q

how does a change in potential happen in chem reactions

A

when bonds are broken

35
Q

does breaking a bond require energy or does making one require it

A

breaking a bond requires energy

36
Q

how to find delta h for chem reaction

A

summing up bonds broken plus bonds created

37
Q

standard state for gas

A

pure substance 1 atm pressure

38
Q

standard state for liquid or solid

A

1 atm and 25 deg celcius

39
Q

standard state for aq

A

1 M concentration

40
Q

what does a bomb calorimeter ensure

A

reactions occur at constant volume

41
Q

what bonds are broken and formed in ending thermos reaction

A

weak are broken and strong form

42
Q

what bonds are broken and formed in exothermic reaction

A

strong broken and weak formed

43
Q

what is standard enthalpy of formation

A

energy for when a mop of compound forms from constituent elements in standard states

44
Q

how to calc change in enthalpy of reaction

A

sum of prod bonds - sum of react bonds
multiply all by their coefficients

45
Q

born havre cycle

A

a series of steps based on hess law that represent formation of ionic compounds and constituent elements

46
Q

how to find lattice energy

A

sum of energies after using born janet cycle

Chem 130 (20 decks)

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