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Chemistry 2 > Exam 1 > Flashcards

Exam 1 Flashcards

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1
Q

What flows from

A

Hot to cold

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2
Q

Thermal equilibrium is reached

A

Over time reguardless of material ( any material will cool down or heat up to reach equilibrium

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3
Q

Energy

A

Capacity to do work

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4
Q

Work (w)

A

Force acting over a distance

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5
Q

Heat (q)

A

Flow of energy caused by a temperature difference

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6
Q

First law of thermodynamics

A

Energy can neither be created or destroyed

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7
Q

System

A

Whatever is actually undergoing change ( reaction) ex: chemicals doing a reaction

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8
Q

Surroundings

A

Everything around the reaction, beaker, water, air ect

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9
Q

Internal energy

A

Sum of all the kinetic energy and potential energy

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10
Q

State function

A

Property whose value is independent of pathway

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11
Q

If energy is gained

A

It’s positive internal energy (>E)

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12
Q

If the energy is released

A

It’s a negative > that’s a delta E

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13
Q

When the system gains thermal energy it’s is

A

Positive sign

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14
Q

When a system loses thermal energy it’s (q or heat)

A

Negative

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15
Q

Work(w) when work is done ON the system it’s

A

Positive

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16
Q

(W) when work is done BY the system it’s

A

Negative

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17
Q

Delta E( change in internal energy) energy flows INTO the system is

A

Positive

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18
Q

(E) energy flows out the system it’s

A

Negative

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19
Q

Work occurs when a______is caused by a _______ change against an external ________

A

1.Force
2.volume
3.pressure

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20
Q

Calorimetry

A

The process of measuring the amount of heat released or absorbed during a chemical reaction

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21
Q

Coffee cup calorimetry

A

Calculating the q (heat) based on changes in temperature at constant pressure

22
Q

Bomb calorimetry

A

calculating the delta E of a system at constant volume

23
Q

Heat capacity (c)

A

Systems ability to absorb thermal energy without undergoing a large change in system

24
Q

Specific heat (c or cs)

A

Amount of heat required to raise a temperature of 1g of a substance by 1 degree C

25
Q

Measuring a delta H of a reaction (enthalpy)

A

Measure of heat exchange at constant temperature

26
Q

Endothermic

A

Heat absorbed +🔼H

27
Q

Exothermic

A

Heat released (- 🔼H)

28
Q

Heat of reaction absorbed or released depends on the _______ of reactants

A

Amount

29
Q

Hess’s law (rule 1)

A

If equation is multiplied by a factor then 🔼Hrxn is multiplied by the same factor

30
Q

Hess law rule 2

A

If the chemical equation is reversed the sign changes

31
Q

Hess law 3

A

Add up the series of steps and the sum will be the 🔼 Hrxn for the overall equation

32
Q

Spontaneous process

A

One that occurs without intervention ( ex rust)

33
Q

Non spontaneous process

A

Not impossible but needs extra energy

34
Q

Entropy

A

The amount of chaos randomness or disorder in a sample

35
Q

Favorable +🔼S

A

More randomized sample

36
Q

Unfavorable

A

-🔼S less randomized sample

37
Q

For a exothermic process (enthalpy) a negative

A

No energy is required

38
Q

For entropy the more random and positive value is

A

Easier to process energetically

39
Q

Second law of thermodynamics: For any ________ process the entropy of the universe ________

A
  1. Spontaneous
  2. Increases
40
Q

When the temperature is high

A

Impact on entropy is small

41
Q

When temperature is low impact of entropy is

A

Significant

42
Q

At higher temperature water becomes

A

Non spontaneous

43
Q

Exothermic processes

A

Increase 🔼S surr

44
Q

Endothermic processes does what to surrounding

A

Decrease 🔼S surr

45
Q

If 🔼G is - the reaction is

A

Spontaneous

46
Q

If 🔼G is + the reaction is

A

Nonspontaneous

47
Q

Sign for Esys

A

Negative

48
Q

Sign for Esurr

A

Positive

49
Q

What role does a catalyst play in in thermodynamics

A

Catalyst don’t do anything in thermo it’s only in kinetics

50
Q

Can a reaction be endothermic and spontaneous

A

Yes because the entropy can take over

51
Q

Increase reactant concentration shifts it to the

A

Right and find more products

Chemistry 2 (3 decks)

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