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ENGCHEM 111 LEC > ENERGy > Flashcards

ENERGy Flashcards

1
Q

Quadrillion

A

10^15

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2
Q

Btu

A

British thermal unit

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3
Q

1 Btu

A

1054.35 J

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4
Q

Energy supply can be broken down into

A

coal, natural gas, crude oil, NGL,
nuclear energy, and renewable energy

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5
Q

Energy consumption is broken down into four main components

A
  • Residential, 21%
  • Commercial, 19%
  • Industrial, 32%
  • Transportation, 29%
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6
Q

Two broad categories of energy

A

Potential energy and kinetic energy

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7
Q

Associated with the relative position of an object

A

Potential energy

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8
Q

Associated with motion

A

Kinetic energy

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9
Q

Formula for kinetic energy

A

1/2mv^2

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10
Q

The combined kinetic and potential energies of atoms and molecules that make up an object or system

A

Internal energy

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11
Q

Energy released or absorbed during a chemical reaction

A

Chemical energy

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12
Q

Study of the energetic consequences of chemistry

A

Thermochemistry

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13
Q

is the flow of energy between two objects because of a difference in temperature

A

Heat

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14
Q

is the transfer of energy accomplished by a force moving a mass some distance against resistance

A

Work

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15
Q

is the most common work type in chemistry

A

Pressure-volume work

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16
Q

SI unit of energy

A

Joule, J

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17
Q

W = mass x acceleration x distance

A
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18
Q

is the energy required to raise the temperature of 1 lb of water by 1°F

A

1 Btu

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19
Q

is the energy required to raise the temperature of 1 g of water from 14.5 to 15.5°C

A

1 calorie

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20
Q

1 Btu
1 calorie

A

1055 J
4.184 J

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21
Q

The part of the universe being considered

A

System

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22
Q

The remainder of the universe

A

Surroundings

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23
Q

System + Surroundings

A

Universe

24
Q

System and surroundings are separated by a

A

boundary

25
Q

For a system or surroundings, the only possible forms of energy flow are

A

heat q
work w

26
Q

means “change in” and is defined as the difference in the final and initial states

A

delta

27
Q

Formula for change in energy

A

q + w
E final - E initial

28
Q

values indicate that energy is being released

A

Negative values

29
Q

values indicate that energy is being absorbed

A

Positive values

30
Q

states that energy can be transformed from one form to another but cannot be created or destroyed

A

First law of thermodynamics

31
Q

A common way to obtain work from a system is to heat the system

A

Waste Energy

32
Q

Heat not converted to work is considered

A

waste energy

33
Q

is the temperature change in a body of water from hot or cold waste streams, resulting in temperatures different from normal seasonal ranges

A

Thermal pollution

34
Q

is a laboratory method for observing and measuring the flow of heat into and out of a system

A

Calorimetry

35
Q

is a physical property of a substance that describes the amount of heat required to raise the temperature of one gram of a substance by 1°C

A

specific heat capacity or specific heat

36
Q

is a physical property of a substance that describes the amount of heat required to raise the temperature of one mole of a substance by 1°C

A

molar heat capacity

37
Q

Formula specific heat

A

q = mc(delta)T

38
Q

Heat flow is measured using a

A

calorimeter

39
Q

measures the heat evolved or absorbed by the system of interest by measuring the temperature change in the surroundings

A

calorimeter

40
Q

two steps in a calorimetric measurement

A

calibration and actual measurement

41
Q

Heat released or absorbed in a reaction of known quantity of material is measured

A

Actual measurement

42
Q

The calorimeter constant, Ccalorimeter, is determined by dividing the known amount of heat released in the calorimeter by the temperature change of the calorimeter

A

Calibration

43
Q

Three metals aluminum (sh=0.900), copper (sh=0.385), and iron (sh=0.444) all start at room temperature, and they are placed in a furnace for 90 seconds. Which metal is at the highest temperature?
* Aluminum
* Copper
* Iron

A
  • Copper
44
Q

Why does sweating “cool” the body?
* Because water conducts heat better than skin
* Because evaporation absorbs heat
* Because water has a high heat capacity as it warms up on your skin

A
  • Because evaporation absorbs heat
45
Q

Burning 0.500 mol of carbon to form carbon dioxide releases 197 kJ of heat.
How much heat is released if 44.0 g of CO2
is produced in a similar reaction?
* 98.4 kJ
* 197 kJ
* 394 kJ
* 590 kJ

A
  • 394 kJ
46
Q

Conditions under which heat flow, q, occurs will have an impact on the measurement that is made

A

Enthalpy

47
Q

Combustion of octane releases ______________ under constant volume
conditions, represented as qv

A

5.45x 10^3 KJ

48
Q

Combustion of octane releases _______________ under constant pressure conditions, represented as qp

A

5.48x10^3 KJ

49
Q

is the heat flow under conditions of constant pressure

A

Enthalpy

50
Q

When a system releases heat, the process is said to be

A

exothermic (negative)

51
Q

When a system absorbs heat, the process is said to be

A

endothermic (positive)

52
Q

summarizes the overall energetics for a chemical reaction

A

thermochemical equation

53
Q

is the chemical reaction by which one mole of a compound is formed from its elements in their standard states

A

formation reaction

54
Q

is the most stable form of an element at room temperature, 25°C, and pressure, 1 atm

A

standard state

55
Q

Enthalpy change for any process is independent of the particular way the process is carried out

A

Hess’s law

56
Q

is a variable whose value depends only on the state of the system and not its history

A

state function

ENGCHEM 111 LEC (13 decks)

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