Exam 5

Question 1

Kinetic energy

Answer 1

Energy of motion

Question 2

Potential energy

Answer 2

Stored energy

Question 3

SI unit of energy

Answer 3

Joule

Question 4

First law of thermodynamics

Answer 4

energy cannot be created or destroyed; it can only be converted from one form to another

Question 5

state function

Answer 5

the only part that matters is the start and the end, not the steps of how you got there

Question 6

energy is a ________ function

Answer 6

state

Question 7

what does + heat mean in a reaction

Answer 7

endothermic (heat in)

Question 8

what does (-) heat mean in a reaction

Answer 8

exothermic (heat out)

Question 9

Endothermic (sign?)

Answer 9

heat in (+)

Question 10

Exothermic (sign?)

Answer 10

heat out (-)

Question 11

what does C stand for

Answer 11

Heat capacity

Question 12

what does Cs stand for

Answer 12

Specific heat capacity

Question 13

q (heat) = (is pretty much the same as)

Answer 13

ΔH Enthalpy (at constant pressure)

Question 14

ΔHrxn = ΔHfinal - ΔHinitial

Question 15

Hess’s Law

Answer 15

enthalpies are additive

Question 16

Standard state conditions

Answer 16

P = 1 atm
T = 25°
Concentration = 1M

Question 17

1atm = ? mmHg
1atm = ? Torr

Answer 17

760 mmHg
760 Torr

Question 18

ΔH°f

Answer 18

Enthalpy of formation

Question 19

Enthalpy of formation

Answer 19

The energy required to form 1 mol of a substance from its elements in their standard state

Question 20

Calorimetry

Answer 20

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

Question 21

Pressure

Answer 21

the force exerted by molecules on or against another body

Question 22

SI unit for pressure

Answer 22

atm

Question 23

what are the 4 simple gas laws

Answer 23

Boyles law, Charles law, Avogadro’s law, Daltons law

Question 24

Boyles law
(proportionality?)

Answer 24

P and V are related
(at constant T)
(inversely proportional)
P₁V₁ = P₂V₂

Question 25

Charles law
(proportionality?)

Answer 25

V and T are related
(at constant P)
(directly proportional)
V₁ / T₁ = V₂ / T₂

Question 26

Avogadros law
(proportionality?)

Answer 26

V and n are related
(at constant T and P)
(directly proportional)
V₁ / n₁ = V₂ / n₂

Question 27

Daltons law

Answer 27

Pₜ = P₁ + P₂ + P₃

Question 28

what units of temperature are needed to use the gas laws

Answer 28

Kelvin

Question 29

Ideal gas law equation

Answer 29

PV = nRT
units = atm, L, mol, K

Question 30

what are the assumptions for the ideal gas law

Answer 30

1. Molecules have no volume
   (due to the molecules being so far apart)
2. Molecules do not interact with each other

Question 31

STP

Answer 31

Standard Temperature and Pressure
T = 0°C
P = 1 atm

Question 32

STP vs standard state conditions

Answer 32

STP is for gas law equations, standard state conditions are for thermodynamics equations

Question 33

Molar volume (volume occupied by 1 mole of any gas at STP)

Answer 33

22.4 L

Question 34

Kinetic molecular theory of gasses

Answer 34

the theory of moving molecules

theory states:
1. molecules have no volume
2. the average KE of a molecule is proportional to its T (in K)

Question 35

how does molecular speed, temperature and energy apply to KMT

Answer 35

if speed is high, KE is high
if T is high, KE is high

Question 36

Diffusion

Answer 36

random movement of molecules to spread out and fill space

Question 37

q (equation) =

Answer 37

c * m * ΔT

Question 38

ΔH (in relation to q)=

Answer 38

q/mol

Question 39

ΔH = ΔH(products) - ΔH(reactants)

Question 40

KE =

Answer 40

1/2 * m * v^2

Question 41

what makes a gas a real gas

Answer 41

high P
low T

Question 42

Assumptions for the ideal gas law

Answer 42

1. molecules have no volume
2. molecules do not interact with each other

Question 43

what is the unit of heat needed to raise 1 g of a substance 1° C

Answer 43

specific heat capacity