Thermodynamics

Question 1

The law of thermodynamics apply to the ___

Answer 1

universe

Question 1

First law of thermodynamics

Answer 1

energy cannot be created or destroyed’ energy in a system remains constant but may be converted from one form to another

Question 2

The amount of energy contained within a system

Answer 2

enthalpy

Question 3

When heat transferred to the system

Answer 3

endothermic

Question 4

When heat is given off to the environment

Answer 4

exothermic

Question 5

In endothermic reaction, the products have ____ energy than the reactants

Answer 5

more

Question 6

In exothermic reactions the products have ___ energy than the reactants

Answer 6

less

Question 7

the transfer of heat via direct contact

Answer 7

conduction

Question 8

the transfer of heat due to motion of a liquid or gas

Answer 8

convection

Question 9

The transfer of heat via electromagnetic radiation

Answer 9

radiation

Question 10

Used to determine whether an expansion or compression is happening

Answer 10

work

Question 11

Under constant ____, heat and enthalpy within a system is a same (e.g in ___)

Answer 11

pressure, calorimetry

Question 12

The amount of energy that is required to raise the temperature of 1.0 g of a substance by 1°C

Answer 12

specific heat capacity

Question 13

The specific heat capacity for the same molecule depending on the ____, and is given by the formula ____. This means the the qsystem has to = ____. The heat required for a phase change, without changing the temperature is ____

Answer 13

phase, q = mc(delta T), -qsurroundings, q = m(delta H)

Question 14

At a phase change, the ___ stays the same even though the __ __ increases. This is because any additional heat input is used to change the ___ not raise the temperature

Answer 14

temperature, heat energy, phase

Question 15

A bomb calorimeter is used to measure the heat ___ by a sample ___ under a ___ atmosphere in a closed vessel surrounded by ___. The qreaction = ____, and qcal = ____

Answer 15

emitted, burned, oxygen, water, -qcal, c(delta T)

Question 16

There are 3 ways to calculate the standard enthalpy change: through the __ ___, the enthalpies of ___, and ___ law

Answer 16

bond energies, formation, Hess’s

Question 17

It takes energy to ___ a bond as atoms are in a __ __ state when they are not bonded

Answer 17

break, high energy

Question 18

(bond energies) delta H = ______

Answer 18

sum of all bonds broken (reactants) - sum of all bonds formed (products)

Question 19

the standard enthalpy of formation for an element in its standard state is always __

Answer 19

0

Question 20

Says that regardless of the multiple stages or steps of a reaction, the total enthalpy change for the reaction is the sum of all changes

Answer 20

Hess’s law

Question 21

The degree of disorder or randomness in a system

Answer 21

entropy

Question 22

__, ___ molecules have more entropy as they have more ways to move around in a 3D space

Answer 22

large, complicated

Question 23

Says that the entropy of the universe is always increasing

Answer 23

2nd law of thermodynamics

Question 24

The second law of thermodynamics is why heat flows from ___ to ___. The thermal energy becomes more __ __ among the particles which allows for an ___ in the entropy of the particles

Answer 24

hot, cold, spread out, increase

Question 25

says that the entropy of a pure crystalline substance at absolute zero temperature is zero

Answer 25

3rd law of thermodynamics

Question 26

of the 3 states of matter, ___ has the highest entropy. When ___ increases, the entropy increases. ___ temperature increases entropy. If the total number of product molecules is __ than the total number of reactant molecules, the entropy increases

Answer 26

gas, dissolution, higher, greater

Question 27

any process that occurs without the input of external energy

Answer 27

spontaneous reaction

Question 28

All spontaneous processes produce an __ in the entropy of the universe

Answer 28

increase

Question 29

In an exergonic reaction, energy is ___ to the surroundings and delta G is ___ 0. This means that the bonds formed are __ than the ones broken. The reaction is ___

Answer 29

released, <, stronger, spontaneous

Question 30

In endergonic reactions, the energy is __ from the surroundings and delta G ___ 0. This means the bonds formed are ___ than the bonds broken. The reaction is ____

Answer 30

absorbed, >, weaker, nonspontaneous

Question 31

When delta G is negative, Keq is ____ 1, and the __ are favored at equilibrium

Answer 31

> , products

Question 32

When delta G is positive, the K ___ 1, and the ___ are favoured at equilibrium

Answer 32

<, reactants

Question 33

When delta G is at 0, the K = ____ and the products and reactants are ___ ___ at equilibrium

Answer 33

1, equally favored