energy that is stored,
either in an object because of its position or in
a molecule because of its chemical composition
2 of 30
Define Heat
t the energy transferred from one object to
another as the result of a temperature difference
between them
3 of 30
Define temperature
a measure of the kinetic energy
of molecular motion
4 of 30
State the conservation of energy law
Energy cannot
be created or destroyed; it can only be converted
from one form into another
5 of 30
State the first law of thernodynamics
The total
internal energy of an isolated system is constant.
6 of 30
Define internal energy
the sum of kinetic and potential energies for each particle in a system
7 of 30
Define a state function
a function or property whose
value depends only on the present condition of
the system, not on the path used to arrive at that
condition
8 of 30
Define work
the distance (d) moved times the
force (F) that opposes the motion
9 of 30
Define enthalpy change
the heat change
in a reaction or process at constant pressure;
∆H = ∆E + P∆V
10 of 30
Define Heat of Reaction
the enthalpy change for
a reaction
11 of 30
Define Thermochemical equation
gives a balanced
chemical equation along with the value of the
enthalpy change, the amount of heat released or
absorbed when reactants are converted to products
12 of 30
Define exothermic
a reaction in which heat is evolved
and the temperature of the surroundings rises
13 of 30
Define endothermic
a reaction in which heat is
absorbed and the temperature of the surroundings falls
14 of 30
Define Heat Capacity
the amount of heat required
to raise the temperature of an object or substance
a given amount
15 of 30
Define molar heat capacity (Cm)
the amount of heat
necessary to raise the temperature of 1 mol of a
substance 1°C
16 of 30
State Hess' Law
The overall enthalpy change for
a reaction is equal to the sum of the enthalpy
changes for the individual steps in the reaction
17 of 30
Define standard heat of formation (∆H°f)
the
enthalpy change ∆H°f for the hypothetical
formation of 1 mol of a substance in its standard
state from the most stable forms of its constituent
elements in their standard states
18 of 30
Define a thermodynamic state
conditions
under which thermodynamic measurements are
reported; 298.15 K (25°C), 1 atm pressure for each
gas, 1 M concentration for solutions
19 of 30
Define Entropy
a measure of
the amount of molecular randomness in a system
20 of 30
Define Gibbs free-energy change (∆G)
(∆G)
∆G = ∆H - T∆S
21 of 30
Define a spontaneous process
one that proceeds on its
own without any continuous external influence
22 of 30
State the equation for Kinetic Energy
Ek=1/2mv^2
23 of 30
State the equation for work
Work (w2)= Force (F) x Distance (d) = -P∆V
24 of 30
State the equation for internal energy
∆E = q + w = q - P∆V
25 of 30
State the equation for enthalpy
∆H = qp = ∆E + P∆V where qp = heat at constant pressure, P = pressure
∆E = internal energy change, and ∆V = volume change
26 of 30
State the equation for Heat Capacity
C = q/∆T
27 of 30
State the equation for Heat Transfer
q = C x ∆T
q = Specific heat (c) x Mass of substance (m) x ∆T
q = Cm x Moles of substance x ∆T
28 of 30
State the equation for Heat of Reaction
For the reaction a A + b B + c ---> c C + d D + c....
∆H°reaction = [c ∆H°f(C) + d ∆H°f(D) +....]-[∆H°(1A) + b ∆H°f(B) +...]
29 of 30
State the equation for free energy change
∆G = ∆H - T∆S where ∆H = enthalpy change, T = temperature, ∆S = entropy change
30 of 30
Other cards in this set
Card 2
Front
Define Potential Energy
Back
energy that is stored,
either in an object because of its position or in
a molecule because of its chemical composition
Comments
No comments have yet been made