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42 Cards in this Set

  • Front
  • Back

When energy is transferred from one object to another, it appears as _________ and/or ________.

Work, heat

__________ is the part of the universe we are focusing on, and the __________ are everything else.

The System, surroundings

∆E = ?

E (final) - E (initial)


also,


E (products) - E (reactants)




(∆E is the transfer of energy to/from system from/to surroundings)

E (final) < E (initial)






when...

A system releases energy to the surroundings




(∆E < 0)

E(final) > E (initial)




when...

A system absorbs energy from the surroundings




(∆E > 0)

Heat (thermal energy) symbolized by ____ , is the energy transferred as a result of difference in ____________ between system and surroundings.

q, temperature

________ (w) is the transfer of energy when an object is moved by __________.

Work, force.

∆E = ________ + ________

q, w


(heat + work)

When ∆E is _______ energy is transferred INTO the system.

When ∆E is _______ energy is transferred OUT from the system.

POSITIVE,


NEGATIVE

When a system transfers energy as heat (q), but does no work (w), ∆E = _______ + ________ .

q, 0







When heat (q) flows OUT, q is __________ .




When heat (q) flows IN, q is __________ .

Negative




Positive

Work (w) done BY a system, w is _________ .




Work (w) done ON a system, w is ________ .

Negative




Positive

________ law of thermodynamics (law of conservation of energy) states the total ___________ of the universe is __________.

First,




energy,




constant.

law of conservation of energy:


∆E (_____) = ∆E (_______) + ∆E (________) = 0

universe,




system,




surroundings.

Equation for Work (w):




w = ?

w = F x d

(force x distance)

Equation for Force:




F = ?

F = m x a




(mass x acceleration)


(m/s) and (m/s^2)

SI unit of energy is the _________ (J), measured in _______ / _______ .

Joule,




kg x m^2




s^2




(1 J = 1 kg⋅m^2 / s^2)

Calorie (cal) is the quantity of energy needed to raise the temp (T) of _______ of water by ______.

1 g




1°C




(specifically, from 14.5°C to 15.5°C)

1 cal = ________ J




1 J = _________ cal

4.184




1/4.184 or 0.2390

______ kJ = 1000 J = _______ kcal = 239.0 cal

1




0.2390

Btu = British thermal unit




________ Btu = 1055 J

1

State function is a _______ dependent ONLY on the _________________ of the system, NOT on the ________ the system takes to reach that state.

property,




current state,




path.

_________ energy (E) of a system is called a _______function.

Internal




state

The current state of a system is made up of its:


_______, _________, ________, and ________.

composition

volume

pressure

temperature


∆E _______ depend on how the change takes place, but only on the _______ between FINAL and INITIAL states.

does not,




difference.

Examples of state functions include...

Pressure (P)


Volume (V)


Temperature (T)


Internal Energy (E)

Enthalpy is a _______________ variable that relates directly to energy changes at _______________ pressure.

thermodynamic,




constant.

Two types of chemical work are:




__________________________ work and


__________________________ work.

electrical




pressure-volume (PV)

Electrical work is done by _________________.

moving charged particles.

PV work is the mechanical work done when ____________________________________________.

the volume of a system changes in the presence of an external pressure (P).

Pressure-volume work Equation

w = -P∆V

1 atm⋅L = ?

101.3 J

Enthalpy (H) is ______ at constant ______.

heat (q)




pressure.

Exothermic; heat as a __________.


_____________ heat and results in a _______________ in the enthalpy of the system.

Product,




Releases,




Decrease.

Endothermic; heat as a __________.


_____________ heat and results in an ______________ in the enthalpy of the system.

Reactant,




absorbs,




increase.

Formula for Enthalpy

H = E + PV

Heat capacity = ?

q / ∆T




[in units of J/K]

Specific heat capacity (c) = ?

q / ( mass x ∆T)




[in units of J/K]

To calculate heat absorbed or released:

q = c ⋅ mass ⋅ ∆T

Molar heat capacity (C) = ?

q / (amount (mol) ⋅ ∆T)




[in units of J/mol⋅K]

Calorimeter is a device used to measure _______ released (or absorbed) by a ______________ or ______________ process.

heat,




physical,




chemical.

Coffee-cup calorimeter measures heat at constant ___________.

Pressure