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ENERGY is the capacity to do work and transfer heat

Kinetic Energy is the energy of motion

Potential Energy is the stored energy that arises from the attractions and repulsions an object experiences in relation to other objects.

Internal Energy is the sum of all kinetic and potential energies.

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The unit for energy is joule (J)

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system: the portion we single out for study

surroundings: everything else

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Open System: matter and energy can be exchanged with the surroundings

Closed System: exchange of energy but no matter

Isolated System: neither energy or matter can be exchanged with the surroundings

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energy moves from a hotter object to a colder one

(q)

in joules or kilojoules

+ = the system gains heat

- = the system loses heat

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(w)

w = -P(change in V)

in Lxatm

+=work done on system

- = work done by system

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Work, Heat and the First Law of Thermodynamics | Thermodynamics (THRM101)

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involved: chemical equation, given mass/moles, and enthalpy

start with given amount and go from grams to moles to kj/mol to calculate heat produced per that amount.

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Heat / Enthalpy (∆H) Stoichiometry Practice Problems & Examples with Thermochemical Equations

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involved: heat capacity (c), a calorimeter, mass, and temp. change.

q = mc(change in temp)

change given values into correct units and plug into equation and solve for missing value

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Calorimetry Problems, Thermochemistry Practice, Specific Heat Capacity, Enthalpy Fusion, Chemistry

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involves: multiple equations with given enthalpy and one equation without given (goal equation)

change (flip) given equations to create the goal equation and add the enthalpy's together

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Hess's Law Problems & Enthalpy Change - Chemistry

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change in enthalpy = sum of enthalpys for products - sum of enthalpys for reactants

given a chemical equation

plug in enthalpy value from chart for each molecule multiplied by its coefficient into the formula.

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Enthalpies of Formation - Chemsitry Tutorial