Enthalpy

Thermodynamics

The study of change in energy/heat

State function

Difference between initial and final condition is independent from the path taken

Endothermic

Takes heat in, reactant

Exothermic

Heat oes out, product

Enthalpy is expression

Delta H

Paths to enthalpy

Calorimetry, Hess’ Law, Heat of formation

Calorimetry equation(s)

0 = q(rxn) + q(cal) + q(sol)

q = mC(delta T)

Hess law

Reactions used to make new reaction

Heat of formation

System

Area you are studying

Surroundings

Everything outisde the system

Universe

The system plus the surroundings

Open system

Exchange matter and energy

Closed system

Exchange energy but not matter

Isolated system

Can’t exchange energy or matter

Internal energy equation

Delta U = q + w

Work equation (non reversible)

w = -p(delta V)

Work equation reversible

w = nRTln(V2/V1)

negative q

-delta h, exothermic

positive q

positive delta H, endothermic

Solution cal

deltaH = q(p)

Bomb cal

delta E = q(v)

Calorimetry

heat absorbed/lost in reaction

Heat capactiy

ability to sustain heat raised to temp of 1 k or c

What is work

Work is motion through a distance against some opposing force.