Chapter 5 Flashcards
energy
capacity to do work/transfer heat
thermodynamics
study of energy and transformations (chemical, mechanical, electrical, etc.)
thermochemistry
relationships b/w chemical reactions and energy changes that involve heat
Potential energy- from position
electrostatic potential energy
interactions b/w charged particles
E(el) =
(kQ1Q2) / d
- Q1/Q2 = electrical charges (2 charge particles)
- d = distance
- k = 8.99 x 10^9 J (m/c^2)
- 1 J = 1 kg m^2/s^2
1st law of thermodynamics
energy can be converted from 1 form to another but it is neither created nor destroyed
making bonds
releases energy
breaking bonds
consumes energy
system
portion we single out to study
open system
exchange heat and mass w/ surroundings
closed system
only exchange heat (not mass) w/ surroundings
isolated system
doesn’t exchange heat or mass w/ surroundings
internal energy
sum of all kinetic and potential energy of system
∆E =
Change in E
∆E = E(final) – E(initial)
∆E = q + w
(+) = E(final) > E(initial)
System gained/absorbed energy from surrounding