AP Chemistry Chapter 5 - Thermodynamics Flashcards

Ek = 1/2mv^2

ΔE = Efinal - Einitial

ΔE = q + w

<p>w = -P ΔV</p> Signup and view all the answers

<p>ΔH = q</p> Signup and view all the answers

<p>q = Cs x m x ΔT</p> Signup and view all the answers

<p>ΔH°rxn = ∑nΔH°f (products) - ∑mΔH°f (reactants)</p> Signup and view all the answers

<p>Eel = (K x Q1 x Q2)/d</p> Signup and view all the answers

<p>1 calorie = 4.184 J</p> Signup and view all the answers

<p>1 calorie/g·°C or 4.184 J/g·°C</p> Signup and view all the answers

<p>q = m x ΔHfus</p> Signup and view all the answers

<p>q = m x ΔHvap</p> Signup and view all the answers

<p>qsoln = Cs (of solution) x m (of solution) x ΔT = -qrxn</p> Signup and view all the answers

<p>qrxn = -Ccal x ΔT</p> Signup and view all the answers

Kinetic energy (Ek) is the energy of motion, calculated by the formula Ek = 1/2mv², where m is mass and v is velocity.

The change in internal energy (ΔE) represents the difference between the final and initial energy states of a system. It's calculated as ΔE = Efinal - Einitial.

The First Law of Thermodynamics states that the change in internal energy (ΔE) equals the sum of heat exchanged (q) and work done (w). This can be expressed as ΔE = q + w.

Pressure-volume work (w) is the work done by a system against a pressure as its volume changes. It's calculated as w = -P ΔV, where P is pressure and ΔV is the change in volume.

Enthalpy change (ΔH) at constant pressure represents the heat exchanged by the system. It's expressed as ΔH = q.

The heat gained or lost (q) in a calorimetric process can be calculated using the formula q = Cs x m x ΔT, where Cs is specific heat, m is mass, and ΔT is the temperature change.

The standard enthalpy change (ΔH°rxn) for a reaction can be calculated using Hess's Law, which states ΔH°rxn = ∑nΔH°f (products) - ∑mΔH°f (reactants).

Electrical potential energy (Eel) between two charges is calculated with the equation Eel = (K x Q1 x Q2)/d, where K is Coulomb's constant, Q1 and Q2 are the charges, and d is the distance between them.

The energy conversion factor between a calorie and a joule is 1 calorie = 4.184 J.

The specific heat of liquid water is 1 calorie/g·°C, which is equivalent to 4.184 J/g·°C.

The heat of fusion (q) is the amount of heat required to melt a solid into a liquid. It's calculated as q = m x ΔHfus, where m is mass and ΔHfus is the enthalpy of fusion.

The heat of vaporization (q) is the amount of heat needed to vaporize a liquid into a gas. It's expressed as q = m x ΔHvap, where ΔHvap is the enthalpy of vaporization.

The heat of solution (qsoln) is the heat change that occurs when a solute dissolves in a solvent. It's calculated using qsoln = Cs (of solution) x m (of solution) x ΔT = -qrxn.

The heat of reaction (qrxn) is determined by qrxn = -Ccal x ΔT, where Ccal is the calorimeter's heat capacity and ΔT is the temperature change.