10th Grade Honors Chemistry Final Exam Flashcards
Thermochemistry ️The study of heat effects in chemical reactions.
Exothermic Reaction ️A reaction that releases energy in the form of heat.
Examples: Combustion, freezing water.
Heat generated is added to the product side (right side) be...
Heat generated is added to the reactant side (left side) because heat is added.
Enthalpy (H or ∆H) ✔️The energy after taking into account the pressure and volume of a substance.
If pressure remains constant, then heat absorbed or released during a chemical reaction is equal to the
enthalpy change for the reaction.
∆H = ✔️H Products - H Reactants.
Standard State of Element (Temperature and Pressure) ✔️Temperature = 25° Celsius.
Pressure = 1 atm.
ΔH° ✔️Standard enthalpy change = the heat transferred in a reaction with reactants and products in
standard states.
,Determining Enthalpy Change ✔️ΔH = (-) Exo.
ΔH = (+) Endo.
If heat is released as in an exothermic process the temperature will increase, but the product will have
less energy than the reactant so enthalpy will be negative.
If heat is absorbed as in an endothermic process the temperature will decrease, but the product will
have more energy than the reactant so enthalpy will be positive.
Sign of ΔH in a Reversed Equation ✔️Sign changes if equation is reversed.
Heat Capacity ✔️Amount of heat needed to raise the temperature of an object 1° Celsius.
Specific Heat ✔️Amount of heat needed to raise the temperature of 1 gram of a substance.
Heat ✔️Transfer of kinetic energy from a hotter object to a colder object.
Enthalpy Problems ✔️1. Convert given mass to moles.
2. Use ΔH (Given in problem)/# of mols from balanced equation.
Example: State whether the following reaction is endothermic or exothermic and whether the reactants
or the products contain more stored heat energy. Then find the quantity of head transferred when 6.29
grams of sulfur dioxide completely.
Elastic Collision ✔️Collision particles of an ideal gas undergo.
Ensures that energy is not lost.
In collisions between ideal gas molecules, the total energy of the gas... ✔️remains the same.
Volatile ✔️Evaporates easily.
Pressure ✔️Force per unit area.
760 mm Hg = 1 atm = 101,325 Pa = 101.325 kPa.
Boyle's Law ✔️Pressure of a gas is inversely proportional to its volume.
The temperature of a gas doesn't change.
P1V1 = P2V2.
Charle's Law ✔️At constant pressure, the volume of a fixed
amount of gas is directly proportional to its absolute temperature.
V=k2T
, V1T2=V2T1.
Avogadro's Law ✔️Equal volumes of gases at the same
temperature and pressure contain an equal number of particles.
V=k3n.
Manometer Measures ✔️Difference in pressure between the two columns of mercury.
Physical Properties of Gases/Kinetic Molecular Theory ✔️1. A gas consists of small particles that have
mass.
2. The particles in a gas must be separated from each other by relatively long distances.
3. The particles of a gas must be in a constant, rapid motion.
4. Collision of gas particles are perfectly elastic.
5. The average kinetic energy (energy of motion KE=mv^2/2) articles depend only on the temperature of
the gas. If you increase the temperature of a gas, you increase the movement of molecules which
increases the pressure.
6. Gas particles exert no force on each other.
Four things that change with relation to gas: ✔️- Amount of gas.
- Pressure.
- Temperature.
- Volume.
Amount of Gas ✔️You can relate the number of moles and the mass to the number of gas particles.
n = mass / molar mass.
Volume ✔️Liter = 1,000 cm^3.
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