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2024 Tahsili Chemistry, Chemical Calculations
Moles
Avogadro's number |
6.02 x 1023 |
Molar Mass |
the mass of one mol of a substance |
Gas Laws
Boyle's Law (Constant Temp) |
P1V1 = P2V2 |
Graph Shape |
a decreasing curve |
Charle's Law (Constant Pressure) |
V1/T1 = V2/T2 |
Graph Shape |
an increasing line |
Gay-Lussac's Law (Constant Volume) |
P1/T1 = P2/T2 |
Graph Shape |
an increasing line |
General Law |
P1V1/T1 = P2V2/T2 |
Ideal Gas Law |
PV = nRT (R = 0.082) |
Standard Conditions (STP) |
temp = 273 K / 0 C and P = 1 atm |
Avogadro's Principle |
equal volumes of gases have equal number of particles at the same temp and pressure |
Chemical Potential Energy and Heat
Chemical Potential Energy |
the stored energy in the structure of matter |
Heat |
the energy transferred between objects (Joules) |
Calorie |
the amount of energy required to raise 1 gram of water by 1 degree C |
Heat Content (H) |
the amount of stored heat energy per mol under constant pressure |
Change in Heat Content / Enthalpy (ΔH) |
the energy absorbed or released in a reaction |
Enthalpy Formula |
ΔH = H (products) - H (reactants) |
H (products) < H (reactants) |
the reaction is exothermic, and will have a negative value |
H (products) > H (reactants) |
the reaction is endothermic, and will have a positive value |
Hess's law |
states that regardless of the multiple stages, the total enthalpy change is the sum of all the changes |
Standard heat of formation |
The change in heat content when 1 mol of compound is formed from its elements in standard conditions |
endothermic = positive = cold reactions |
exothermic = negative = warm reactions |
the heat of formation in standard conditions = 0 |
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Empirical and Molecular Formulas
Percent composition of A in AB |
( Mass of A / Mass of AB ) x 100% |
Empirical Formula |
The simplest whole number ratio of atoms (Ex: CH) |
Molecular Formula |
The actual number of atoms in a molecule (Ex: C6H6) |
N whole Number |
N = molecular formula mass / empirical formula mass |
Hydrated Salts |
salts with water molecules in it's crystals |
when hydrated salts are heated, they lose their water |
Calculations In Gases
Limiting Reactant |
the substance that is used up completely |
Excess Reactant |
the substance that is not used up and remains after the reaction |
Theoretical yield |
the largest amount of product that can be produced |
Actual Yield |
the amount produced by the experiment |
Percent Yield |
= (actual yield / theoretical yield) x 100 |
Kinetic Molecular Theory of Gases
a gas is comprised of molecules whose average distance between each other is greater than the size of its particles |
The particles of a gas exert no attractive forces on each other or the container |
The particles are in constant random motion |
The KE of a particle depends on its mass and velocity |
Gas Behavior
Diffusion |
the movement of particles from areas of high concentration to areas of low concentration |
Graham's Law of Diffusion |
Rate1 / Rate2 = √(molar mass 2 / molar mass 1) |
Flowing |
the movement of gases through small holes |
Pressure
Pressure |
the force applied perpendicularly to the surface of an object per unit area |
SI unit |
Pascal (N/m2) |
Barometer |
measures atmospheric pressure |
Manometer |
measures the pressure of a trapped gas |
Dalton's Law of partial pressure |
the total pressure of a mixture of gases is equal to the sum of the individual pressures |
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