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106 Cards in this Set
- Front
- Back
1 kg = ? lbs |
2.2 lbs |
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1 in = ? cm |
2.54 cm |
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K = C + ? |
K = C + 273.15 |
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F = C? |
F = 1.8C + 32 |
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V of cylinder = ? |
V = pi(r^2)h |
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standard deviation = ? |
= SQRT((SUMd^2)/(n-1)) |
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10^6=(name and symbol) 10^3= 10^2= 10^1= |
Mega (M) kilo (k) hecto (h) deka (da) |
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10^-1= 10^-2= 10^-3= 10^-6= 10^-9= 10^-12= |
deci (d) centi (c) milli (m) micro (u) nano (n) pico (p) |
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1 L = ?qt |
1.057 qts |
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1 mL=?cm^3 |
1 cm^3 |
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1 gallon = ?qts |
= 4 qts |
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can K be (-)? K is proportional to... |
NO the average amount of kinetic energy |
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in the solid state, |
atoms and molecules pack closely in a fixed location |
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a homogenous mixture has... |
uniform composition and properties throughout |
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a heterogenous mixture has... |
different substances that remain physically seperate |
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a chemical change is... |
when a substance combines with another substance, either through synthesis or decomposition
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a physical change only... |
affects the form of a substance, not it's chemical composition. It often involves state changes (liquid, gas, or solid) |
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a physical property is... |
any measurable property whose value describes the state of a physical system (density) |
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kinetic energy is best defined as... |
the energy of motion |
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intensive and extensive properties??? |
need more info |
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exact numbers... |
can be considered to have an infinite number of significant figures |
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ionic: covalent: |
metal + nonmetal (cation + anion) nonmetal+nonmental (use prefixes) |
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Free element charge: 2 exceptions to charges: |
0 hydrogen in hydrides, where H = -1 (when H is bonded to a metal, it acts as a nonmetal) peroxides (e.g. H2O2), where O acts as -1 |
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3 transition metals that have definite oxidation states (don't need parentheses): Mercury is written as: |
Cd2+, Zn2+, Ag+ Hg2^2+ |
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acetate ammonium |
C2H3O2(-) NH4(+) |
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carbonate chromate |
CO3(2-) CrO4(2-) |
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hypochlorite chlorite chlorate perchlorate |
ClO(-) ClO2(-) ClO3(-) ClO4(-) |
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cyanide dichromate |
CN- Cr2O7(2-) |
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dihydrogen phosphate hydrogen carbonate |
H2PO4(-) HCO3(-) |
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hydrogen phosphate hydrogen sulfate |
HPO4(2-) HSO4(-) |
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hydroxide oxalate |
OH- C2O4(2-) |
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Nitrite Nitrate |
NO2(-) NO3(-) |
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permanganate peroxide |
MnO4(-) O2(2-) |
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phosphate sulfite sulfate |
PO4(3-) SO3(2-) SO4(2-) |
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Sb As Ba Be B Br |
Antimony Arsenic Barium Beryllium Boron Bromine |
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Ga Au Kr Ne Ni Pd |
Gallium Gold Krypton Neon Nickel Palladium |
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Pt Pu Ra Rn Rb |
Platinum Plutonium Radium Radon Rubidium |
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Sr W U Zr |
Strontium Tungsten Uranium Zirconium |
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Properties of solids: 4: |
fixed shape, fixed volume, can't be compressed or flow |
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Properties of liquids: 4: |
indefinite shape, fixed volume, can't be compressed, can flow |
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Properties of gas: 4: |
indefinite shape, indefinite volume, can be compressed, can flow |
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Close packing of matter leads to________, while loose packing leads to _________. |
definite volume and shape, indefinite volume and shape |
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2 kinds of solids and what makes them different: Examples: 2 of each |
crystalline - molecules are arranged in an orderly, geometric patter. Amorphous - pattern of molecules is not arranged at all. crystalline examples: salt and diamonds amorphous examples: plastic, glass, charcoal |
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Liquids are ________ packed, making them ________. |
tightly packed, making them incompressable. This allows liquids to take the shape of the container, but does not allow them to escape and expand to fill container like a gas. |
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In a gas state, particles are free from each other, there is a lot of __________ between particles. Because of this, particles can be _________ and gas can __________ to fill a container. |
empty space, compressed expand |
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a pure substance is ________ whose __________ does not change from one sample to another. It is made of a single type of ______ or _______. All samples have the same ________. |
matter whose composition does not change. atom or molecule. All samples have the same characteristics. |
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________ whose composition varies from one _____ to another is called a ____________. It has ________ combined in __________. Because the composition varies, ____________. |
Matter, sample, mixture. 2 or more types of atoms or molecules combined in VARIABLE PROPORTIONS. samples have different characteristics. |
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substances that cannot be broken down into simpler substances by chemical reactions are called__________ substances that can be decomposed are called_________. Most pure substances are _______________. |
elements - composed of single kind of atom although may be O2, etc. compounds. They are combinations of elements and molecules. All molecules of a compound are IDENTICAL so all samples of a compound behave in the same way. Compounds. |
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Difference between a mixture and a compound? |
A mixtures physical properties are not consistent because it has different molecules in varying degrees. A compound's properties are always the same because it consists of 2 or more atoms, but IDENTICAL molecules. Most pure substances are made of this. |
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A pure substance can be an _______ or a ____________, as long as it has only one kind of substance. |
element, compound |
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A _________ mixture describes one that has uniform composition throughout. Every piece of the sample has ________. A_________ mixture does not have uniform composition. It contains regions with _________ and the atoms and molecules_______ |
homogenous, the same characteristics herterogenous mixture, different characteristics, atoms and molecules are not mixed uniformly. |
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A good way to tell a homogenous mixture is one that is made of multiple substances but appears to be one substance. |
see other side |
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Pure substance vs.____________ Element vs. __________ homogenous mixture vs. _____________ |
mixture compound heterogenous mixture |
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Match the physical change to it's lab technique: boiling point - state of matter - adhereance to surface volatility density |
distallation filtration chromatogrpahy evaporation centrifugation and decanting |
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changes that alter the state or appearance of the matter without altering the composition are called_________ changes that alter the composition of the matter are called_________ |
physical changes chemical changes - atoms rearrange into new molecules, but all original atoms are still present |
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the characteristics of matter that can be changed without changing its composition____________. the characteristics that determine how the composition of matter changes as a result of contact with other matter or the influence of energy are ___________ |
physical properties (density, mass) chemical properties (polarity) |
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__________ force is the push or pull on objects that have an electrical charge. |
electrostatic force |
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_______ energy is due to the composition of matter and its position in the universe. |
potential - it arises from electrostatic forces between atoms, molecules and subatomic particles |
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materials that posses _______ potential energy are less ________. processes in nature tend to occur on their own when the result is material(s) with lower total potential energy |
high, less stable |
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1. Zero’s between numbers are significant. 30.09 has 4 SF 2. Zero’s that precede are NOT significant. 0.000034 has 2 SF 3. Zero’s at the end of decimals are significant. 0.00900 has 3 SF 4. Zero’s at the end without decimals are either. 4050 has either 4 SF or 3 SF |
see other side |
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________ is an indication of how close a measurement comes to the actual value of the quantity. It produces ___________. __________is an indication of how reproducible a measurement is. It produces ______. |
accuracy, systematic precision, random errors |
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______ believed matter was infinitely divisible while ________ believed that matter had a tiny, indivisible particle. |
Aristotle, Democritus |
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Law of conservation of mass: |
matter can neither be created nor destroyed - it all must add up in the end |
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Law of definite proportions |
a chemical compound always contains the exact same composition by mass |
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Law of Multiple Proportions |
when two elements combine with each other to form more than one compound, the weights of one element that combine with a fixed weight of the other are in a ratio of small whole numbers. For example, there are five distinct oxides of nitrogen, and the weights of oxygen in combination with 14 grams of nitrogen are, in increasing order, 8, 16, 24, 32, and 40 grams, or in a ratio of 1, 2, 3, 4, 5. |
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Dalton's Atomic Theory: Each element is composed of_______ All atoms of a given element have the same __________ and ______ that are unique to that element atoms combine in________ In a chemical reaction, atoms of one element cannot__________ |
tiny, indestructible particles called atoms mass and properties simple, whole number ratios to form molecules and compounds change into atoms of another element |
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the number of protons in the nucleus of an atom is called the _______ the percentage of an element that is 1 isotope is called the isotope’s _________ |
atomic number natural abundance. Note: the only thing different is the mass. All isotopes are CHEMICALLY identical |
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________ behave much differently than the neutral atom When the elements are arranged in order of increasing atomic mass, certain sets of properties recur periodically This is associated with __________ |
ions periodic law Mendeleev |
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Metals are _______ at room temp (except Hg), conduct _______ and ________. Are ______, ______, and ________. The ______ e- to form cations. |
solids heat and electricity shiny, malleable, ductile lose electrons |
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Nonmetals are found in ______. They are poor conductors of _____ and _______. Solids are _________. They ___ e- to become anions. |
all 3 states, heat and electricity brittle gain |
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_____ show some properties of metals and some of nonmetals. They are also known as ______ |
metalloids semiconductors |
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Despite its position on the periodic table, ____ is a nonmetal |
hydrogen |
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Columns of the periodic table are called ___ or ______ while rows are called ______. |
groups or families periods each period shows the pattern of properties repeated in the next period |
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Transition Elements vs. _______ or ______ B vs. ____ |
Main Group or Representative Elements A |
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Purples = alkalai metals Blue = alkali earth metals Yellow = transition metals Green = nonmetals Brown = metalloids Orange = non metal beige = halogens light blue = inert elements/ noble gases off-white = lanthanides then actinides |
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hydrogen forms _____ with nonmetals and ______ with metals |
compounds, hydrides (where it's charge is -1) |
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Alkali metals are ____ and have ____ boiling points and _______. The are very ________ and almost never found uncombined in nature. They react with water to form ____ aka _______ solutions. |
soft, low boiling points and density. reactive. basic aka alkaline |
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Alkali earth metals are ______, _____ melting and ______ than alkali metals. They are _______, but less so than alkali. form stable, insoluble oxides from which they are normally extracted |
harder, higher melting and denser. reactive. |
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All halogens are _________ and _______ |
nonmetals, diatomic |
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Noble gases are all gases at _______. The have low ___ and _____ points. They are very _____. |
room temperature. low melting and boiling points. unreactive. |
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The atomic mass is the sum of the _________ times _______. |
fractional abundance of the isotope times the mass of the isotope |
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masses and abundances of isotopes are measured with a ________ a _______ is a graph that gives the relative mass and relative abundance of each particle |
mass spectrometer mass spectrum |
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Avogadro’s Number = 6.0221421 x 1023 First list all atoms in order of metals, nonmetals, then “H” & “O” last. Leave the species that is split between more than one compound for last. |
see other side |
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Change Observation formation of a precipitate solid is formed formation of water heat is formed formation of a gas bubbles formed other changes are: Electrochemistry electrons are transferred Thermochemistry heat is transferred |
see other side |
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IONIC EQUATIONS have the substances which exist as ions written in ionic form. H+ (aq) + Cl- (aq) + Na+ (aq) + OH-(aq) → Na+ (aq) + Cl- (aq) + H2O (l) Precipitation, Acid/base, and Redox reactions can all be written depicting the appropriate substances as ions NET IONIC EQUATIONS are ionic equations with the Spectator ions removed. H+ (aq) + OH-(aq) → H2O (l) SPECTATOR IONS do not participate in a reaction (that is they do not react to form a new substance). Common Spectator ions are Group I, many Group II, and NO3- (nitrate) and C2H3O2- (acetate) ions. |
see other side |
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% X = (total atomic mass of X / molar mass which contains X) |
see other side |
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soluable vs _________ miscible vs ________, which means that the substances easily mix to form a uniform solution or that they separate into 2 distinct layers. a solution is a _________ mixture. |
insoluble miscible vs immiscible homogenous |
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The solute remains uniformly distributed throughout the solution and will not settle out through time. if the attractions between solute and solvent are strong enough, the solute will dissolve |
see other side |
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________ dissociate into ions when dissolved. ___________ do not dissociate when dissolved. |
ionic compounds. molecular compounds. |
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______ are species which conducts electricity when dissolved in water strong acid, bases and salts are ________ weak acid and bases are ________ |
electrolytes strong electrolytes weak electrolytes |
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ENDPOINT = POINT OF NEUTRALIZATION = EQUIVALENCE POINT At the end point for the titration of a strong acid with a strong base, the moles of acid (H+) equals the moles of base (OH-) to produce the neutral species water (H2O). If the mole ratio in the balanced chemical equation is NOT 1:1 then you must rely on the mole relationship and handle the problem like any other stoichiometry problem. |
see other side |
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titration technique: known solution in buret: |
volumetric analysis titrant |
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The concentration of the titrant must be known (called the standard solution).The exact reaction between the titrant and reacted substance must be known.The equivalence point must be known. An indicator that changes color at, or very near, the equivalence point is often used.The point at which the indicator changes color is called the end point. The goal is to choose an indicator whose end point coincides with the equivalence point. NOTE: Equivalence Point ≠ End Point! WHY???5. The volume of titrant required to reach the equivalence point must be known (measured) as accurately as possible. |
see other side |
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P = F/A 1 atm = 760 mmHg = 760 torr = 14.69 psi = 101.3 kPa Boyle’s Law P1V1 = P2V2 Charles’ Law V1 / T1 = V2 / T2 Guy-Lussac’s Law P1 / T1 = P2 / T2 Avogadro’s Law V1 / n1 = V2 / n2 Combined Gas Law P1V1 / T1 = P2 V2 / T2 |
Pressure = force per area unit |
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Dalton's Law of Partial Pressures: Ptotal = Pgas A + P gas B + Pgas C … PA = χAPTotal. dSTP = molar mass/molar volume d = (MM) P / R T |
see other side |
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root mean square speed = SQRT (3RT/MM) where R = 8.3145 J/K mol KE per mole = 3/2 RT |
see other side |
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Heavy molecules (such as CO2) travel with speeds close to their average values. The greater the molar mass, the lower the average speed and the narrower the spread of speeds. Light molecules (such as H2) not only have higher average speeds, but also a wider range of speeds. |
Maxwell distribution of speeds |
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Rate of effusion of gas A = √(molar mass B / molar mass A) Rate of effusion of gas B |
see other side |
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a ________ is the quantity of heat required to change the temperature of one gram of water by one degree Celsius |
calorie |
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1 cal = 4.184 J 1000 cal = 1kcal The third law of thermodynamics:The entropy of a perfect ________ at 0 K is _______.There is __________ at absolute 0 K. |
crystal, 0. no molecular movement |
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____________ gives off heat ____________ takes in heat |
exothermic endothermic |
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___________ is the same of all the kinetic/ potential energy in a system _______ is the variable for heat added to or liberated from the system. A positive variable, means that heat is being ______ while a negative means heat is being _______ to surroundings. This holds true for w too. |
internal q, added. transferred |
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─Work = External Pressure x Change in Volume State Function: In this case, it does not matter how crazy it was getting from A to B. It only matters what initial and final values were. It is important to know when it is a state function and when it is not. E.g. boiling water - doesn’t matter how water got from cold to hot, just the difference. State function means life it easier! Enthalpy is a state function |
see other side |
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Hess’s LawIf a reaction is carried out in a series of steps, ΔH for the reaction will be equal to the sum of the enthalpy changes for the individual steps. |
see other side |
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decomposition is endothermic because heat is needed to break bonds. synthesis is exothermic. |
see other side |
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formation of the elements trick still applies - if elements are present, be wary that the value is probably zero. |
see other side |