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40 Cards in this Set
- Front
- Back
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What are the three states of mater?
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solid liquid gas
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Solid Particles are _____ and tightly packed together. particles. particles are ____ to each other solids maintain their ___ they have a ____ they are___ |
well ordered very attracted shape and volume high density non compressible |
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Liquids particles are still close together, but can ___ particles are ___ to each other liquids take the ___, but ___ they have a slightly ___ they are ___ |
flow past one another less attracted shape of their container, maintain their volume lower density slightly compressible |
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Gas particles are __, in a very chaotic arrangement particles are ___ to each other gases take ___ they have a ___. they are ___. |
far apart barley attracted shape and volume of their container very low density very compressible |
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kinetic molecular Gas particles are ___. they move in ___. they are very____. they collide with ___. they ___ as the temp ___. |
constantly in motion straight lines very far apart elastic collisions (no energy lost) speed up, increases ( kinetic energy increases.) |
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Gas laws Boyles law Pressure (P) and Volume(V) vary indirectly |
volume increases pressure decreases volume decreases pressure increases |
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Boyles law Inspiration Diaphragm lowers, chest wall expands, __ If volume gets __, pressure gets __ outside pressure is ___ than inside pressure air rushes __ lungs to equalize pressure. |
increasing volume of lungs larger, small greater into |
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Boyles law continued expiration (exhaling) Diaphragm raises, chest wall collapses, ___. If volume gets __, pressure gets larger __ inside pressure is ___ than outside pressure. air rushes___ lungs to equalize pressure. |
increasing volume of lungs small, larger greater out of |
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Charles Law Volume (V) and temp (T) vary directly |
temp increases volume increases temp decreases volume decreases |
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changes in state |
endothermic heat goes into the object > Melting evaporation or vaporization solid >>>> liquid >>>>> gas <<< <<< freezing condensation < exothermic heat comes out of the object |
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Boiling point transition temp between ___ and ___. Particles overcome ___ to escape as gas |
liquid, gas states water (I) > water (g) < I-----l---------l---------l---------l 20c 99c 100c 101c 120c transition temp both states are present |
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Melting point transition temp. between ___ and ___ particles must overcome attraction to each other and break up _____. |
solid, liquid the solids rigid structure water (S) > water (I) < l-------l--------l-----l---------l -20c -1c 0c 10c 15c |
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Decomposition |
occurs when atomic bonds break before state change occurs charring and burning occurs |
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Special properties of water Solid water is ___ than liquid water solid water has a ___ than liquid water water has a larger capacity for ___ water has a high ___ |
less dense larger volume absorbing heat surface tension (resistance of a liquids surface to disruption) |
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The mole avogadros number a mole (mol) is a ___ of a substance. avogadros number of items together make up 1 mole avogadros number is ___ when written with 4 significant figures. |
counted quantity 6.022x10^23 |
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For elements 1 mole C= ? For compounds 1 mole = ? allows conversion mole of an element <---> atoms of element moles of a compound <---> molecules of compound |
6.022x10^23 atoms of C 6.022x10^23 molecules |
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2.3x10^24 atoms of He makes up how many moles? |
initial value (old unit): 2.3x 10^24 atoms desired new unit: moles Conversion factor: 1 mole He= 6.022x10^23 atoms He 2.3x10^24atomes He X 1 mole He/6.022x10^23 atoms He = 3.8 mol He |
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How many molecules are in 3.00 moles of PH3?
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initial value(old): 3.00 moles of PH3 desired new unit: molecules conversion factor: 1 mole PH3= 6.022X10^23 molecules PH3 3.00 mole PH3 X 6.022X10^23/1 mol PH3= 1.81 X 10^24 |
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Molar mass of an element the molar mass of an element is the ___. what are the molar masses of H, C, and S? |
number of grams in 1 mol of any element 1 mole H= 6.022X10^23 molecules weights 1.01g 1 mole H= 1.01 g H (atomic/molar mass) 1 mole C= 12.01 g C 1 mole S= 32.06 g S |
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molar mass of a compound for a compound simply ___ the molar masses of ___ in the compound multiplied by ___. NH3? |
add, each element, its subscript N= 14.01 can also just multiply H 3xs H= 1.01 H= 1.01 h= 1.01 ------------ 17.04 g NH3= 1 mole NH3 |
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Calculations using molar mass what is the mass in grams of 4.00 moles of Pb? |
given value(old unit): desired new unit: mass (grams) conversion factor: 207.2 g Pb= 1 mol Pb 4.00 mol Pb X 207.2 g/ 1 mol Pb= 829 g Pb |
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how many moles are in 32.00 grams of H20?
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given value (old): 32.00 g H2O
desired new unit: moles conversion factor: 18.02 h H2O= 1 mol H2O add H mass and O mass togehter 32.00 g H2O * 1 mole H2O/ 32.00 g H2O= 1.776 mol H2O |
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what is the mass of 10.33 moles of NiC2? |
given value(old): 10.33 moles NiCl2desired new unit: mass(g)conversion factor: 1 mol NiCl2=129059 g NiCl2
10.33 mol NiCl2 * 129.59 g NiCl2/ 1 mol NiCl2= 1339 g NiCl2 |
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Chemical reactions yield Reactants ---> products H2(g) + O2(g) ---> H2O(l) law of conservation of matter: all equations must be balanced with coefficients which have the ______ possible. nothing will just disappear, balance equation multiply coefficients then add to see if they are equal. |
smallest whole number ratio |
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Balance __ H2(g) + __ O2(g) ----> __ H2O(l) |
2 H2 2H2O |
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Balance __ P4O10(s) + __ H2O(l) --> H4P2O7(aq) |
4 h2o 2 H4P2O7 |
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__ Al + __ H2SO4 --> __ Al2(SO4)3 + __ H2 |
2 Al 3 3 H2 |
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Moles and equations The coefficients of a balanced equation tells you the ___ ratio for each compound in the equation. 2 H2(g) + O2(g) --> 2 H20 they serve as a ___. this allows us to convert ___ in a balanced equation into __ in that same equation. |
mole-to-mole 2 mol 1 mol 2 mol free-form conversion factor moles of one substance moles of any other substance. |
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2 H2(g) + O2(g) --> 2 H20(l)
2 mol 1 mol 2 mol how many moles of H2O are formed when 2.00 moles of O2 react? |
2.00 mol O2 * 2 mol H2O/ 1 mol O2 = 4.00 mol H2O
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N2(g) + 3H2(g) --> 2 NH3(g) 1 mol 3 mol 2 mol how many moles of H2 reacted to form 0.22 mol NH3? |
0.22 mol NH3 * 3 mol H2/ 2 mol NH3= 0.33 mol H2 |
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For any reaction involving 2 species (A and B) we can convert: moles of a <--> moles of B l l v v grams of A grams of B |
no back |
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B A N2(g) + 3H2(g) --> 2 NH3(g) mole of A ---------------- moles of H2 l l grams NH3 7.04 g NH3 grams of H2 (2.02gH2)=1 |
2.4 g NH3 * 1 mol NH3/ 17.04 g NH3 * 3 mol H2/ 2 mol NH3 * 2.02 g H2/ 1 mol H2 = 0.43 g H2 |
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heat and reactions endothermic reactions energy (heat) must be ___ by the reactants. the energy will appear on the ___ of the chemical equation CO2 + H2O + heat --> C6H12O6(s) + O2 endothermic reactions feel ___ to the touch |
absorbed reactant side cold |
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ecothermic reactions energy (heat) must be ____ when products form. the energy will appear on the ____ of the chemical equation. CH4 + 2O2 --> CO2 + 2H2O + heat4 exothermic reactions feel ___ to the touch |
released product side warm |
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Rates of reactions Conditions required for a reaction to occur reactant molecules must __. the molecules must have the correct orientation to each other. they must have appropriate __ during the collision (activation energy) |
collide energy |
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Factors which affect the rate (speed) of a reaction. concentrations of reactants: a large # of molecules in a small area will collide more often temperature of reactants: a high temp makes molecule move faster, causing them to collide more often. adding a catalyst: the catalyst lowers the activation energy of a reaction allowing it to proceed faster. |
no back |
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reversible reaction and equilibrium reversible reaction aA + bB ----. cC dD reactants <--- products at equilibrium the rate of the forward reaction is equal to the rate of the ___. reactants are forming products __ as products are forming reactants. there is ___ in the amount of reactants or products present. |
reverse reaction exactly as fast no net change |
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Lechateliers principle states that the position of an equilibrium ___ in response to stress applied to that system. equilibrium shifts away from whats being added. equilibrium shifts toward whats being removed |
shifts |
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lechatieliers principle example H2 + I2 <---> 2 HI if I2 Removed: eq. will shift towards I2 (reactants) if H2 is added: eq will shift away from H2 (products) if HI is added: eq will shift away from HI (reactants) |
what the f is this shi |
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N2 + 3H2<---> 2NH3 + heat(exo) if heat is added: eq will shift away from heat (reactants) if heat is removed: eq will shift towards heat (products) |
no back |
