Entry Task: Block 1 Feb 1st- 2nd Block 2 Entry Task Question: WRITE THE QUESTION DOWN! How many moles are in 2.57 x1048 molecules of phosphorus dioxide?

Agenda: Sign off and discuss Mole Particle ws Mole notes #2 MolesGrams HW: MolesGrams ws

I can … Calculate the number of moles in a given mass Calculate the number of moles  particles. Calculate the molar mass of a compound.

Place starting amount here Moles Particles How many atoms are in 4.31 moles of carbon? Stoichiometry- set up! Place starting amount here Place the units you want to get rid of diagonal from each other 4.31 moles of C --------------- 6.02 x 1023 atoms = 25.946 x 1023 atoms C 1 mole of C ---------------- 3 Sig Figs and Sci notation!!! Place conversion here = 2.59 x 1024 atoms C

Place starting amount here Moles Particles How many moles are in a 5.55 x 1037 formula units of zinc II phosphate Stoichiometry- set up! Place starting amount here Place the units you want to get rid of diagonal from each other 1 mole of Zn3(PO4)2 5.55 x1037 fu Zn3(PO4)2 ------------- = 0.922 x1014 moles Subtract exponents 6.02 x 1023 fu Zn3(PO4)2 --------------- Place conversion here 3 Sig Figs and Sci notation!!! = 9.22 x1013 moles of Zn3(PO4)2

Place starting amount here Moles Particles How many moles are in a 9.25 x 1058 atoms of gold? Stoichiometry- set up! Place starting amount here Place the units you want to get rid of diagonal from each other 9.25 x1058 atom Au ------------- 1 mole of Au = 1.54 x1035 moles Au 6.02 x 1023 atoms --------- Subtract exponents Place conversion here

Place starting amount here Moles Particles How many atoms are in 989 moles of magnesium? Stoichiometry- set up! Place starting amount here Place the units you want to get rid of diagonal from each other 989 moles of Mg --------------- 6.02 x 1023 atoms = 5950 x 1023 atoms Mg 1 mole of Mg ---------------- 3 Sig Figs and Sci notation!!! Place conversion here = 5.95 x 1026 atoms Mg

Place starting amount here Moles Particles How many moles are in a 2.57 x 1048 molecules of phosphorus dioxide? Stoichiometry- set up! Place starting amount here Place the units you want to get rid of diagonal from each other 2.57 x1048 molecules PO2 ------------- 1 mole PO2 = 0.427 x1025 moles Subtract exponents 6.02 x 1023 molecules PO2 ------------ Place conversion here = 4.27 x1024 moles

Place starting amount here Moles Particles How many atoms are in 0.130 moles of iron III oxide? Stoichiometry- set up! Place starting amount here Place the units you want to get rid of diagonal from each other 0.130 moles of Fe2O3 --------------- 6.02 x 1023 atoms = 0.7826 x 1023 atoms Fe2O3 1 mole of Fe2O3 ---------------- 3 Sig Figs and Sci notation!!! Place conversion here = 7.83 x 1022 atoms Fe2O3

Place starting amount here Moles Particles How many formula units are in 2.85 moles of lithium chlorate? Stoichiometry- set up! Place starting amount here Place the units you want to get rid of diagonal from each other 2.85 moles of LiClO3 --------------- 6.02 x 1023 f.u = 17.157 x 1023 fu of LiClO3 1 mole of LiClO3 ---------------- 3 Sig Figs and Sci notation!!! Place conversion here = 1.72 x 1024 f.u. of LiClO3

Place starting amount here Moles Particles How many moles are in a 5.50 x 1046 atoms of copper? Stoichiometry- set up! Place starting amount here Place the units you want to get rid of diagonal from each other 1 mole of Cu 5.50 x1046 atoms Cu ------------- = 0.914 x1023 moles Subtract exponents 6.02 x 1023 atoms Cu --------- Place conversion here 3 Sig Figs and Sci notation!!! = 9.14 x1022 moles of Cu

Place starting amount here Moles Particles How many moles are in a 2.50 x 1031 molecules of water? Stoichiometry- set up! Place starting amount here Place the units you want to get rid of diagonal from each other 1 mole of water 2.50 x1031 molecules of water ------------- = 0.415 x108 moles Subtract exponents 6.02 x 1023 molecules of water --------- Place conversion here 3 Sig Figs and Sci notation!!! = 4.15 x107 moles of water

Place starting amount here Moles Particles How many formula units are in 0.364 moles of barium nitrate? Stoichiometry- set up! Place starting amount here Place the units you want to get rid of diagonal from each other 0.364 moles of Ba(NO3)2 --------------- 6.02 x 1023 f.u = 2.19 x 1023 fu of Ba(NO3)2 1 mole of Ba(NO3)2 ---------------- 3 Sig Figs and Sci notation!!! Place conversion here

Mole Notes #2

Moles to Mass Conversions A dozen feathers and a dozen eggs would not have the same mass. Neither would a mole of Hydrogen and a mole of zinc. To get masses, use the atomic mass from the periodic table The atomic mass represents the mass of 1 mole of that atom. This would also be known as its molar mass.

Moles to Mass Conversions Practice: Use your atomic mass on the periodic table as its molar mass. What is the atomic mass of carbon? 12.01 grams What is the mass of 1 mole of carbon? 12.01 grams What is the atomic mass of sodium? 22.9 grams What is the mass of 1 mole of sodium? 22.9 grams

Molar Mass What is the molar mass of Water- H2O Hydrogen = 1.0079 X 2 = 2.0158 grams Oxygen = 15.999 X 1 = 15.999 grams H2O molar mass = 18.015 grams for 1 mole

Molar Mass Lead II nitrate What is the molar mass of lead II nitrate? Pb +2 NO3 -1 NO3 -1 Pb(NO3)2 Pb= 207.2 g X 1 = 207.2 g N= 14.007 g X 2 = 28.014 g O= 15.999 g X 6 = 95.994 g 331.208 grams for 1 mole of Pb(NO3)2

So the molar mass of compound/molecule/atoms/ions is the same as its mass in 1 mole OR 6.02 x1023 compounds/molecules/atoms/ions.

Moles Grams How many grams would be in 2.0 moles of water? Stoichiometry- set up! Place starting amount here Place the units you want to get rid of diagonal from each other 2.0 moles of water --------------- 18 grams = 36 grams of water 1 mole of water --------------- = 3.6 x101 grams of water Place conversion 1mole = molar mass

Moles Grams How many grams would be in 0.65 moles of water? Stoichiometry- set up! Place starting amount here Place the units you want to get rid of diagonal from each other 0.65 moles of water --------------- 18 grams = 11.7 grams of water 1 mole of water --------------- = 1.2 x101 grams of water Place conversion 1mole = molar mass

GramsMoles How many moles would be in 0.65 grams of water? Stoichiometry- set up! Place starting amount here Place the units you want to get rid of diagonal from each other 0.65 grams of water --------------- 1 mole of water = 0.036 moles of water 18 grams --------------- = 3.6 x10-2 moles of water Place conversion 1mole = molar mass

GramsMoles How many moles would be in 75.0 grams of Lead II nitrate? Stoichiometry- set up! Place starting amount here Place the units you want to get rid of diagonal from each other 75.0 grams of Pb(NO3)2 --------------- 1 mole of Pb(NO3)2 = 0.226 moles of Pb(NO3)2 331.208 grams ----------- = 2.26 x10-1 moles of Pb(NO3)2 Place conversion 1mole = molar mass

Place starting amount here GramsMoles What if I have 0.680 moles of Ammonium phosphate, how many grams would that be? (NH4)3PO4 N= 14.007 g X 3 = 42.021 g H= 1.0079 g X 12 = 12.095 g Place starting amount here P= 30.974 g X 1 = 30.974 g O= 15.999 g X 4 = 63.996 g 1 mole = 149.086 grams 0.680 mole (NH4)3PO4 --------------- 149 grams of (NH4)3PO4 = 101 grams of (NH4)3PO4 1 mole (NH4)3PO4 -------------- 3 Sig Figs and Sci notation!!! Place conversion here = 1.01 X 102 grams of (NH4)3PO4

Place starting amount here GramsMoles What if I have 3.5 moles of Strontium chlorate, how many grams would that be? Sr(ClO3)2 Sr= 87.62 g X 1 = 87.62 g Place starting amount here Cl= 35.453 g X 2 = 70.906 g O= 15.999 g X 6 = 95.994 g 1 mole = 254.52 grams 3.5 mole Sr(ClO3)2 --------------- 255 grams of Sr(ClO3)2 = 891 grams of Sr(ClO3)2 1 mole Sr(ClO3)2 -------------- 2 Sig Figs and Sci notation!!! Place conversion here = 8.9 x102grams of Sr(ClO3)2