1. Chemical Reactions H2H2 + O 2  H2OH2O reacts with to yield reactantsproduct 2 H atoms 2 O atoms 1 O atom conservation of mass 2 44 22 (g) (l) balanced chemical reaction (s) = solid (aq) = aqueous  = heat h = light

2. H2H2 + O 2  H2OH2O 22 (g) (l) atomic4 H atoms 2 O atoms 4 H atoms 2 O atoms molecular2 H 2 1 O 2 2 H 2 O molar 2 mol H 2 1 mol O 2 2 mol H 2 O mass g H 2 g O 2 g H 2 O 36.04 g reactants 36.04 g products coefficients stoichiometry described by balanced reaction 2.0162 x32.0018.022 x

3. Solid iron reacts with oxygen to form solid iron(III) oxide 1. Determine reactants and products Fe (s) O 2 (g) Fe O (s) 23 2. Write the unbalanced equation Fe (s) O 2 (g) Fe O 2 3 (s) + 3. Balance the atoms of one element Fe (s) O 2 (g) Fe O 2 3 (s) + 23 24 4(55.84 g) + 3(32.00 g) 2(159.68 g)

4. Magnesium reacts with hydrochloric acid to make hydrogen gas and magnesium chloride Mg (s) HCl (aq) H2H2 (g)MgCl 2 (aq) Mg (s) + HCl(aq)  H 2 (g) + MgCl 2 (aq) 2 1.1g Mg 0.045 mol 0.090 mol 0.180 mol 0.240 mol 0.360 mol 0.05 mol0.022 mol 0.045 mol 0.050 mol Limiting reagent HClH2H2 1. 2. 3.

5. H2H2 + O 2  H2OH2O 22 (g) (l)

6. Ammonia reacts with oxygen to produce nitrogen monoxide, a gas, and water 1.1. NH 3 (g)O 2 (g)NO (g)H 2 O (l) 2.2. NH 3 (g)O 2 (g)NO (g)H 2 O (l) ++ 3.3. NH 3 (g) O 2 (g) NO (g) H 2 O (l) + +232 5/2 4 546 If we start with 10.0 g of ammonia, how much water (l) can we produce?

7. If we start with 10.0 g of ammonia, how much water (l) can we produce? NH 3 (g) O 2 (g) NO (g) H 2 O (l) + +464 5 10.0 g NH 3 1 mol NH 3 17.03 g =0.587 mol NH 3 = g H 2 O 4 mol NH 3 6 mol H 2 O g H 2 O 1 mol H 2 O 18.02 15.9 If we start with 10.0 g of ammonia and 10.0 g O 2 how much water (l) can we produce?

8. If we start with 10.0 g of ammonia and 10.0 g O 2 how much water (l) can we produce? NH 3 (g) O 2 (g) NO (g) H 2 O (l) + +464 5 10.0 g NH 3 1 mol NH 3 17.0 g =0.587 mol NH 3 10.0 g O 2 1 mol O 2 32.0 g =0.313 mol O 2 0.587 mol NH 3 4 mol NH 3 5 mol O 2 = 0.734 mol O 2 limiting reagent 0.313 mol O 2 5 mol O 2 6 mol H 2 O 1 mol H 2 O 18.0 g = 6.76 g H 2 O theoretical yield

9. If we start with 10.0 g of ammonia and 10.0 g O 2 how much water (g) can we produce? NH 3 (g) O 2 (g) NO (g) H 2 O (l) + +464 5 10.0 g NH 3 1 mol NH 3 17.03 g =0.587 mol NH 3 10.0 g O 2 1 mol O 2 32.00 g =0.313 mol O 2 Which reagent will be left after the reaction is complete? How much of it will remain (g)? NH 3 0.313 mol O 2 5 mol O 2 4 mol NH 3 =.250 mol NH 3 consumed.587 mol-.250 mol =.337 mol NH 3 x 17.03 g/mol = 5.74 g NH 3 limiting reagent

10. Hydrofluoric acid is made by treating calcium fluoride with sulfuric acid. The other product is calcium sulfate. Ca F SO 4 2- H+H+ 2 F-F- H+H+ Ca 2+ CaF 2 (s) + H 2 SO 4 (l) 2 +- 2  HF (l) + CaSO 4 (s) 2 6.00 kg CaF 2 excess H 2 SO 4 2.86 kg HF limiting reagent 6.00 kg CaF 2 1000 g 1 kg 1 mol CaF 2 78.08 g CaF 2 1 mol CaF 2 2 mol HF 1 mol HF 20.008 g HF 1000 g 1 kg 3.07 kg HF % yield = theoretical 3.07 kg = 93.2 %= 2.86 kg actual