balanced chemical reaction

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Limiting Reactants and Percent Yield

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balanced chemical reaction Chemical Reactions reactants product 2 H2 + O2  2 H2O (g) (g) (l) to yield reacts with 2 H atoms 4 2 H atoms 4 2 O atoms 1 O atom 2 (s) = solid conservation of mass (aq) = aqueous  = heat balanced chemical reaction h = light

described by balanced reaction H2 + O2  H2O 2 (g) (l) coefficients atomic 4 H atoms 2 O atoms 4 H atoms 2 O atoms molecular 2 H2 1 O2 2 H2O molar 2 mol H2 1 mol O2 2 mol H2O 2 x 2.016 g H2 32.00 g O2 2 x g H2O 18.02 mass 36.04 g reactants 36.04 g products stoichiometry described by balanced reaction

Solid iron reacts with oxygen to form solid iron(III) oxide 1. Determine reactants and products Fe (s) O2 (g) Fe O (s) 2 3 2. Write the unbalanced equation Fe (s) + O2 (g) Fe O 2 3 (s) 3. Balance the atoms of one element 4 2 Fe (s) O2 (g) Fe O 2 3 (s) + 3 2 4 (55.84 g) + 3 (32.00 g) 2 (159.68 g)

Magnesium reacts with hydrochloric acid to make hydrogen gas and magnesium chloride 1. Mg (s) HCl (aq) H2 (g) Mg Cl (aq) 2 3. 2. Mg (s) + HCl(aq)  H2(g) + MgCl2 (aq) 2 Limiting reagent 1.1g Mg HCl H2 0.05 mol 0.045 mol 0.022 mol 0.090 mol 0.045 mol 0.180 mol 0.050 mol 0.240 mol 0.050 mol 0.360 mol 0.050 mol

2 H2 + O2  2 H2O (g) (g) (l)

Ammonia reacts with oxygen to produce nitrogen monoxide, a gas, and water 1. NH3 (g) O2 (g) NO (g) H2O (l) 2. NH3 (g) + O2 (g) NO (g) + H2O (l) 3. 2 NH3 (g) O2 (g) NO (g) H2O (l) + 2 3 5/2 4 5 4 6 If we start with 10.0 g of ammonia, how much water (l) can we produce?

If we start with 10.0 g of ammonia, how much water (l) can we produce? NH3 (g) O2 (g) NO (g) H2O (l) + 4 6 5 10.0 g NH3 1 mol NH3 = 0.587 mol NH3 17.03 g 0.587 mol NH3 6 mol H2O 18.02 g H2O = g H2O 15.9 4 mol NH3 1 mol H2O If we start with 10.0 g of ammonia and 10.0 g O2 how much water (l) can we produce?

If we start with 10.0 g of ammonia and 10.0 g O2 how much water (l) can we produce? NH3 (g) O2 (g) NO (g) H2O (l) + 4 6 5 10.0 g NH3 1 mol NH3 17.0 g = 0.587 mol NH3 10.0 g O2 1 mol O2 = 0.313 mol O2 limiting reagent 32.0 g 0.587 mol NH3 5 mol O2 = 0.734 mol O2 4 mol NH3 0.313 mol O2 6 mol H2O 18.0 g = 6.76 g H2O 5 mol O2 1 mol H2O theoretical yield

If we start with 10.0 g of ammonia and 10.0 g O2 how much water (g) can we produce? NH3 (g) O2 (g) NO (g) H2O (l) + 4 6 5 10.0 g NH3 1 mol NH3 17.03 g = 0.587 mol NH3 limiting reagent 10.0 g O2 1 mol O2 = 0.313 mol O2 32.00 g Which reagent will be left after the reaction is complete? How much of it will remain (g)? NH3 0.313 mol O2 4 mol NH3 = .250 mol NH3 consumed 5 mol O2 .587 mol - .250 mol = .337 mol NH3 x 17.03 g/mol = 5.74 g NH3

Hydrofluoric acid is made by treating calcium fluoride with sulfuric acid. The other product is calcium sulfate. Ca F 2 H+ SO42- H+ F- Ca2+ SO42- 2 + - 2 CaF2 (s) + H2SO4 (l)  HF (l) 2 + CaSO4 (s) 6.00 kg CaF2 excess H2SO4 2.86 kg HF limiting reagent 6.00 kg CaF2 1000 g 1 mol CaF2 2 mol HF 20.008 g HF 1 kg 1 kg 78.08 g CaF2 1 mol CaF2 1 mol HF 1000 g 3.07 kg HF % yield = actual = 2.86 kg = 93.2 % theoretical 3.07 kg