"Limiting reactant" Essays and Research Papers

Limiting Reagents and Percentage Yield Worksheet 1.      Consider the reaction              I2O5(g) + 5 CO(g) ------->  5 CO2(g) + I2(g) a)   80.0 grams of iodine(V) oxide‚ I2O5‚ reacts with 28.0 grams of carbon monoxide‚ CO.       Determine the mass of iodine I2‚ which could be produced? 80 g I2O5 1 mol I2O5 1 mol I2 1 333.8 g I2O5 1 mol I2O5 28 g CO 1 mol CO 1 mol I2 253.8 g I2 1 28 g CO 5 mol CO 1 mol I2 b)   If‚ in the above situation‚ only 0.160 moles‚ of iodine‚ I2 was produced

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Determining the Limiting Reactant and Percent Yield in a Precipitation Reaction Objectives: Observe the reaction between solutions of sodium carbonate and calcium chloride. Determine which of the reactants is the limiting reactant and which is the excess reactant. Determine the theoretical mass of precipitate that should form. Compare the actual mass with the theoretical mass of precipitate and calculate the percent yield. Materials: Balance 0.70 M sodium carbonate solution‚ Na2CO3(aq)

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Experiment 8 Chemical Kinetics Abstract This experiment was done to determine the effects of the nature of the reactants‚ concentration‚ temperature‚ surface area and catalyst on the rate of chemical reactions. The nature of the reactants implies a difference if the reactants are aqueous or organic‚ acidic or basic or if they occur in the same phase or not. Acid-base reactions‚ formation of salts‚ and exchange of ions are fast reactions while reactions in which large molecules are formed

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and see if a precipitate or gas forms between any of these reactions. Research 1. Table A Reactants in Aqueous Solutions Predictions (1) MgCl₂(aq) + 2NaOH(aq) Mg(OH)₂(s) + 2NaCl(aq) (2) FeCl₃(aq) + 3NaOH(aq) Fe(OH)₃(s) + 3NaCl(aq) (3) 2KCl(aq) + Na₂SO₄(aq) K₂SO₄(s) + 2NaCl(aq) (4) CaCl₂(aq) + 2AgNO₃(aq) Ca(NO₃)₂(s) + Ag₂Cl(aq) (5) CuSO₄(aq) + Na₃PO₄(aq) Cu₃PO₄(aq) + Na₂SO₄(s) 2. Table B Reactants Predictions (1) Na₂CO₃(s) + 2HCl(aq) NaCl(aq) + CO₂(g) + H₂O(l) (2) NH₄Cl(s) + NaOH(aq) NaCl(aq)

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Experiment 2: The Effect of Different Reactants on the Type of Gases Produced Abdul Aziz Malik Submission Date: 18th April 2012 Background Information In the experiment‚ when oxygen is being tested‚ a glowing splint will be used and when that splint is placed in to the mystery gas and the splint reignites‚ then the gas is oxygen. When hydrogen is being tested‚ a burning splint will be used and when the splint is placed in to the mystery gas and a “pop” sound occurs‚ then the gas is hydrogen

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CALCULATIONS Determining the amount Limiting Reagent used. nlimiting reagent = Molarity x Volume or Mass / Molar Mass Example: Limiting reagent is 5mL of 1.0 M HCl nlimiting reagent = Molarity x Volume nlimiting reagent = (1.0 [mol/L]) x 0.005 [L]) = 0.005 mol Determining the qrxn and qcal. qrxn + qcal = 0 -qrxn = qcal qrxn = ΔHrxn x nlimiting reagent qcal = Ccal ΔT qrxn = - Ccal ΔT + mcsolid ΔT (note: only if there is a precipitate formed in the reaction)

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a final product of the double­replacement reaction; it breaks down (decomposes) immediately  into two products. (3 points)                                                   ___HCl___ + __NaHCO3___ → __H2O___ + __CO2___ +  __NACl___    The NaHCO3 is the limiting reactant and the HCl is the excess reactant in this experiment.  Determine the theoretical yield of the NaCl product‚ showing all of your work in the space below.  (5 points)    12.71 NaHCO3 / 84.01 g/mol = 0.1513 moles  0.1513 moles * 58.44 g/mol (NaCL molar mass) = 8

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much pure aspirin as possible. The reactants‚ acetyl anhydride and salicylic acid‚ must react in phosphoric acid. With phosphoric acid as a catalyst‚ the reaction yields aspirin and acetic acid. The equation for the reaction is as follows: “(CH3CO)2O + HOC6H4COOH □(→┴yields ) CH3CO2C6H4CO2H + CH3COOH” (French et al‚ 82). Aspirin and salicylic acid have similar properties‚ but many choose aspirin for medicine because it is not as acidic as salicylic acid. The limiting reagent limits how much product

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applicable 1. Product 2. Reactant / Reagent 3. Theoretical Yield 4. Actual Yield 5. Percent Yield 6. Excess Reagent 7. Limiting Reagent 8. Law of Conservation of Matter Short Answer – explain the following: 9. What is conserved in every balanced equation (multiple answers)? 10. What determines the mole ratio in a balanced equation? 11. What is the proper method to determine limiting reagents? 12. What is the relationship between the masses of products and reactants? Practice problems: 13. Using

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and Na3PO4. We determine the mole ratios by graphing the volume of reactant #1 vs. volume of precipitate for each reaction. Data Part 1.) Cylinder 1 2 3 4 5 6 7 Fe(NO3)3‚ 0.1 M‚ ml 5 10 12 15 17 20 24 NaOH‚ 0.1 M‚ ml 55 50 48 45 43 40 36 Fe:OH mole ratio 1:11 1:5 1:4 1:3 2:5 1:2 2:3 Volume Precipitate (ml) 6 10 12 16 22 8 11 Appearance Reactant Fe(NO3)3 Tinted orange/brown Reactant NaOH clear Product Parcipitate Fuzzy dark brown Part 2.) Cylinder

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