DATA
Empty Evaporating dish and watch glass: 33.6g
Evaporating dish, watch glass and NaHCO3: 35.08g
Evaporating dish, watch glass and product: 34.65
NaHCO3(s) + HCL (aq) ----> NaCl(s) + H2O(L) + CO2(g)
1. Determine the mass if the sodium bicarbonate reacted?
2. Calculate the theoretical yield of NaCl
3. Indentify the resude in the evaporation dish.
4. Determine the actual yield of NaCl
5. Calculate the percent yield of the experiment
6. Which is the limiting reactant? what evidence supports your answer?
No one here is going to do this for you. However, we will gladly critique your work or thinking.
1. To determine the mass of sodium bicarbonate (NaHCO3) that reacted, you need to find the difference in mass between the empty evaporating dish and watch glass and the mass of the evaporating dish, watch glass, and product.
Mass of NaHCO3 reacted = Mass of (Evaporating dish, watch glass, and product) - Mass of (Empty evaporating dish and watch glass)
= 34.65g - 33.6g
= 1.05g
Therefore, the mass of sodium bicarbonate that reacted is 1.05g.
2. The theoretical yield of NaCl can be calculated based on the balanced chemical equation and the stoichiometry. The balanced equation states that 1 mole of NaHCO3 reacts to produce 1 mole of NaCl.
To calculate the theoretical yield of NaCl, we need to convert the mass of sodium bicarbonate reacted (from question 1) to moles, and then use the stoichiometry to determine the moles of NaCl produced.
Molar mass of NaHCO3 = 22.99g/mol + 1.01g/mol + 12.01g/mol + 3(16.00g/mol)
= 84.01g/mol
Moles of NaHCO3 reacted = Mass of NaHCO3 reacted / Molar mass of NaHCO3
= 1.05g / 84.01g/mol
= 0.0125 mol
Since the stoichiometry of the reaction is 1:1, the moles of NaCl produced is also 0.0125 mol.
Theoretical yield of NaCl = Moles of NaCl produced * Molar mass of NaCl
= 0.0125 mol * (22.99g/mol + 35.45g/mol)
= 0.0125 mol * 58.44g/mol
= 0.73g
Therefore, the theoretical yield of NaCl is 0.73g.
3. To identify the residue in the evaporating dish, you need to subtract the mass of NaHCO3 reacted from the mass of the evaporating dish, watch glass, and NaHCO3.
Mass of residue = Mass of (Evaporating dish, watch glass, and NaHCO3) - Mass of NaHCO3 reacted
= 35.08g - 1.05g
= 34.03g
Therefore, the residue in the evaporating dish weighs 34.03g.
4. To determine the actual yield of NaCl, you need to find the difference in mass between the residue in the evaporating dish and the empty evaporating dish and watch glass.
Actual yield of NaCl = Mass of residue - Mass of (Empty evaporating dish and watch glass)
= 34.03g - 33.6g
= 0.43g
Therefore, the actual yield of NaCl is 0.43g.
5. The percent yield of the experiment can be calculated by dividing the actual yield (from question 4) by the theoretical yield (from question 2), and then multiplying by 100.
Percent yield = (Actual yield / Theoretical yield) * 100
= (0.43g / 0.73g) * 100
= 58.9%
Therefore, the percent yield of the experiment is approximately 58.9%.
6. To determine the limiting reactant, you must compare the moles of NaHCO3 and HCl in the reaction.
From the balanced chemical equation, the stoichiometric ratio between NaHCO3 and HCl is 1:1. Therefore, the limiting reactant will be the one with the smaller mole value.
To find the moles of HCl, we need to convert the mass of the product (NaCl) to moles, using the molar mass of NaCl.
Molar mass of NaCl = 22.99g/mol + 35.45g/mol
= 58.44g/mol
Moles of NaCl produced = Mass of NaCl / Molar mass of NaCl
= 0.43g / 58.44g/mol
= 0.0074 mol
Since the stoichiometry of the reaction is 1:1, the moles of HCl consumed is also 0.0074 mol.
Therefore, from the given information, we can conclude that the limiting reactant is HCl. The evidence to support this is that the moles of NaHCO3 (0.0125 mol from question 2) is greater than the moles of HCl (0.0074 mol).
Note: It is important to note that the limiting reactant should be determined based on the stoichiometry and not just the masses provided.