Respuesta :
Taking into account the reaction stoichiometry, the percent yield of BaCO₃ is 81.07%.
Reaction stoichiometry
In first place, the balanced reaction is:
BaCl₂ + Na₂CO₃ → BaCO₃ + 2 NaCl
By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:
- BaCl₂: 1 mole
- Na₂CO₃: 1 mole
- BaCO₃: 1 mole
- NaCl: 2 moles
Definition of molarity
Molarity is a measure of the concentration of a solute in a solution and indicates the number of moles of solute that are dissolved in a given volume.
The molarity of a solution is calculated by:
molarity= number of moles÷ volume
Amount of reagent in this case
In first place, you know:
- Molarity of BaCl₂= 0.500 M
- Number of moles of BaCl₂= ?
- Volume of BaCl₂= 25 mL= 0.025 L (being 1000 mL= 1 L)
- Molarity of Na₂CO₃= 0.500 M
- Number of moles of Na₂CO₃= ?
- Volume of Na₂CO₃= 25 mL= 0.025 L (being 1000 mL= 1 L)
Replacing in the definition of molarity:
0.500 M= number of moles of Na₂CO₃÷ 0.025 L
Solving:
number of moles of Na₂CO₃= 0.500 M× 0.025 L
number of moles of Na₂CO₃= 0.0125 moles
0.500 M= number of moles of BaCl₂÷ 0.025 L
Solving:
number of moles of BaCl₂= 0.500 M× 0.025 L
number of moles of BaCl₂= 0.0125 moles
This indicates that 0.0125 mol of Na₂CO₃ and 0.0125 mol of BaCl₂ are present.
Since the stoichiometric ratio of the reactants is 1:1, if 0.0125 mol of Na₂CO₃ and BaCl₂ are present, since the amounts are equal, it makes no difference to work with any of the reactants.
Percent yield
The percent yield is the ratio of the actual return to the theoretical return expressed as a percentage.
The percent yield is calculated as the experimental yield divided by the theoretical yield multiplied by 100%:
percent yield= (actual yield÷ theoretical yield)×100%
where the theoretical yield is the amount of product acquired through the complete conversion of all reagents in the final product, that is, it is the maximum amount of product that could be formed from the given amounts of reagents.
Theoretical yield of BaCO₃
The following rule of three can be applied: if by reaction stoichiometry 1 mole of BaCl₂ form 1 mole of BaCO₃, 0.0125 moles of BaCl₂ form how many moles of BaCO₃?
moles of BaCO₃= (0.0125 moles of BaCl₂×1 mole of BaCO₃)÷ 1 mole of BaCl₂
moles of BaCO₃= 0.0125 moles
Being the molar mass of BaCO₃ 197.35 g/mole, the theoretical yield of BaCO₃ is calculated as:
theoretical yield of BaCO₃= 0.0125 moles× 197.35 g/mole
theoretical yield of BaCO₃= 2.466875 grams
Percent yield for the reaction in this case
In this case, you know:
- actual yield= 2 grams
- theorical yield= 2.466875 grams
Replacing in the definition of percent yield:
percent yield= (2 grams÷ 2.466875 grams)× 100 %
Solving:
percent yield= 81.07%
Finally, the percent yield for the reaction is 81.07%.
Learn more about the reaction stoichiometry:
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