To find the actual yield, we need to first calculate the theoretical yield using stoichiometric calculations.
From the balanced chemical equation, we can see that 2 moles of sodium react with 1 mole of chlorine gas to produce 2 moles of sodium chloride.
1 mole of sodium has a molar mass of 22.99 g.
Therefore, 57.50 g of sodium is equal to 57.50 g / 22.99 g/mole = 2.50 moles of sodium.
Since the reaction is 2 moles of sodium to 2 moles of sodium chloride, we can deduce that 2.50 moles of sodium will produce 2.50 moles of sodium chloride.
The molar mass of sodium chloride is 58.44 g/mole.
Therefore, the theoretical yield of sodium chloride is 2.50 moles x 58.44 g/mole = 146.10 g.
Now, to find the actual yield, we can use the formula for percentage yield:
percentage yield = (actual yield / theoretical yield) x 100
Rearranging the formula to solve for the actual yield:
actual yield = (percentage yield / 100) x theoretical yield
actual yield = (86 / 100) x 146.10 g
actual yield = 0.86 x 146.10 g
actual yield = 125.67 g
Therefore, the actual yield of sodium chloride is 125.67 grams.
A chemist reacted 57.50 grams of sodium metal with an excess amount of chlorine gas. The chemical reaction that occurred is shown.
2Na + Cl2 → 2NaCl
If the percentage yield of the reaction is 86%, what is the actual yield? Show your work, including the use of stoichiometric calculations and conversion factors.
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